The external work done in case of a closed gaseous system is `W = int pdV` - establish this relation.

In a process, if dU, dW and dQ are change in internal energy, work done and heat accepted respectively for a system, what is the relation between dU , dQ and dW?

Show that the external work done by a gas in an isothermal expansion is equal to the heat supplied to the gas.

(i) What do you mean by heat of reaction at constannt volume and heat of reaction at constant pressure? (ii) Establish the relation DeltaH=DeltaU=DeltanRT for a chemical reaction in gaseous state.

Pressure-volume (PV) work done by an ideal gaseous system at constant volume is (where E is internal energy of the system)

The internal energy of a system is U_(1) . In a process, work done by the system is W and heat accepted by the system is Q. At the end of the process, the internal energy of the system is

Statement I : For a charged particle moving form point P to point Q, the net work done by an electrostatic field on the particle is independent of the path connecting points P and Q. Statement II : The net work done by a conservative force on an object moving along a closed loop is zero.

P*V Work done by an ideal gaseous system at constant volume is (E is internal energy of the system)-

Assuming the system performs only pressure-volume work, show that heat absorbed by a closed system at constant volume is equal to the increase in its internal energy.

Assuming the system performs only pressure-volume work, show that heat evolved by a closed systemm at constant pressure is equal to the decrease in its enthalpy.