Thermodynamics B/C

[Justin72835]

Answer (Click to Show Hidden Text)

I'm pretty sure that for this problem you would just use an equation to convert between the two temperatures.

For converting from Kelvin to Réaumur: R = (K - 273.15)*0.8

For converting from Réaumur to Kelvin: K = 1.25R + 273.15

Correct, your turn!

You have a heat refrigerator that requires 1340 W of work. You also find that the refrigerator releases heat into a heat sink at a rate of 4250 W. How much heat can the refrigerator extract from a cold reservoir and what is its coefficient of performance?

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You have a heat refrigerator that requires 1340 W of work. You also find that the refrigerator releases heat into a heat sink at a rate of 4250 W. How much heat can the refrigerator extract from a cold reservoir and what is its coefficient of performance?

Answer (Click to Show Hidden Text)

First Law of Thermodynamics: [math]1340 J + Q_c = 4250 J[/math]. [math]Q_c = 2910 J[/math]. [math]COP = \frac{Q_h}{W} = \frac{4250 J}{1340 J} = 3.17[/math]. [b]2910 W[/b] and [b]3.17[/b]

[Justin72835]

You have a heat refrigerator that requires 1340 W of work. You also find that the refrigerator releases heat into a heat sink at a rate of 4250 W. How much heat can the refrigerator extract from a cold reservoir and what is its coefficient of performance?

Answer (Click to Show Hidden Text)

First Law of Thermodynamics: [math]1340 J + Q_c = 4250 J[/math]. [math]Q_c = 2910 J[/math]. [math]COP = \frac{Q_h}{W} = \frac{4250 J}{1340 J} = 3.17[/math]. [b]2910 W[/b] and [b]3.17[/b]

Overall correct but since we're dealing with a heat refrigerator the formula is actually COP = Qc/W. This is because we are interested in the heat we can extract (Qc) rather than the heat given off at the very end (Qc). Everything is else was good. Your turn!

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A 500. g iron rod at 50. degrees Celsius is dropped into a (very big) beaker filled with 2.0 L of water at 20. degrees Celsius. 80.0% of the heat transferred from the iron rod is lost to the surroundings and is not transferred to the water. Find the power in watts of the transfer of energy into the water if the system reaches thermal equilibrium in exactly one minute.

Use the values of c = 0.50 J/(g*K) for iron and c = 4.0 J/(g*K) for water. Use appropriate significant figures.

[Justin72835]

A 500. g iron rod at 50. degrees Celsius is dropped into a (very big) beaker filled with 2.0 L of water at 20. degrees Celsius. 80.0% of the heat transferred from the iron rod is lost to the surroundings and is not transferred to the water. Find the power in watts of the transfer of energy into the water if the system reaches thermal equilibrium in exactly one minute.

Use the values of c = 0.50 J/(g*K) for iron and c = 4.0 J/(g*K) for water. Use appropriate significant figures.

Answer (Click to Show Hidden Text)

Since the 80% heat lost by the iron rod goes into the surroundings and 20% of it goes into changing the water's temperature, we get the following equation:

[math]Q_{iron}=-(Q_{water}+Q_{surroundings})=-5Q_{water}[/math]

Now we can plug in all our known values to find the equilibrium temperature, then the heat transferred:

[math]m_{iron}c_{iron}(T_f-50)=-5m_{water}c_{water}(T_f-20)[/math] where Tf = 20.1863 degrees Celsius.

Plugging this value back into the equation, you find that the Qiron = 7453.42 J. Dividing this value by 60 gives P = 124 W.

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Answer (Click to Show Hidden Text)

Since the 80% heat lost by the iron rod goes into the surroundings and 20% of it goes into changing the water's temperature, we get the following equation:

[math]Q_{iron}=-(Q_{water}+Q_{surroundings})=-5Q_{water}[/math]

Now we can plug in all our known values to find the equilibrium temperature, then the heat transferred:

[math]m_{iron}c_{iron}(T_f-50)=-5m_{water}c_{water}(T_f-20)[/math] where Tf = 20.1863 degrees Celsius.

Plugging this value back into the equation, you find that the Qiron = 7453.42 J. Dividing this value by 60 gives P = 124 W.

Yes, except transfer of heat into the water and not out of the rod and also only two sigfigs. Your turn!

[Justin72835]

Yes, except transfer of heat into the water and not out of the rod and also only two sigfigs. Your turn!

