This is a 3-part question, I\'ve already found parts a and b, just need help wit

Question

This is a 3-part question, I've already found parts a and b, just need help with part c.

A cylinder contains 3 moles of helium gas at a temperature of 300 K.
Molar heat capacity for helium at constant volume= 2.98 Cal/Mol*K
Molar heat capacity for helium at constant pressure= 4.97 Cal/Mol*K
1 Cal = 4.186 Joules

a) how much heat must be transferred to the gas to increase its temperature to 500 K if the gas is heated at a constant volume? ANSWER: 7484.568 J of heat

b) how much heat must be transferred to the gas at constant pressure to raise the temperature to 500 K? ANSWER: 12482.652 J of heat

c) what is the work done by the gas in the process???

Explanation / Answer

in process a) work done by the gas is zero since there is no change in volume of the gas

in process b) we know tht Q +W(in) -W(out) =U

U=ncT =3(2.98)(200)*4.186=7484.568 J

Q=12482.652 W(in)=0 since no work is done on the system

hence work (out) =12482.652-7484.568 = 4998.084 J

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