Thermodynamics B/C

[MattChina]

Properties or quantities that depend on the path taken from the initial state to the final state are called _________?

Answer (Click to Show Hidden Text)

Path or path-dependent functions

correct. Your turn.

[Justin72835]

Since nobody has posted in the last couple of days:

A double-pane window consists of two glass sheets, each with dimensions of 75 cm x 75 cm x 0.6 cm, separated by a 0.4 cm stagnant air space. The indoor surface temperature is 25 degrees Celcius, while the outdoor surface temperature is 0 degrees Celsius. What is the rate of heat flow through the window in calories per second?

k=2E-3 cal/s*cm*C for glass and 2E-4 cal/s*cm*C for air.

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

Since nobody has posted in the last couple of days:

A double-pane window consists of two glass sheets, each with dimensions of 75 cm x 75 cm x 0.6 cm, separated by a 0.4 cm stagnant air space. The indoor surface temperature is 25 degrees Celcius, while the outdoor surface temperature is 0 degrees Celsius. What is the rate of heat flow through the window in calories per second?

k=2E-3 cal/s*cm*C for glass and 2E-4 cal/s*cm*C for air.

Answer (Click to Show Hidden Text)

[math]R_{total} = R_1 + R_2 + R_3 = \frac{0.6 cm}{2*10^{-3} \frac{cal}{s*cm*\degree C}} + \frac{0.4 cm}{2*10^{-4} \frac{cal}{s*cm*\degree C}} + \frac{0.6 cm}{2*10^{-3} \frac{cal}{s*cm*\degree C}} = 2600 \frac{s*cm^2*\degree C}{cal}[/math]

[math]W = \frac{kA \Delta T}{d} = \frac{A\Delta T}{R} = \frac{75 cm * 75 cm * 25 \degree C}{2600 \frac{s*cm^2*\degree C}{cal}} = 54 \frac{cal}{s}[/math] (or 5E1 if you want to use proper sigfigs).

[Justin72835]

Since nobody has posted in the last couple of days:

A double-pane window consists of two glass sheets, each with dimensions of 75 cm x 75 cm x 0.6 cm, separated by a 0.4 cm stagnant air space. The indoor surface temperature is 25 degrees Celcius, while the outdoor surface temperature is 0 degrees Celsius. What is the rate of heat flow through the window in calories per second?

k=2E-3 cal/s*cm*C for glass and 2E-4 cal/s*cm*C for air.

Answer (Click to Show Hidden Text)

[math]R_{total} = R_1 + R_2 + R_3 = \frac{0.6 cm}{2*10^{-3} \frac{cal}{s*cm*\degree C}} + \frac{0.4 cm}{2*10^{-4} \frac{cal}{s*cm*\degree C}} + \frac{0.6 cm}{2*10^{-3} \frac{cal}{s*cm*\degree C}} = 2600 \frac{s*cm^2*\degree C}{cal}[/math]

[math]W = \frac{kA \Delta T}{d} = \frac{A\Delta T}{R} = \frac{75 cm * 75 cm * 25 \degree C}{2600 \frac{s*cm^2*\degree C}{cal}} = 54 \frac{cal}{s}[/math] (or 5E1 if you want to use proper sigfigs).

Great job; you're next!

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

Fill in the blank (assume all other factors are the same). Explain why using the statistical definition of entropy.
1) A gas with more volume has _ entropy than a gas with less volume.
2) A hotter gas has _ entropy than a colder gas.
3) A mole of multiple gases has _ entropy than a mole of a single gas (Bonus: what is this increase in entropy called?).
4) a diatomic gas has _ entropy than a monatomic gas.

[MattChina]

Fill in the blank (assume all other factors are the same). Explain why using the statistical definition of entropy.
1) A gas with more volume has _ entropy than a gas with less volume.
2) A hotter gas has _ entropy than a colder gas.
3) A mole of multiple gases has _ entropy than a mole of a single gas (Bonus: what is this increase in entropy called?).
4) a diatomic gas has _ entropy than a monatomic gas.

