List of top Chemistry Questions on Thermodynamics asked in NEET (UG)

The standard heat of formation, in kcal/mol, of $Ba^{2+}$ is:
Given: Standard heat of formation of SO₄²⁻(aq) = -216 kcal/mol, standard heat of crystallization of BaSO₄(s) = -4.5 kcal/mol, standard heat of formation of BaSO₄(s) = -349 kcal/mol.

Match List I with List II

List-I (Process)		List-II (Conditions)
(A)	Isothermal process	(I)	No heat exchange
(B)	Isochoric process	(II)	Carried out at constant temperature
(C)	Isobaric process	(III)	Carried out at constant volume
(D)	Adiabatic process	(IV)	Carried out at constant pressure

Choose the correct answer from the options given below:

The enthalpy of combustion of H₂, cyclohexene (C₆H₁₀) and cyclohexene (C₆H₁₂) are -241, -3800 and -3920 kJ per mol respectively. Heat of hydrogenation of cyclohexene is:

Assume each reaction is carried out in an open container. For which reaction will ∆H = ∆E?

At 25°C,the dissociation constant of a base, BOH, is 1.0 x 10^-12. The concentration of hydroxyl ions in 0.01 M aqueous solution of the base would be:

Which of the following pairs of a chemical reaction is certain to result in a spontaneous reaction?

A reaction occurs spontaneously if:

The absolute enthalpy of neutralisation of the reaction: MgO_(s)+2HCl_(aq)$\rightarrow$ MgCl_2(aq)+H₂O (l) will be:

If the bond energies of H–H, Br – Br and H –Br are 433, 192 and 364 kJ mol^–1 respectively the ∆Hº for the reaction H₂(g) + Br₂(g) $\rightarrow$2HBr(g)

Considering entropy (S) as a thermodynamic parameter, the criterion for the spontaneity of any process is

The solubility product of a sparingly soluble salt AX₂ is 3.2 ×10–11. Its solubility (in moles/liter) is

The work done during the expansion of a gas from a volume of 4 dm³ to 6 dm³ against a constant external pressure of 3 atm is

The standard enthalpy and standard entropy changes for the oxidation of ammonia at 298 K are –382.64 kJ mol^–1 and –145.6 JK^–1 mol^–1, respectively. Standard Gibbs energy change for the same reaction at 298 K is

The molar heat capacity of water at constant pressure, C, is 75 JK^–1mol^–1. When 1.0 KJ of heat is supplied to 100 g of water which is free to expand, the increase in temperature of water is:

For which one of the following equations is ∆Hº_reactequal to ∆Hº_f for the product:

Enthalpy of CH₄+$\frac{1}{2}$O₂$\rightarrow$CH₃OH is negative. If enthalpy of combustion of CH₄ and CH₃OH are x and y respectively. Then which relation is correct : -

Change in enthalpy for reaction 2H2O2(l) → 2H2O(l) + O2(g) If heat of formation of H2O2(l) and H2O(l) are – 188 & – 286 KJ/mol respectively : -

When 1 mol gas is heated at constant volume temp. is raised from 298 to 308 K. Heat supplied to the gas is 500 J. Then which statement is correct : -