Physics Book - User contributions [en]

Energy Transfer due to a Temperature Difference

2015-11-10T17:39:57Z

Wpark39:

This section will be sharing how to calculate energy transfer in systems that are affected by temperature changes. This related to Chapter 7 in the Text Book and Exam 3.

Woong Jun Park<br>
wpark39

==The Main Idea==

When hot and cold objects are placed into contact with one another, there is a transfer of energy from the hot to the cold object. This is not your typical energy transfer as "work", but rather it is called Q.

<b>Q = Energy Transfer Due to a Temperature Difference<br></b>
<b>delta(E) = Q + W</b>

Like Work (W), Q can be negative because there could be a transfer of energy out of the system rather than it coming into the system (this can happen if the system has a higher temperature than its surroundings).

In the following, we will cover examples and more functionalities of how this Energy Transfer works.

===A Mathematical Model===

The following are mathematical models that you will use in these calculations:

*<b>The Energy Principle</b>
*delta(E_system) = W + Q + other energy transfers

*Q = mC(deltaT)
Q = Heat Added
m = mass
C = Specific Heat
deltaT = change in Temperature

===A Computational Model===

Check this video out for a brief understanding of how Heat & Temperature relate to Physics. <br>
[https://www.youtube.com/embed/bODiX2PjCPE Heat Transfer]

Check this video out for a detailed look into the topic.<br>
[https://www.youtube.com/embed/XmXr58ySUhI Relationship between deltaE and Q+W]

==Examples==
<b>Example 1:</b>
How much heat energy is required to raise the temperature of 55.0g of water from 25° C to 28.6° C? <br>

Q=mCdeltatT<br>
Q=55g*4.2J/g/K*(28.6° C-25° C)<br>
Q=827.64J<br>

<b>Example 2:</b>
180 grams of boiling water (temperature 100° C, heat capacity 4.2 J/gram/K) are poured into an aluminum pan whose mass is 800 grams and initial temperature 24° C (the heat capacity of aluminum is 0.9 J/gram/K).<br>

After a short time, what is the temperature of the water?<br>

System: Water+Pan<br>
Q = mC(deltaT)<br>
180g*4.2(J/g/K)*(100-T) = 800g*0.9(J/g/K)*(T-22)<br>
T=61.95° C <br>

*In this case, you would assume that the heat capacities for both water and aluminum don't really change with temperature. And also assume the energy transfer between the system and the surroundings was negligible. <br>

<b>Example 3:</b>
Suppose you warm up 510 grams of water (about half a liter, or about a pint) on a stove, and while this is happening, you also stir the water with a beater, doing 6104 J of work on the water. After the large-scale motion of the water has dissipated away, the temperature of the water is observed to have risen from 23°C to 82°C.<br>
A) What was the change in the thermal energy of the water?<br>
deltatE = mCdeltaT<br>
510g*4.2(J/g/K)(82-23)<br>
deltatE = 126378 J<br>
<br>
B) Taking the water as the system, how much energy transfer due to a temperature difference (microscopic work) Q was there across the system boundary?<br>
Q = E-W<br>
126378J - 6e4J<br>
Q = 66378J<br>
<br>
C) Taking the water as the system, what was the energy change of the surroundings? <br>
deltaE_system = - deltaE_surroundings<br>
deltaE_surroundings = -126378<br>

==Connectedness==

I am a Business, Pre-Dental student so health topics have always been very interesting to me. Although this topic may not relate directly to my major, it does have real world applications in the health field.

Specific heat and this transfer of energy can be applied to taking patient's temperatures using a thermometer. There is liquid and material that is inside the thermometer that a have low specific capacities. This allows for a very precise measurement of the temperature. This is not necessarily

Another industrial application can e seen in engine parts that expand and contract because of the constant change in heat within the engine.

==History==

The history of heat and work can be dated back to 1789 when the French scientist Antoine Lavoisier created a new theory - the <i>phlogiston theory</i> on Chemistry that basically negated all previous findings of combustion. He gave heat a meaning and definition that led to the interpretation of heat that is accepted today.

The modern interpretation is what we hold true in the example questions that we used earlier Q = mCdeltatT.

