Thermodynamics B/C

[CPScienceDude]

Reboot time?

[Justin72835]

Let's start this back up again.

A plastic cup of negligible heat capacity is filled with 300 grams of ice at a temperature of -10 degrees Celsius. The cup is then placed in a large room at a temperature of 23 degrees Celsius. After a significant amount of time, the ice inside the cup is completely melted and the water reaches the same temperature of the room. Assume that the room is large enough that its temperature does not change.

What is the total change entropy of the ice/water?

Use these values when calculating your answer (Click to Show Hidden Text)

specific heat of ice = 2.108 J/g*K
heat of fusion = 334 J/g
specific heat of water = 4.184 J/g*K

Hint (Click to Show Hidden Text)

Treat the entire process as three separate processes (the ice warming up to its freezing point, the ice melting, and the water warming up to 23 degrees Celsius). Then you can calculate the change in entropy for each process and add them up to get the final answer.

[Carpenter]

Let's start this back up again.

A plastic cup of negligible heat capacity is filled with 300 grams of ice at a temperature of -10 degrees Celsius. The cup is then placed in a large room at a temperature of 23 degrees Celsius. After a significant amount of time, the ice inside the cup is completely melted and the water reaches the same temperature of the room. Assume that the room is large enough that its temperature does not change.

What is the total change entropy of the ice/water?

Use these values when calculating your answer (Click to Show Hidden Text)

specific heat of ice = 2.108 J/g*K
heat of fusion = 334 J/g
specific heat of water = 4.184 J/g*K

Hint (Click to Show Hidden Text)

Treat the entire process as three separate processes (the ice warming up to its freezing point, the ice melting, and the water warming up to 23 degrees Celsius). Then you can calculate the change in entropy for each process and add them up to get the final answer.

Not to be that guy, but I'm pretty sure this question requires calculus. I don't think this question should be showing up here or on any tests at invitationals.

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

Let's start this back up again.

A plastic cup of negligible heat capacity is filled with 300 grams of ice at a temperature of -10 degrees Celsius. The cup is then placed in a large room at a temperature of 23 degrees Celsius. After a significant amount of time, the ice inside the cup is completely melted and the water reaches the same temperature of the room. Assume that the room is large enough that its temperature does not change.

What is the total change entropy of the ice/water?

Use these values when calculating your answer (Click to Show Hidden Text)

specific heat of ice = 2.108 J/g*K
heat of fusion = 334 J/g
specific heat of water = 4.184 J/g*K

Hint (Click to Show Hidden Text)

Treat the entire process as three separate processes (the ice warming up to its freezing point, the ice melting, and the water warming up to 23 degrees Celsius). Then you can calculate the change in entropy for each process and add them up to get the final answer.

Not to be that guy, but I'm pretty sure this question requires calculus. I don't think this question should be showing up here or on any tests at invitationals.

Click to Show Answer

Now, using Wolfram Alpha or a sufficiently smart calculator to compute the integrals and sum everything together, I get .

[blueflannel27]

Let's start this back up again.

A plastic cup of negligible heat capacity is filled with 300 grams of ice at a temperature of -10 degrees Celsius. The cup is then placed in a large room at a temperature of 23 degrees Celsius. After a significant amount of time, the ice inside the cup is completely melted and the water reaches the same temperature of the room. Assume that the room is large enough that its temperature does not change.

What is the total change entropy of the ice/water?

Use these values when calculating your answer (Click to Show Hidden Text)

specific heat of ice = 2.108 J/g*K
heat of fusion = 334 J/g
specific heat of water = 4.184 J/g*K

Hint (Click to Show Hidden Text)

Treat the entire process as three separate processes (the ice warming up to its freezing point, the ice melting, and the water warming up to 23 degrees Celsius). Then you can calculate the change in entropy for each process and add them up to get the final answer.

Not to be that guy, but I'm pretty sure this question requires calculus. I don't think this question should be showing up here or on any tests at invitationals.

Click to Show Answer

Now, using Wolfram Alpha or a sufficiently smart calculator to compute the integrals and sum everything together, I get .

Correct me if I'm wrong, but shouldn't the entropy for the melting process be this instead?

[Things2do]

Not to be that guy, but I'm pretty sure this question requires calculus. I don't think this question should be showing up here or on any tests at invitationals.

Click to Show Answer

Now, using Wolfram Alpha or a sufficiently smart calculator to compute the integrals and sum everything together, I get .

Correct me if I'm wrong, but shouldn't the entropy for the melting process be this instead?

Click to Show Answer

Have you heard of the hide functions?

Code: Select all

[hide]title|hidden[/hide]
[spoiler]Hidden[/spoiler]
And
[Answer]hidden[/answer]

title (Click to Show Hidden Text)

hidden

Hidden

Click to Show Answer

hidden

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

Not to be that guy, but I'm pretty sure this question requires calculus. I don't think this question should be showing up here or on any tests at invitationals.

Click to Show Answer

Now, using Wolfram Alpha or a sufficiently smart calculator to compute the integrals and sum everything together, I get .

Correct me if I'm wrong, but shouldn't the entropy for the melting process be this instead?

Yes, that's right. As my physics teacher says, I was just testing to see if you were paying attention.

The corrected answer should be (Click to Show Hidden Text)

[math]\boxed{491.90\ \frac{\textrm{J}}{\textrm{K}}}[/math].

What do the triple point and critical point mean on a phase diagram? Why is the phase diagram of water special?

[Justin72835]

Click to Show Answer

Now, using Wolfram Alpha or a sufficiently smart calculator to compute the integrals and sum everything together, I get .

Correct me if I'm wrong, but shouldn't the entropy for the melting process be this instead?

Yes, that's right. As my physics teacher says, I was just testing to see if you were paying attention.

The corrected answer should be (Click to Show Hidden Text)

[math]\boxed{491.90\ \frac{\textrm{J}}{\textrm{K}}}[/math].

What do the triple point and critical point mean on a phase diagram? Why is the phase diagram of water special?

Yup, you got it. Someone else can answer UTF's next question.

[JoeyC]

The triple point is where a material can be a solid, liquid, and gas all at once. The critical point is where the boundary between liquid and vapor ceases to exist.

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

The triple point is where a material can be a solid, liquid, and gas all at once. The critical point is where the boundary between liquid and vapor ceases to exist.

Okay yes, but For the triple point, I would word it more clearly as where the solid, liquid, and gas phases coexist because a single object cannot be all three of them at the same time. Technically, critical point refers to any end point of a phase equilibrium curve, not just the one between liquids and vapors. Some possible answers for why the water phase diagram is special: Ice has a high number of phases (18 or more according to Wikipedia) Water expands when it is cooled below 4 degrees Celsius, so the boundary between liquid water and ice goes to the left as pressure increases above atmospheric pressure instead of to the right. Your turn!