One mole of an ideal gas is expanded freely and isothermally at `300 K` from `10` litres to `100` litres. If `DeltaE=0`, the value of `DeltaH` is

One mole of an ideal gas expanded freely and isothermally at 300 K from 5 litres to 10 litres. If DeltaE is 0 , then DeltaH is

One mole of an ideal gas is expanded freely and isothermally at 300K from 5L to 10L volume. If Delta E =0 , then Delta H is

4g of he gas is expanded isothermally at 300K from litre to 10L. The molar change in entropy is:

One mole of an ideal gas at 300 K is expanded ‘ isothermally from an Initial volume of ( litre to 10 litre. What is the value of AE for this process ?

One mole of an ideal gas expands isothermally at 300 K from 1 litre to 101 litres at constant pressure of 1 atmosphere. The work done during this change is (1 lit atrn = 24.2 cals)

One mole of an ideal gas at 300K is expanded isothermally from an inital volume of 1 litre to 10 litres. The DeltaE for this process is (R=2cal mol^(-1)K^(-1))