One mole of an ideal gas at 300K is expanded isothermally from one litre volume to ten litres of volume. Find change in internal energy in this process? R= 2cal/K/mol.
Calculate the work done when one mole of gas expands reversible isothermally from 5 atm to 1 atm at 300K? (value of log5= 0.6989)
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$\begingroup$ PLease read the posting guidelines. This is not a "do your homework for you" site. $\endgroup$– Carl WitthoftNov 16, 2015 at 12:44
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1 Answer
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Answer 1.
As its isothermal so the temperature remains constant. So the change in internal energy is 0.
Answer 2.
Its formula is $W = -nRT$ $log_e(P_i/P_f)$
Putting the values we get $W = -4012.6497831$
Here $W$ is work done on the system