1.more
2.more
3.more
4.more

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

Fill in the blank (assume all other factors are the same). Explain why using the statistical definition of entropy.
1) A gas with more volume has _ entropy than a gas with less volume.
2) A hotter gas has _ entropy than a colder gas.
3) A mole of multiple gases has _ entropy than a mole of a single gas (Bonus: what is this increase in entropy called?).
4) a diatomic gas has _ entropy than a monatomic gas.

1.more
2.more
3.more
4.more

I believe you missed the essential part of the question

[BasuSiddha23]

I'm going to go ahead and ask a question:

1) What is the name of the only book Carnot published explaining the theoretical maximum efficiency of heat engines?
2) Which two of the four thermodynamic laws explain properties of entropy? What do these two laws state specifically?
3) Convert 354 degrees Fahrenheit to Rankine

[Justin72835]

Fill in the blank (assume all other factors are the same). Explain why using the statistical definition of entropy.
1) A gas with more volume has _ entropy than a gas with less volume.
2) A hotter gas has _ entropy than a colder gas.
3) A mole of multiple gases has _ entropy than a mole of a single gas (Bonus: what is this increase in entropy called?).
4) a diatomic gas has _ entropy than a monatomic gas.

1.more
2.more
3.more
4.more

I believe you missed the essential part of the question

I'll give it a shot (Click to Show Hidden Text)

1. More. By increasing the volume of the gas, you also increase the number of the microstates of the system by allowing the gas particles to occupy more locations. With more possible states for the gas to obtain, there is more entropy present.

2. More. By increasing the temperature of the gas, you are also increasing the average kinetic energy of the gas particles and thus their rms velocity. With the movements of the gas particles being more erratic and unpredictable at higher temperatures, there are undoubtedly more possible microstates, meaning that the system has a higher entropy.

3. More. WIth a homogenous gas, there are a set number of microstates. Switching any particles around won't create any new microstates because the particles are all identical. However, if instead of a single gas there were multiple gases, switching two gas particles of different species will create new microstates. Thus, the mix of gases has a higher entropy than the homogenous gas. Also, idk what the bonus is :? .

4. More. While monatomic gases only have 3 degrees of freedom (being able to move in the x, y, and z directions), diatomic gases actually have 5 degrees of freedom (being able to move in the x, y, and z directions + vibrational motion + rotational motion). Because of the extra 2 degrees of freedom, the diatomic gas actually has more possible microstates as the molecules can have different orientations and can vibrate differently as well. Therefore, a diatomic gas has more entropy than a monatomic gas.

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

1.more
2.more
3.more
4.more

I believe you missed the essential part of the question

I'll give it a shot (Click to Show Hidden Text)

1. More. By increasing the volume of the gas, you also increase the number of the microstates of the system by allowing the gas particles to occupy more locations. With more possible states for the gas to obtain, there is more entropy present.

2. More. By increasing the temperature of the gas, you are also increasing the average kinetic energy of the gas particles and thus their rms velocity. With the movements of the gas particles being more erratic and unpredictable at higher temperatures, there are undoubtedly more possible microstates, meaning that the system has a higher entropy.

3. More. WIth a homogenous gas, there are a set number of microstates. Switching any particles around won't create any new microstates because the particles are all identical. However, if instead of a single gas there were multiple gases, switching two gas particles of different species will create new microstates. Thus, the mix of gases has a higher entropy than the homogenous gas. Also, idk what the bonus is :? .

4. More. While monatomic gases only have 3 degrees of freedom (being able to move in the x, y, and z directions), diatomic gases actually have 5 degrees of freedom (being able to move in the x, y, and z directions + vibrational motion + rotational motion). Because of the extra 2 degrees of freedom, the diatomic gas actually has more possible microstates as the molecules can have different orientations and can vibrate differently as well. Therefore, a diatomic gas has more entropy than a monatomic gas.

Yep, go ahead!