You fill a container with 3.5 L of water at an initial temperature of 90 °C. After 1 hour of cooling, you measure the temperature the temperature of the water to have dropped to 65 °C. Lastly, the surrounding temperature of the container remained at a steady 24 °C throughout the entire cooling process. Calculate the change in entropy for the entire system (including both the water and the surroundings).

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Yes, except transfer of heat into the water and not out of the rod and also only two sigfigs. Your turn!

You fill a container with 3.5 L of water at an initial temperature of 90 °C. After 1 hour of cooling, you measure the temperature the temperature of the water to have dropped to 65 °C. Lastly, the surrounding temperature of the container remained at a steady 24 °C throughout the entire cooling process. Calculate the change in entropy for the entire system (including both the water and the surroundings).

Answer (Click to Show Hidden Text)

[math]\frac{Q}{\Delta T} = 3.5 L * 1 kg/L * 4180 J/(kg*K) = 14630 J/K[/math]

[math]Q = 14630 J/K * 25 K = 365750 J[/math]

[math]\Delta T(Q) = \frac{Q}{14360 J/K}[/math]

[math]T(Q) = 363.15 K + \frac{Q}{14360 J/K}[/math]

[math]\Delta S_{total} = \Delta S_{surroundings} + \Delta S_{water} = \frac{365750 J}{297.15 K} - \int^{365750 J}_{0 J} \frac{dQ}{T(Q)}[/math]

[math]\Delta S_{total} = 1230.856 J/K - 973.409 J/K = 257.45 J/K \approx 260 J/K[/math]

With special thanks to WolframAlpha.

P.S. is there a better way to format the equations than having a separate tag every line?

[Justin72835]

Answer (Click to Show Hidden Text)

[math]\frac{Q}{\Delta T} = 3.5 L * 1 kg/L * 4180 J/(kg*K) = 14630 J/K[/math]

[math]Q = 14630 J/K * 25 K = 365750 J[/math]

[math]\Delta T(Q) = \frac{Q}{14360 J/K}[/math]

[math]T(Q) = 363.15 K + \frac{Q}{14360 J/K}[/math]

[math]\Delta S_{total} = \Delta S_{surroundings} + \Delta S_{water} = \frac{365750 J}{297.15 K} - \int^{365750 J}_{0 J} \frac{dQ}{T(Q)}[/math]

[math]\Delta S_{total} = 1230.856 J/K - 973.409 J/K = 257.45 J/K \approx 260 J/K[/math]

With special thanks to WolframAlpha.

P.S. is there a better way to format the equations than having a separate tag ---- every line?

Hmm I got 187 J/K as my answer when I did it. I think the fourth line should be



with a minus instead of a plus. If it were plus, then you would see your temperature increasing (since Q is always positive) instead of decreasing. I redid your work with this correction and I got the same answer. What do you think?

Also, we'll have to make do with putting the math tag before every equation

[UTF-8 U+6211 U+662F]

Hmm I got 187 J/K as my answer when I did it. I think the fourth line should be



with a minus instead of a plus. If it were plus, then you would see your temperature increasing (since Q is always positive) instead of decreasing. I redid your work with this correction and I got the same answer. What do you think?

Yeah, that's my bad.

Revised Answer (Click to Show Hidden Text)

[math]\frac{Q}{\Delta T} = 3.5 L * 1 kg/L * 4180 J/(kg*K) = 14630 J/K[/math]

[math]Q_f = 14630 J/K * 25 K = 365750 J[/math]

[math]\Delta T(Q) = -\frac{Q}{14360 J/K}[/math]

[math]T(Q) = 363.15 K - \frac{Q}{14360 J/K}[/math]

[math]\Delta S_{total} = \Delta S_{surroundings} + \Delta S_{water} = \frac{365750 J}{297.15 K} - \int^{365750 J}_{0 J} \frac{dQ}{T(Q)}[/math]

[math]\Delta S_{total} = 1230.856 J/K - 1044.22 J/K = 186.634 J/K \approx 190 J/K[/math]

EDIT: Oh yeah, next question. An 10g iron rod at 50 degrees Celsius is dropped into a 1L beaker of water at 60 degrees Celsius. How does the length of the rod change? Use the values of c = 0.50 J/(g*K) for iron and c = 4.0 J/(g*K) for water. Use as many sigfigs as you want.