Discuss the significance of the mathematical expression in which the heat absorbed by a system is related to internal energy and work done by the system.

What will happen to internal energy if work is done by the system?

Define the term 'enthalpy'. What will happen to the internal energy if work is done by the system ?

Figure shows the P-V siagram of a cyclic process. If dQ is the heat energy supplied to the system, dU is change in the internal energy of the system and dW is the work done by the system, then which of the following relations is/are correct

Assertion: If a gas is heated isothennally, then no part of the heat supplied is used to increase the internal energy. Reason: Change in internal energy equals work done on the system.

For a gaseous system find change in internal energy if the heat supplied to the system is 50 J and work done by the system is 16 J.

Express the change in internal energy of a system when (i) No heat is absorbed by the system from the surroundings, but work (w) is done on the system. What type of wall does the system have ? ii) No work is done on the system, but q amount of heat is taken out from the system and given to the surroundings. What type of wall does the system have? (iii) w amount of work is done by the system and q amount of heat is supplied to the system. What type of system would it be?