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One mole of an ideal gas undergoes reversible isothermal expansion from an initial volume V_(1) to a final volume 10V_(1), and does 10 kJ of work. The initial pressure was 1xx10^(7) Pa. (a) Calculate V_(1) . (b) If there were two moles of the gas, what had been its temperature ? |
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Answer» Solution :For reversible ISOTHERMAL expansion of an ideal gas, (a) `W=-2.303nRTlog.(V_(2))/(V_(1))=-10,000("GIVEN")` or `2.303xx1xx8.314xxTlog.(10V_(1))/(V_(1))=10,000` `T=522.27K` We have `pV=nRT` `10^(7)xxV_(1)=1xx8.314xx522.27` `V_(1)=4.342xx10^(-4)m^(3)` (b) Assuming pressure to remain constant, for 2 moles of the ideal gas. `T=(522.27)/(2)=261.13 K`. |
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