10 mole of an ideal gas is heated at constant pressure of one atmosphere from `27^(@)C` to `127^(@)C`. If `C_(v,m)=21.686+10^(-3)T(JK^(-1).mol^(-1))`, then `DeltaH` for the process is :

Two mole of an ideal gas is heated at constant pressure of one atmosphere from 27^(@)C to 127^(@)C . If C_(v,m)=20+10^(-2)"T JK"^(-1).mol^(-1) , then q and DeltaU for the process are respectively:

Two mole of an ideal gas is heated at constant pressure of one atmosphere from 27^(@)C to 127^(@)C . If C_(v,m)=20+10^(-2)"T JK"^(-1).mol^(-1) , then q and DeltaU for the process are respectively:

Two mole of an ideal gas is heated at constant pressure of one atmosphere from 27^(@)C to 127^(@)C . If C_(v,m)=20+10^(-2)" T JK"^(-1).mol^(-1) , then q and DeltaU for the process are respectively:

Two mole of an ideal gas is heated at constant pressure of one atmosphere from 27^(@)C to 127^(@)C . If C_(v, m) = 20 + 10^(-2) TJK^(-1) mol^(-1) , then q and Delta U for the process are respectively.

10 mole of an ideal gas is heated at constant pressure of one atmosphere from 27^(@)C to 127^(@)C . If C_(v, m) = 21.686 + 10^(-3) T , then Delta H for the process is x xx 10^(5) J1 . Then x is

3.0 moles of ideal gas is heated at constant pressure from 27^(@)C to 127^(@)C . Then the work expansion of gas is

One mole of an ideal monoatomic gas is heated at a constant pressure of 1 atmosphere from 0^(@) C to 100^(@0 C. Work done by the gas is

One mole of an ideal monoatomic gas is heated at constant pressure from 0^@C to 100^@C . Calculate work done.