Thermodynamics Questions

Heat required to raise the temperature of 1 mole of a substances by 1°C is called:

Given below are two statements: Statement I: A process or change is said to be reversible, if a change is brought out in such a way that the process could be reversed by an infinitesimal change. Statement II: A reversible process proceeds infinitely

Given below are two statements: Statement I: First law of thermodynamics is able to predict the spontaneity of a chemical reaction. Statement II: For chemical reactions, heat absorbed at constant volume, is measured in a bomb calorimeter.

Consider the reaction, 2X(s) + Y(g) → 2Z(g) + 700 kJ The signs of ΔH, ΔS and ΔG respectively are;

∆H and ∆S for a reaction are 4500 J mol–1 and 4.5 J K–1 mol–1 respectively. The reaction will be spontaneous;

The value of Cp/Cv γ for a monoatomic gas is;

Which of the following reactions correctly indicates the process of atomization?

When 1 mol of gas is heated at constant volume, temperature is raised from 298 to 308 K. Heat supplied to the gas is 500 J. Then which statement is correct?

The property, which can be classified as an intensive property, is;

Hess’s law is used in the determination of

Given below are two statements: Statement I: System and surroundings together constitute the universe. Statement II: The wall that separates the system from the surroundings is called boundary.

The incorrect option in the following table is:

Calculate entropy change when 5 moles of an ideal gas expands reversibly and isothermally from an initial volume of 5 litre to 50 litre at 27°C.

Enthalpy of combustion of carbon to CO2 is –393.52 kJ/mol. The heat released upon the formation of 11 g of CO2 from carbon and dioxygen is:

Two moles of an ideal gas are allowed to expand reversibly and isothermally at 300 K from a pressure of 1 atm to a pressure of 0.1 atm. The change in Gibbs free energy is:

The difference between enthalpy of reaction and change in internal energy at constant volume for the reaction given below at 25°C in kJ is: 2C6H6(l) + 15O2(g) → 12CO2(g) + 6H2O(l)

Given below are two statements: Statement I: If work is done on the system then work is positive. Statement II: If the work is done by the system then work is negative.

If the enthalpy change for the transition of liquid water to steam is 300 kJ mol–1 at 27°C, the entropy change for the process would be:

In thermodynamics, a process is called reversible when:

Which of the following is correct option for free expansion of an ideal gas under adiabatic condition?

Hess’s law states that;

In the combustion of 0.4 g of CH4, 0.25 kCal. of heat is liberated. The heat of combustion of CH4 is

When 229 J of energy is supplied as heat at constant pressure to 3 mol Ar(g), the temperature of the sample is increased by 2.55K. Calculate the molar heat capacity at constant volume;

For the given reaction : CO2(g) + H2(g) → CO(g) + H2O(g); ∆H = 40 kJ The ∆H is called;