One mole of a dilute gas initially has a pressure equal to 1.00 atm, and a volum

Question

One mole of a dilute gas initially has a pressure equal to 1.00 atm, and a volume equal to 10.0 L and an internal energy of 1.52 kJ. As the gas is slowly heated, the plot of its state on aPV diagram moves in a straight line to the final state. The gas now has a pressure equal to 2.00 atm, and a volume equal to 71.0 L, and an internal energy equal to 21.6 kJ.

(a) Find the work done by the gas.
  kJ

(b) Find the heat absorbed by the gas.
  kJ

If you get answer for a. 91.5 ,which is wrong, please re-think / re-do it... for b, if you get 111.58, which is wrong again. This is why I have to post it again here.

please show your steps and get right answers. thanks

Explanation / Answer

Part A:

work done = area under P-V graph

1*[71.0-10.0] + [1/2 * [2.0 - 1.0] * [71.0 - 10.0] = 91.5 J

work done by the gas = 0.0915 kJ

Part B:

heat = work done + change in internal energy = 0.0915 kJ + [21.6 - 1.52] kJ

heat absorbed by the gas = 20.1715 kJ

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