Two moles of an ideal monoatomic gas are expanded according to the equation pT=constant form its initial state `(p_0, V_0)` to the final state due to which its pressure becomes half of the initial pressure. The change in internal energy is

One mole of an ideal monoatomic gas at temperature T_0 expands slowly according to the law p/V = constant. If the final temperature is 2T_0 , heat supplied to the gas is

One mole of an ideal monoatomic gas at temperature T_0 expands slowly according to the law p/V = constant. If the final temperature is 2T_0 , heat supplied to the gas is

One mole of an ideal monoatomic gas at temperature T_(0) expands slowely according to the law P/V=constant. If the final temperature is 2T_(0) heat supplied to the gas is -

One mole of an ideal monoatomic gas at temperature T_0 expands slowly according to the law p/V = constant. If the final temperature is 2T_0 , heat supplied to the gas is

One mole of an ideal monoatomic gas at temperature T_0 expands slowly according to the law p/V = constant. If the final temperature is 2T_0 , heat supplied to the gas is

One mole of an ideal monoatomic gas at temperature T_0 expands slowly according to the law p/V = constant. If the final temperature is 2T_0 , heat supplied to the gas is

One mole of an ideal monoatomic gas expands isothermally against constant external pressure of 1 atm from initial volume of 1l to a state where its final pressure becomes equal to external pressure. If initial temperature of gas is 300K then total entropy change of system in the above process is: [R =0.082L atm mol^(-1)K^(-1)= 8.3J mol^(-1) K^(-1) ]

One mole of an ideal monoatomic gas expands isothermally against constant external pressure of 1 atm from initial volume of 1L to a state where its final pressure becomes equal to external pressure. If initial temperature of gas is 300K then total entropy change of system in the above process is: [R=0.082L atm mol^(-1) K^(-1)-=8.3J mol^(-1) K^(-1)]