In 1798, Benjamin Thompson - minister for war and police in the German state of Bavaria - wanted to figure out where all the heat from the cannons were coming from. He observed that the surroundings of the cannon got hotter and not colder. He hypothesized that some of the mechanical work done on the cannon was converted to heat.

In 1849, English physicist James Prescott Joule published his work and findings on the conversion of work to heat that Thompson started. He formulated <i>work equivalent of heat.</i> 1 newton meter of work = 0.241 calories of heat.

In 1850, German physicist Clausius published his works on how conserved quantity is neither heat nor work, but a combination of both. He named this Energy and that is where we get the macroscopic equation deltaE = Q - W.

== See also ==

Relevant material and additional reading can be looked into the history of Joule and the laws of thermodynamics.

===Further reading===
[http://www.britannica.com/science/specific-heat Specific Heat: Britannica]<br>
[http://www.nature.com/nature/journal/v181/n4609/abs/181642a0.html Dependence of Heat Capacity on Thermal History: Nature Publishing Group]<br>
[http://environmentalresearchweb.org/cws/article/news/51788 Environmental Research Web | Uneven Climate Change Due to Atmospheric Heat Capacity]

===External links===
[http://water.usgs.gov/edu/heat-capacity.html USGS Water Science School]<br>
[http://www.sciencedirect.com/science/article/pii/S2095263513000630 Science Direct | Determination of specific heat capacity by transient plane source]<br>
[https://www.youtube.com/embed/bODiX2PjCPE Heat Transfer]<br>
[https://www.youtube.com/embed/XmXr58ySUhI Relationship between deltaE and Q+W]<br>

==References==

"A Brief History of Heat and Work." A Brief History of Heat and Work. N.p., n.d. Web. 10 Nov. 2015.\

"Application of Specific Heat Capacity" : Application of Specific Heat Capacity. N.p., n.d. Web. 10 Nov. 2015.

"CHAPTER 4: HEAT." : 4.2 Specific Heat Capacity. N.p., n.d. Web. 10 Nov. 2015.

Division of Building Technology, Chalmers University of Technology, Gothenburg SE-412 96, Sweden
Received 23 August 2013, Revised 3 September 2013, Accepted 10 September 2013, Available online 22 October 2013

"Re: What Are Some Practical Uses of Determining the Specific Heat of a Metal?" Re: What Are Some Practical Uses of Determining the Specific Heat of a Metal? N.p., n.d. Web. 10 Nov. 2015.

[[Category:Energy]]

Energy Transfer due to a Temperature Difference

2015-11-10T17:36:14Z

Wpark39:

This section will be sharing how to calculate energy transfer in systems that are affected by temperature changes. This related to Chapter 7 in the Text Book and Exam 3.

Woong Jun Park<br>
wpark39

==The Main Idea==

When hot and cold objects are placed into contact with one another, there is a transfer of energy from the hot to the cold object. This is not your typical energy transfer as "work", but rather it is called Q.

<b>Q = Energy Transfer Due to a Temperature Difference<br></b>
<b>delta(E) = Q + W</b>

Like Work (W), Q can be negative because there could be a transfer of energy out of the system rather than it coming into the system (this can happen if the system has a higher temperature than its surroundings).

In the following, we will cover examples and more functionalities of how this Energy Transfer works.

===A Mathematical Model===

The following are mathematical models that you will use in these calculations:

<b>The Energy Principle</b>
delta(E_system) = W + Q + other energy transfers

<b>Q</b>
Q = mC(deltaT)
Q = Heat Added
m = mass
C = Specific Heat
deltaT = change in Temperature

===A Computational Model===

Check this video out for a brief understanding of how Heat & Temperature relate to Physics. <br>
[https://www.youtube.com/embed/bODiX2PjCPE Heat Transfer]

Check this video out for a detailed look into the topic.<br>
[https://www.youtube.com/embed/XmXr58ySUhI Relationship between deltaE and Q+W]

==Examples==
<b>Example 1:</b>
How much heat energy is required to raise the temperature of 55.0g of water from 25° C to 28.6° C? <br>

Q=mCdeltatT<br>
Q=55g*4.2J/g/K*(28.6° C-25° C)<br>
Q=827.64J<br>

<b>Example 2:</b>
180 grams of boiling water (temperature 100° C, heat capacity 4.2 J/gram/K) are poured into an aluminum pan whose mass is 800 grams and initial temperature 24° C (the heat capacity of aluminum is 0.9 J/gram/K).<br>

