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## Main Question or Discussion Point

Hi

Just wondering if I could have a bit of help on this question. Thanks in advance!

3) 100 g of steam at 150_C and 1 kg of water at 20_C are placed together inside

an insulated volume. The specic heat of steam is 2.02x10^3J kg_1K_1, that

of water is 4.19 x10^3 J kg_1K_1 and the latent heat of evaporation of water is

226x10^6 J kg_1.

a) Once the two fluids have come into thermal equilibrium what is left - water or

steam?

b) Calculate the final temperature of the system.

c) Is the net change in the internal energy of the system positive, negative or

zero?

d) Calculate the increase in entropy of the system.

Just wondering if I could have a bit of help on this question. Thanks in advance!

3) 100 g of steam at 150_C and 1 kg of water at 20_C are placed together inside

an insulated volume. The specic heat of steam is 2.02x10^3J kg_1K_1, that

of water is 4.19 x10^3 J kg_1K_1 and the latent heat of evaporation of water is

226x10^6 J kg_1.

a) Once the two fluids have come into thermal equilibrium what is left - water or

steam?

b) Calculate the final temperature of the system.

c) Is the net change in the internal energy of the system positive, negative or

zero?

d) Calculate the increase in entropy of the system.