Thermodynamics- 1st Law Question

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SUMMARY

The discussion centers on applying the First Law of Thermodynamics to calculate the increase in internal energy of a gas in a piston system. The gas is maintained at a constant pressure of 8 kPa while being heated, resulting in a heat input of 42 J and a piston displacement of 40 mm. The equation Q - W = ΔU is utilized, where W is the work done by the gas. The solution involves calculating the change in volume using the cross-sectional area of the piston and the displacement.

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Homework Statement



A gas is enclosed in a container fitted with a piston of cross-sectional area 0.1 m2. The pressure of the gas is maintained constant at 8 kPa, while the gas is heated slowly and the piston moves outward a distance of 40 mm. Heat input to the gas during this process is 42 J. What is the increase in internal energy of the gas?

Homework Equations



I know that the first law needs to be used here, and i am neglecting Kinetic and Potential Energy

Q-W=(delta)U

The Attempt at a Solution



Im having trouble solving for work, this is what i have so far.

42J-8KPa(V2-V1)=(delta) U

any help would be great, thanks

FordRanger
 
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You don't really need to know V1 and V2. You only need the change in volume. Since you have the cross sectional area of the cylinder and the displacement, you can find delta-V and complete your problem.
 
Thanks, i ended up figuring it out pretty soon after posting.
 

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