After a short time, what is the temperature of the water?<br>

System: Water+Pan<br>
Q = mC(deltaT)<br>
180g*4.2(J/g/K)*(100-T) = 800g*0.9(J/g/K)*(T-22)<br>
T=61.95° C <br>

*In this case, you would assume that the heat capacities for both water and aluminum don't really change with temperature. And also assume the energy transfer between the system and the surroundings was negligible. <br>

<b>Example 3:</b>
Suppose you warm up 510 grams of water (about half a liter, or about a pint) on a stove, and while this is happening, you also stir the water with a beater, doing 6104 J of work on the water. After the large-scale motion of the water has dissipated away, the temperature of the water is observed to have risen from 23°C to 82°C.<br>
A) What was the change in the thermal energy of the water?<br>
deltatE = mCdeltaT<br>
510g*4.2(J/g/K)(82-23)<br>
deltatE = 126378 J<br>
<br>
B) Taking the water as the system, how much energy transfer due to a temperature difference (microscopic work) Q was there across the system boundary?<br>
Q = E-W<br>
126378J - 6e4J<br>
Q = 66378J<br>
<br>
C) Taking the water as the system, what was the energy change of the surroundings? <br>
deltaE_system = - deltaE_surroundings<br>
deltaE_surroundings = -126378<br>

==Connectedness==

I am a Business, Pre-Dental student so health topics have always been very interesting to me. Although this topic may not relate directly to my major, it does have real world applications in the health field.

Specific heat and this transfer of energy can be applied to taking patient's temperatures using a thermometer. There is liquid and material that is inside the thermometer that a have low specific capacities. This allows for a very precise measurement of the temperature. This is not necessarily

Another industrial application can e seen in engine parts that expand and contract because of the constant change in heat within the engine.

==History==

The history of heat and work can be dated back to 1789 when the French scientist Antoine Lavoisier created a new theory - the <i>phlogiston theory</i> on Chemistry that basically negated all previous findings of combustion. He gave heat a meaning and definition that led to the interpretation of heat that is accepted today.

The modern interpretation is what we hold true in the example questions that we used earlier Q = mCdeltatT.

In 1798, Benjamin Thompson - minister for war and police in the German state of Bavaria - wanted to figure out where all the heat from the cannons were coming from. He observed that the surroundings of the cannon got hotter and not colder. He hypothesized that some of the mechanical work done on the cannon was converted to heat.

In 1849, English physicist James Prescott Joule published his work and findings on the conversion of work to heat that Thompson started. He formulated <i>work equivalent of heat.</i> 1 newton meter of work = 0.241 calories of heat.

In 1850, German physicist Clausius published his works on how conserved quantity is neither heat nor work, but a combination of both. He named this Energy and that is where we get the macroscopic equation deltaE = Q - W.

== See also ==

Relevant material and additional reading can be looked into the history of Joule and the laws of thermodynamics.

===Further reading===
[http://www.britannica.com/science/specific-heat Specific Heat: Britannica]<br>
[http://www.nature.com/nature/journal/v181/n4609/abs/181642a0.html Dependence of Heat Capacity on Thermal History: Nature Publishing Group]<br>
[http://environmentalresearchweb.org/cws/article/news/51788 Environmental Research Web | Uneven Climate Change Due to Atmospheric Heat Capacity]

===External links===
[http://water.usgs.gov/edu/heat-capacity.html USGS Water Science School]<br>
[http://www.sciencedirect.com/science/article/pii/S2095263513000630 Science Direct | Determination of specific heat capacity by transient plane source]

==References==

"A Brief History of Heat and Work." A Brief History of Heat and Work. N.p., n.d. Web. 10 Nov. 2015.\

"Application of Specific Heat Capacity" : Application of Specific Heat Capacity. N.p., n.d. Web. 10 Nov. 2015.

"CHAPTER 4: HEAT." : 4.2 Specific Heat Capacity. N.p., n.d. Web. 10 Nov. 2015.

Division of Building Technology, Chalmers University of Technology, Gothenburg SE-412 96, Sweden
Received 23 August 2013, Revised 3 September 2013, Accepted 10 September 2013, Available online 22 October 2013

"Re: What Are Some Practical Uses of Determining the Specific Heat of a Metal?" Re: What Are Some Practical Uses of Determining the Specific Heat of a Metal? N.p., n.d. Web. 10 Nov. 2015.

