In an adiabatic expansion of a gas initial and final temperatures are `T_(1)`and `T_(2)` respectively, then the change in internal energy of the gas is

n moles of an ideal monoatomic gas undergoes an isothermal expansion at temperature T, during which its volume becomes 4 times. The work done on the gas and change in internal energy of the gas respectively are

What happens to the change in internal energy of a gas during adiabatic expansion?

What happens to the change in internal energy of a gas during adiabatic expansion?

One mole of hydrogen, assumed to be ideal, is adiabatically expanded from its initial state (P_(1), V_(1), T_(1)) to the final state (P_(2), V_(2), T_(2)) . The decrease in the internal energy of the gas during this process will be given by

One mole of hydrogen, assumed to be ideal, is adiabatically expanded from its initial state (P_(1), V_(1), T_(1)) to the final state (P_(2), V_(2), T_(2)) . The decrease in the internal energy of the gas during this process will be given by

One mole of hydrogen, assumed to be ideal, is adiabatically expanded from its initial state (P_(1), V_(1), T_(1)) to the final state (P_(2), V_(2), T_(2)) . The decrease in the internal energy of the gas during this process will be given by

The initial state of 1 mol of an ideal gas is (P_(1),V_(1),T_(1)) . The gas is expanded by a reversible isothermal process and also by a reversible adiabatic process separately. If final volume of the gas is same in both the processes, and changes in internal energy in the isothermal and adiabatic processes are DeltaU_(1) and DeltaU_(2) respectively, then-

An ideal gas expands adiabatically from an initial temperature T_(1) to a final temperature T_(2) . Prove that the work done by the gas is C_(V) (T_(1) - T_(2)) .