250 litre of an ideal gas is heated at constant pressure from 27^(@)C such that its volume becomes 500 litre . The final temperature is
One mole of an ideal gas is heated at constant pressure so that its temperature rises by DeltaT = 72 K. In The heat supplied is Q=1.6 kJ, find the change in its internal energy and the work done by the gas.
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 :
One mole of an ideal gas is heated at constant pressure from 0^(@)C to 100^(@)C . a. Calculate the work done. b. If the gas were expanded isothermally and reversibly at 0^(@)C from 1 atm to some othe pressure P , what must be the final pressure if the maixmum work is equal to the work in (a) ?
One mole of an ideal gas is heated at constant pressure from 0^(@)C to 100^(@)C (A) Calculate work done. (B) If the gas were expanded isothermally and reversibly at 0^(@)C from 1 atm to some other pressure P_(1) , water must be the final pressure if the maximum work is equal to the work involned in (a)?
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:
When an ideal gas is heated at constant pressure, the fraction of the heat energy supplied whicn increases the internal energy of the gas 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
An ideal gas is heated at constant pressure and absorbs amount of heat Q. if the adiabatic exponent is gamma . Then find the fraction of heat absorbed in raising the internal energy and perofrming the work is.