[[Category:Energy]]

Energy Transfer due to a Temperature Difference

2015-11-10T17:34:37Z

Wpark39:

This section will be sharing how to calculate energy transfer in systems that are affected by temperature changes. This related to Chapter 7 in the Text Book and Exam 3.

Woong Jun Park<br>
wpark39

==The Main Idea==

When hot and cold objects are placed into contact with one another, there is a transfer of energy from the hot to the cold object. This is not your typical energy transfer as "work", but rather it is called Q.

<b>Q = Energy Transfer Due to a Temperature Difference'''<br></b>
<b>delta(E) = Q + W</b>

Like Work (W), Q can be negative because there could be a transfer of energy out of the system rather than it coming into the system (this can happen if the system has a higher temperature than its surroundings).

In the following, we will cover examples and more functionalities of how this Energy Transfer works.

===A Mathematical Model===

The following are mathematical models that you will use in these calculations:

<b>The Energy Principle</b>
delta(E_system) = W + Q + other energy transfers

<b>Q</b>
Q = mC(deltaT)
Q = Heat Added
m = mass
C = Specific Heat
deltaT = change in Temperature

===A Computational Model===

Check this video out for a brief understanding of how Heat & Temperature relate to Physics. <br>
[https://www.youtube.com/embed/bODiX2PjCPE Heat Transfer]

Check this video out for a detailed look into the topic.<br>
[https://www.youtube.com/embed/XmXr58ySUhI Relationship between deltaE and Q+W]

==Examples==
<b>Example 1:</b>
How much heat energy is required to raise the temperature of 55.0g of water from 25° C to 28.6° C? <br>

Q=mCdeltatT<br>
Q=55g*4.2J/g/K*(28.6° C-25° C)<br>
Q=827.64J<br>

<b>Example 2:</b>
180 grams of boiling water (temperature 100° C, heat capacity 4.2 J/gram/K) are poured into an aluminum pan whose mass is 800 grams and initial temperature 24° C (the heat capacity of aluminum is 0.9 J/gram/K).<br>

After a short time, what is the temperature of the water?<br>

System: Water+Pan<br>
Q = mC(deltaT)<br>
180g*4.2(J/g/K)*(100-T) = 800g*0.9(J/g/K)*(T-22)<br>
T=61.95° C <br>

*In this case, you would assume that the heat capacities for both water and aluminum don't really change with temperature. And also assume the energy transfer between the system and the surroundings was negligible. <br>

<b>Example 3:</b>
Suppose you warm up 510 grams of water (about half a liter, or about a pint) on a stove, and while this is happening, you also stir the water with a beater, doing 6104 J of work on the water. After the large-scale motion of the water has dissipated away, the temperature of the water is observed to have risen from 23°C to 82°C.<br>
A) What was the change in the thermal energy of the water?<br>
deltatE = mCdeltaT<br>
510g*4.2(J/g/K)(82-23)<br>
deltatE = 126378 J<br>
<br>
B) Taking the water as the system, how much energy transfer due to a temperature difference (microscopic work) Q was there across the system boundary?<br>
Q = E-W<br>
126378J - 6e4J<br>
Q = 66378J<br>
<br>
C) Taking the water as the system, what was the energy change of the surroundings? <br>
deltaE_system = - deltaE_surroundings<br>
deltaE_surroundings = -126378<br>

==Connectedness==

I am a Business, Pre-Dental student so health topics have always been very interesting to me. Although this topic may not relate directly to my major, it does have real world applications in the health field.

Specific heat and this transfer of energy can be applied to taking patient's temperatures using a thermometer. There is liquid and material that is inside the thermometer that a have low specific capacities. This allows for a very precise measurement of the temperature. This is not necessarily

Another industrial application can e seen in engine parts that expand and contract because of the constant change in heat within the engine.

==History==

The history of heat and work can be dated back to 1789 when the French scientist Antoine Lavoisier created a new theory - the <i>phlogiston theory</i> on Chemistry that basically negated all previous findings of combustion. He gave heat a meaning and definition that led to the interpretation of heat that is accepted today.

