If an ideal gas is heated at constant pressure :

One mole of an ideal gas is heated at constant pressure. If an 100 Joule heat energy supplied to the gas, then work done by the gas will be …….. (gamma=1.4)

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 :

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 of 1 atmosphere form 0^@C to 100^@C the change in the internal energy is (R = 8 J/ mol K )

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)?