[Joniaguis]

I need some assistance over the following question. I don't know exactly which equation I have to use.

Determine the entropy change when one mole of a liquid (bpt 356K) is heated from 298K up to 428K given the following information:

Cp of liquid: 45 cal/mole/degree
Cp of vapour: 10.8 + 3.35 x 10^-2 T + 0.95 x 10^-4 T² cal/mole/degree
heat of vapourisation: 4405 cal/mole

[o0CY0o]

I need some assistance over the following question. I don't know exactly which equation I have to use.

Determine the entropy change when one mole of a liquid (bpt 356K) is heated from 298K up to 428K given the following information:

Cp of liquid: 45 cal/mole/degree
Cp of vapour: 10.8 + 3.35 x 10^-2 T + 0.95 x 10^-4 T² cal/mole/degree
heat of vapourisation: 4405 cal/mole

For this question, we need to consider 3 steps.
one the entropy change for liquid form 298K to 356K. 2nd the entropy for phase change. 3rd entropy change of gas phase from 356K to 428K


1.  :delta:S= 45 ln (356/298)
2.  :delta:S= :delta:H/T  = 4405/356
3.   :delta:S= intergrate C/T with respect to T for upper limit is 428 and lower limit is 356 where C is taken as 10.8 + 3.35 x 10^-2 T + 0.95 x 10^-4 T² cal/mole/degree.