The modern interpretation is what we hold true in the example questions that we used earlier Q = mCdeltatT.

In 1798, Benjamin Thompson - minister for war and police in the German state of Bavaria - wanted to figure out where all the heat from the cannons were coming from. He observed that the surroundings of the cannon got hotter and not colder. He hypothesized that some of the mechanical work done on the cannon was converted to heat.

In 1849, English physicist James Prescott Joule published his work and findings on the conversion of work to heat that Thompson started. He formulated <i>work equivalent of heat.</i> 1 newton meter of work = 0.241 calories of heat.

In 1850, German physicist Clausius published his works on how conserved quantity is neither heat nor work, but a combination of both. He named this Energy and that is where we get the macroscopic equation deltaE = Q - W.

== See also ==

Relevant material and additional reading can be looked into the history of Joule and the laws of thermodynamics.

===Further reading===
[http://www.britannica.com/science/specific-heat Specific Heat: Britannica]<br>
[http://www.nature.com/nature/journal/v181/n4609/abs/181642a0.html Dependence of Heat Capacity on Thermal History: Nature Publishing Group]<br>
[http://environmentalresearchweb.org/cws/article/news/51788 Environmental Research Web | Uneven Climate Change Due to Atmospheric Heat Capacity]

===External links===
[http://water.usgs.gov/edu/heat-capacity.html USGS Water Science School]<br>
[http://www.sciencedirect.com/science/article/pii/S2095263513000630 Science Direct | Determination of specific heat capacity by transient plane source]

==References==

"A Brief History of Heat and Work." A Brief History of Heat and Work. N.p., n.d. Web. 10 Nov. 2015.\

"Application of Specific Heat Capacity" : Application of Specific Heat Capacity. N.p., n.d. Web. 10 Nov. 2015.

"CHAPTER 4: HEAT." : 4.2 Specific Heat Capacity. N.p., n.d. Web. 10 Nov. 2015.

Division of Building Technology, Chalmers University of Technology, Gothenburg SE-412 96, Sweden
Received 23 August 2013, Revised 3 September 2013, Accepted 10 September 2013, Available online 22 October 2013

"Re: What Are Some Practical Uses of Determining the Specific Heat of a Metal?" Re: What Are Some Practical Uses of Determining the Specific Heat of a Metal? N.p., n.d. Web. 10 Nov. 2015.

[[Category:Energy]]

Energy Transfer due to a Temperature Difference

2015-11-10T17:00:35Z

Wpark39:

This section will be sharing how to calculate energy transfer in systems that are affected by temperature changes. This related to Chapter 7 in the Text Book, Homework Week 10, and Exam 3.

Woong Jun Park
wpark39

==The Main Idea==

When hot and cold objects are placed into contact with one another, there is a transfer of energy from the hot to the cold object. This is not your typical energy transfer as "work", but rather it is called Q.

'''Q = Energy Transfer Due to a Temperature Difference'''<br>
<b>delta(E) = Q + W</b>

Like Work (W), Q can be negative because there could be a transfer of energy out of the system rather than it coming into the system (this can happen if the system has a higher temperature than its surroundings).

In the following, we will cover examples and more functionalities of how this Energy Transfer works.

===A Mathematical Model===

The following are mathematical models that you will use in these calculations:

<b>The Energy Principle</b>
delta(E_system) = W + Q + other energy transfers

<b>Q</b>
Q = mC(deltaT)
Q = Heat Added
m = mass
C = Specific Heat
deltaT = change in Temperature

===A Computational Model===

Check this video out for a brief understanding of how Heat & Temperature relate to Physics. <br>
[https://www.youtube.com/embed/bODiX2PjCPE Heat Transfer]

Check this video out for a detailed look into the topic.<br>
[https://www.youtube.com/embed/XmXr58ySUhI Relationship between deltaE and Q+W]

==Examples==
<b>Example 1:</b>
How much heat energy is required to raise the temperature of 55.0g of water from 25° C to 28.6° C? <br>

Q=mCdeltatT<br>
Q=55g*4.2J/g/K*(28.6° C-25° C)<br>
Q=827.64J<br>

<b>Example 2:</b>
180 grams of boiling water (temperature 100° C, heat capacity 4.2 J/gram/K) are poured into an aluminum pan whose mass is 800 grams and initial temperature 24° C (the heat capacity of aluminum is 0.9 J/gram/K).<br>

