The enthalpy of reaction at 273 K is -3.75 kJ. What will be the enthalpy of reaction at 373 K if ΔC_p is assumed to be zero ?

(a) -3075               (b) zero                (c) -3.75 x           (d) -3.75

10 ml of 1(N) NaOH is added with 10 ml of 1M HNO₃ and the mixture is shaken. The rise in temperature t₁ is noted. The experiment is repeated by using 100 ml of each of the same stock solution and increase in temperature t₂ is noted again. Which of the following relation is correct ?

(a) 2t₁ = t₂            (b) 10 t₁ = t₂           (c) t₁ = t₂            (d) t₁ = 10 t₂

Which of the following statement is false

The lattice energy of solid NaCl is 180 kcal/mol. The dissolution of the solid in water in the form of ions is endothermic to the extent of 1 kcal/mol. If the solution energies of Na⁺ and Cl^– are in the ratio 6:5, what is the enthalpy of hydration of Na⁺ ion.

The first I. P of A(g) is I₁ & second I.P. is I₂. Hence the E. A (Electron affinity)of A^Θ (g) is

(a) I₁/2             (b) I₁ + I₂             (c) I₁ – I₂/2             (d) I₁

If E is mean kinetic energy of one mole ideal monoatomic gas of mass ‘M’, the v_rms is related as

(a)                  (b)                    (c)                       (d)

For a reversible process at T = 300 K, the volume is increased from V₁ = 1L to V₂ = 10L. Calculate ΔH if the process is isothermal

The combustion of 2.650 of indium raised the temperature of a calorimeter 1.055^oC. The energy equivalent of the calorimeter was 2412.81 cal per ^oC. Calculate the molar energy of combustion of indium (Molar mass of indium 114.8)

Calculate DH when 10 litres of an ideal gas at STP is heated to 100^oC in a closed container

If 2 kJ of energy raises the temperature of a calorimeter containing 45 g of water from 23 to 32^oC, what is the water equivalent of the calorimeter ?

In thermodynamics, a process is called reversible when

Calculate Q and W for the isothermal reversible expansion of one mole of an ideal gas from an initial pressure of 1.0 bar to a final pressure of 0.1 bar at a constant temperature of 273 K

The enthalpy change of a compound is its :

At 300 K, the standard enthalpies of formation of C₆H₅COOH(s). CO₂(g) and H₂O(s) are – 408,   -393 and – 286 kJ mol^-1 respectively. Calculate the heat of combustion of benzoic acid at constant volume

(a) – 3296 kJ mol^-1         (b) – 3200 kJ mol^-1       

(c) – 3201 kJ mol^-1         (d) – 3603 kJ mol^-1

The standard molar enthalpies of formation of cyclohexane (l) and benzene (l) at 25^oC are -156 and +49 kJ mol^-1 respectively. The standard enthalpy of hydrogenation of cyclohexane (l) at 25^oC is – 119 kJ/mol. Find resonance energy of benzene

(a) – 152 kJ mol^-1          (b) – 159 kJ mol^-1

(c) +152 kJ mol^-1           (d) +159 kJ mol^-1