Question 9.7

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Rohan Chaudhari- 1K
Posts: 32
Joined: Fri Sep 29, 2017 7:06 am

Question 9.7

Postby Rohan Chaudhari- 1K » Thu Jan 25, 2018 9:15 pm

"Assuming that the heat capacity of an ideal gas is independent of temperature, calculate the entropy change associated with raising the temperature of 1.00 mol of ideal gas atoms reversibly from 37.6 C to 157.9 C at a) constant pressure and b) constant volume"

What exactly is the question asking me to do and which equations are you supposed to use for this?

Jeremiah Samaniego 2C
Posts: 33
Joined: Fri Sep 29, 2017 7:05 am

Re: Question 9.7

Postby Jeremiah Samaniego 2C » Thu Jan 25, 2018 9:19 pm

The question wants you to calculate ∆S, or the entropy change, when temperature increases at a) constant pressure and b) constant volume.

We can find ∆S using the formula ∆S = n*C*ln(T2/T1), where n is moles and C is heat capacity. Because we are using the heat capacity of ideal gas, we will refer to the heat capacities stated in Chapter 8. That is, Cv = (3/2)R and Cp = (5/2)R, where R is in the units of J x K-1 x mol-1.

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