After a short time, what is the temperature of the water?<br>

System: Water+Pan<br>
Q = mC(deltaT)<br>
180g*4.2(J/g/K)*(100-T) = 800g*0.9(J/g/K)*(T-22)<br>
T=61.95° C <br>

*In this case, you would assume that the heat capacities for both water and aluminum don't really change with temperature. And also assume the energy transfer between the system and the surroundings was negligible. <br>

<b>Example 3:</b>
Suppose you warm up 510 grams of water (about half a liter, or about a pint) on a stove, and while this is happening, you also stir the water with a beater, doing 6104 J of work on the water. After the large-scale motion of the water has dissipated away, the temperature of the water is observed to have risen from 23°C to 82°C.<br>
A) What was the change in the thermal energy of the water?<br>
deltatE = mCdeltaT<br>
510g*4.2(J/g/K)(82-23)<br>
deltatE = 126378 J<br>
<br>
B) Taking the water as the system, how much energy transfer due to a temperature difference (microscopic work) Q was there across the system boundary?<br>
Q = E-W<br>
126378J - 6e4J<br>
Q = 66378J<br>
<br>
C) Taking the water as the system, what was the energy change of the surroundings? <br>
deltaE_system = - deltaE_surroundings<br>
deltaE_surroundings = -126378<br>

==Connectedness==

I am a Business, Pre-Dental student so health topics have always been very interesting to me. Although this topic may not relate directly to my major, it does have real world applications in the health field.

Specific heat and this transfer of energy can be applied to taking patient's temperatures using a thermometer. There is liquid and material that is inside the thermometer that a have low specific capacities. This allows for a very precise measurement of the temperature. This is not necessarily

Another industrial application can e seen in engine parts that expand and contract because of the constant change in heat within the engine.

==History==

Put this idea in historical context. Give the reader the Who, What, When, Where, and Why.

== See also ==

Are there related topics or categories in this wiki resource for the curious reader to explore? How does this topic fit into that context?

===Further reading===

Books, Articles or other print media on this topic

===External links===

Internet resources on this topic

==References==

Dean, O. (22-06-2008) Application of Specific Heat Retrieved on 10 November 2015 from http://fiziknota.blogspot.com.au/2008/06/application-of-specific-heat-capacity.html

Breen, M. (2001) Re. What are some practical uses of determining the specific heat of a metal. Retrieved on 10 November 2015 from http://www.madsci.org/posts/archives/2001-02/981315429.Rg.r.html

[[Category:Energy]]

Energy Transfer due to a Temperature Difference

2015-11-10T15:55:41Z

Wpark39: Created page with "This section will be sharing how to calculate energy transfer in systems that are affected by temperature changes. This related to Chapter 7 in the Text Book, Homework Week 10..."

This section will be sharing how to calculate energy transfer in systems that are affected by temperature changes. This related to Chapter 7 in the Text Book, Homework Week 10, and Exam 3.

==The Main Idea==

When hot and cold objects are placed into contact with one another, there is a transfer of energy from the hot to the cold object. This is not your typical energy transfer as "work", but rather it is called Q.

'''Q = Energy Transfer Due to a Temperature Difference'''<br>
<b>delta(E) = Q + W</b>

Like Work (W), Q can be negative because there could be a transfer of energy out of the system rather than it coming into the system (this can happen if the system has a higher temperature than its surroundings).

In the following, we will cover examples and more functionalities of how this Energy Transfer works.

===A Mathematical Model===

The following are mathematical models that you will use in these calculations:

<b>The Energy Principle</b>
delta(E_system) = W + Q + other energy transfers

<b>Q</b>
Q = mC(deltaT)
Q = Heat Added
m = mass
C = Specific Heat
deltaT = change in Temperature

===A Computational Model===

Check this video out for a brief understanding of how Heat & Temperature relate to Physics. <br>
[https://www.youtube.com/embed/bODiX2PjCPE Heat Transfer]

Check this video out for a detailed look into the topic.<br>
[https://www.youtube.com/embed/XmXr58ySUhI Relationship between deltaE and Q+W]

==Examples==
<b>Example 1:</b>
How much heat energy is required to raise the temperature of
55.0g of water from 25° C to 28.6° C?

