# Homework Help: PV diagrams

1. Aug 10, 2011

### Punkyc7

Two moles of an ideal gas are heated at constant pressure from a temperature of 29C to 110C.
calculate the work done by the gas

So work is the area under the PV curve, the only problem is I have no volume or intital pressure so PV=nRT doesnt help. Then I was thinking about Q= delta U -W but that doesnt seem to help.

How should I go about this problem because im stuck?

2. Aug 10, 2011

### Pi-Bond

The work done in general is

$W=\int PdV$

With constant pressure, this simplifies to

$W=P(V_{f}-V{i})$

where Vf and Vi are the final and initial volumes respectively. You can find these volumes by using the fact that the pressure P is constant (both volumes will have P in the denominator which will be eliminated from the expression above)

3. Aug 10, 2011

### rock.freak667

Well if the work done by a gas at constant pressure is given by W=P(V2-V1) how would this translate if you replace PV with nRT? (with the appropriate subscript)

4. Aug 10, 2011

### zspdztzx

Hi! Here are my two cents!

If there is no heat loss or particle loss in this process, then given the pressure is constant, therefore internal energy of the gas, delta-U, is zero, which, translates to, heat that flowed in, delta-Q, equals to W, the work done by the gas (i.e. expansion).

Therefore, avg KE increase in gas (reflected as temp increase) shall equal to the heat energy that flowed in, in turns, shall equal to the work done by the gas in expansion.

Equationally speaking:
W=Q=Delta-KE=n*(3/2)*R*Delta-T
(where "n" is number of moles of gas, "R" is ideal gas constant, and "Delta-T" is temperature difference in K and it's equal to temp difference in C).

Maybe I am wrong (please correct me if so!).. :)