Q=mCdeltatT
Q=55g*4.2J/g/K*(28.6° C-25° C)
Q=827.64J

<b>Example 2:</b>
180 grams of boiling water (temperature 100° C, heat capacity 4.2 J/gram/K) are poured into an aluminum pan whose mass is 800 grams and initial temperature 24° C (the heat capacity of aluminum is 0.9 J/gram/K).

After a short time, what is the temperature of the water?

System: Water+Pan
Q = mC(deltaT)
180g*4.2(J/g/K)*(100-T) = 800g*0.9(J/g/K)*(T-22)
T=61.95° C

*In this case, you would assume that the heat capacities for both water and aluminum don't really change with temperature. And also assume the energy transfer between the system and the surroundings was negligible.

<b>Example 3:</b>
Suppose you warm up 510 grams of water (about half a liter, or about a pint) on a stove, and while this is happening, you also stir the water with a beater, doing 6104 J of work on the water. After the large-scale motion of the water has dissipated away, the temperature of the water is observed to have risen from 23°C to 82°C.
A) What was the change in the thermal energy of the water?

deltatE = mCdeltaT
510g*4.2(J/g/K)(82-23)
deltatE = 126378 J

B) Taking the water as the system, how much energy transfer due to a temperature difference (microscopic work) Q was there across the system boundary?
Q = E-W
126378J - 6e4J
Q = 66378J

C) Taking the water as the system, what was the energy change of the surroundings?
deltaE_system = - deltaE_surroundings
deltaE_surroundings = -126378

<h>

Example 3:
==Connectedness==
#How is this topic connected to something that you are interested in?
#How is it connected to your major?
#Is there an interesting industrial application?

==History==

Put this idea in historical context. Give the reader the Who, What, When, Where, and Why.

== See also ==

Are there related topics or categories in this wiki resource for the curious reader to explore? How does this topic fit into that context?

===Further reading===

Books, Articles or other print media on this topic

===External links===

Internet resources on this topic

==References==

This section contains the the references you used while writing this page

[[Category:Which Category did you place this in?]]

Main Page

2015-11-10T15:14:04Z

Wpark39: /* Energy */

__NOTOC__
Welcome to the Georgia Tech Wiki for Intro Physics. This resources was created so that students can contribute and curate content to help those with limited or no access to a textbook. When reading this website, please correct any errors you may come across. If you read something that isn't clear, please consider revising it!

Looking to make a contribution?
#Pick a specific topic from intro physics
#Add that topic, as a link to a new page, under the appropriate category listed below by editing this page.
#Copy and paste the default [[Template]] into your new page and start editing.

Please remember that this is not a textbook and you are not limited to expressing your ideas with only text and equations. Whenever possible embed: pictures, videos, diagrams, simulations, computational models (e.g. Glowscript), and whatever content you think makes learning physics easier for other students.

== Source Material ==
All of the content added to this resource must be in the public domain or similar free resource. If you are unsure about a source, contact the original author for permission. That said, there is a surprisingly large amount of introductory physics content scattered across the web. Here is an incomplete list of intro physics resources (please update as needed).
* A physics resource written by experts for an expert audience [https://en.wikipedia.org/wiki/Portal:Physics Physics Portal]
* A wiki book on modern physics [https://en.wikibooks.org/wiki/Modern_Physics Modern Physics Wiki]
* The MIT open courseware for intro physics [http://ocw.mit.edu/resources/res-8-002-a-wikitextbook-for-introductory-mechanics-fall-2009/index.htm MITOCW Wiki]
* An online concept map of intro physics [http://hyperphysics.phy-astr.gsu.edu/hbase/hph.html HyperPhysics]
* Interactive physics simulations [https://phet.colorado.edu/en/simulations/category/physics PhET]
* OpenStax algebra based intro physics textbook [https://openstaxcollege.org/textbooks/college-physics College Physics]
* The Open Source Physics project is a collection of online physics resources [http://www.opensourcephysics.org/ OSP]
* A resource guide compiled by the [http://www.aapt.org/ AAPT] for educators [http://www.compadre.org/ ComPADRE]

== Organizing Catagories ==
These are the broad, overarching categories, that we cover in two semester of introductory physics. You can add subcategories or make a new category as needed. A single topic should direct readers to a page in one of these catagories.

<div class="toccolours mw-collapsible mw-collapsed">
===Interactions===
<div class="mw-collapsible-content">
*[[Fundamental Interactions]]
*[[System & Surroundings]]
*[[Newton's First Law of Motion]]

</div>
</div>

<div class="toccolours mw-collapsible mw-collapsed">

===Theory===
<div class="mw-collapsible-content">
*[[Einstein's Theory of Relativity]]
</div>
</div>

<div class="toccolours mw-collapsible mw-collapsed">

===Notable Scientists===
<div class="mw-collapsible-content">
*[[Albert Einstein]]
*[[Ernest Rutherford]]
</div>
</div>
<div class="toccolours mw-collapsible mw-collapsed">

===Properties of Matter===
<div class="mw-collapsible-content">
*[[Mass]]
*[[Charge]]
*[[Spin]]
*[[SI Units]]
</div>
</div>

<div class="toccolours mw-collapsible mw-collapsed">

===Contact Interactions===
<div class="mw-collapsible-content">
* [[Young's Modulus]]
* [[Friction]]
* [[Tension]]
</div>
</div>

<div class="toccolours mw-collapsible mw-collapsed">

===Momentum===
<div class="mw-collapsible-content">
* [[Vectors]]
* [[Kinematics]]
* Predicting Change in one dimension
* [[Predicting Change in multiple dimensions]]
* [[Momentum Principle]]
* [[Curving Motion]]
</div>
</div>

<div class="toccolours mw-collapsible mw-collapsed">

===Angular Momentum===
<div class="mw-collapsible-content">
* [[The Moments of Inertia]]
* [[Rotation]]
* [[Torque]]
* Predicting a Change in Rotation
</div>
</div>

<div class="toccolours mw-collapsible mw-collapsed">

===Energy===
<div class="mw-collapsible-content">
*[[Predicting Change]]
*[[Rest Mass Energy]]
*[[Kinetic Energy]]
*[[Potential Energy]]
*[[Work]]
*[[Thermal Energy]]
*[[Conservation of Energy]]
*[[Electric Potential]]
*[[Energy Transfer due to a Temperature Difference]]
</div>
</div>

<div class="toccolours mw-collapsible mw-collapsed">

===Fields===
<div class="mw-collapsible-content">
* [[Electric Field]] of a
** [[Point Charge]]
** [[Electric Dipole]]
** [[Capacitor]]
** [[Charged Rod]]
** [[Charged Ring]]
** [[Charged Disk]]
** [[Charged Spherical Shell]]
*[[Electric Potential]]
**[[Potential Difference in a Uniform Field]]
*[[Polarization]]
*[[Magnetic Field]]
**[[Direction of Magnetic Field]]
**[[Bar Magnet]]
**[[Magnetic Force]]
**[[Hall Effect]]
**[[Lorentz Force]]
**[[Biot-Savart Law]]
**[[Integration Techniques for Magnetic Field]]
**[[Sparks in Air]]
**[[Motional Emf]]
</div>
</div>

<div class="toccolours mw-collapsible mw-collapsed">

===Simple Circuits===
<div class="mw-collapsible-content">
*[[Components]]
*[[Steady State]]
*[[Non Steady State]]
*[[Node Rule]]
*[[Loop Rule]]
*[[Power in a circuit]]
*[[Ammeters,Voltmeters,Ohmmeters]]
*[[Current]]
*[[Ohm's Law]]
</div>
</div>

<div class="toccolours mw-collapsible mw-collapsed">

===Maxwell's Equations===
<div class="mw-collapsible-content">
*[[Gauss's Flux Theorem]]
**[[Electric Fields]]
**[[Magnetic Fields]]
*[[Faraday's Law]]
**[[Inductance]]
*[[Ampere-Maxwell Law]]
</div>
</div>

<div class="toccolours mw-collapsible mw-collapsed">

===Radiation===
<div class="mw-collapsible-content">
</div>
</div>

== Resources ==
* Commonly used wiki commands [https://en.wikipedia.org/wiki/Help:Cheatsheet Wiki Cheatsheet]
* A guide to representing equations in math mode [https://en.wikipedia.org/wiki/Help:Displaying_a_formula Wiki Math Mode]
* A page to keep track of all the physics [[Constants]]
* An overview of [[VPython]]