MHT-CET (DEMO) CLASS 11 CHEMISTRY THERMODYNAMICS PAPER

For which of the following reactions, $$\Delta H$$ is equal to $$\Delta U$$ ?

For which of the following processes. $$\Delta \mathrm{S}$$ is negative?

At 320 K , a gas $$A_{2}$$ is $$20 \%$$ dissociated to $$\mathrm{A}(\mathrm{g})$$. The standard free energy change at 320 K and 1 atm in J $$\mathrm{mol}^{-1}$$ is approximately
( $$\left.R=8.314 \mathrm{JK}^{-1} \mathrm{~mol}^{-1} ; \ln 2=0.693 ; \ln 3=1.098\right)$$

For a reaction, $$\mathrm{A}(\mathrm{g}) \rightarrow \mathrm{Al}) ; \Delta \mathrm{H}=-3 \mathrm{RT}$$. The correct statement for the reaction is

The enthalpy change on freezing of 1 mol of water at $$5^{\circ} \mathrm{C}$$ to ice at $$-5^{\circ} \mathrm{C}$$ is:
(Given $$\Delta_{f u s} H=6 \mathrm{kmol}^{-1}$$ at $$0^{0} \mathrm{C}, C_{p}\left(H_{2} \mathrm{O}, l\right)=75.3 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1} \mathrm{C}_{p}\left(\mathrm{H}_{2} \mathrm{O}, \mathrm{s}\right)=36.8 \mathrm{Jmol}^{-1} \mathrm{~K}^{-1}$$ )

A mixture of 2 mole of carbon monoxide gas and one mole of dioxygen gas is enclosed in a vessel and is ignited to convert carbon monoxide into carbon dioxide. If the enthalpy change is $$\Delta \mathrm{H}$$ and internal energy change is $$\Delta U$$, then for the above process –

The enthalpy of neutralization of $$\mathrm{NH}_{4} \mathrm{OH}$$ and $$\mathrm{CH}_{3} \mathrm{COOH}$$ is $$-10.5 \mathrm{kcal} / \mathrm{mole}$$ and enthalpy of neutralization of strong base and $$\mathrm{CH}_{3} \mathrm{COOH}$$ is $$-12.5 \mathrm{kcal} / \mathrm{mole}$$. Calculate the enthalpy of bond dissociation of base $$\mathrm{NH}_{4} \mathrm{OH}-$$

Given that
$$\mathrm{CO}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{~g}) \rightarrow \mathrm{CO}_{2}(\mathrm{~g}) ; \Delta \mathrm{H}^{\mathrm{o}}=-\mathrm{x} \mathrm{kJ}$$
which of the following is correct –

For the reaction,

bond energies are given as under –
(i) $$\mathrm{C}-\mathrm{C}, 346 \mathrm{~kJ} / \mathrm{mol}$$
(ii) $$\mathrm{C}-\mathrm{H}, 413 \mathrm{~kJ} / \mathrm{mol}$$
(iii) $$\mathrm{H}-\mathrm{H}, 437 \mathrm{~kJ} / \mathrm{mol}$$ and
(iv) $$\mathrm{C}=\mathrm{C}, 611 \mathrm{~kJ} / \mathrm{mol}$$

What will be the value of $$\Delta \mathrm{H} 25^{\circ} \mathrm{C}$$ for the above reaction ?

Latent heat of vaporisation of water is $$540 \mathrm{cal} \mathrm{g}^{-1}$$. The entropy change during the evaporation of 1 mole of water at $$100^{\circ} \mathrm{C}$$ is –

The solubility product of AgCl is $$1.6 \times 10^{-10}$$ and $$\log$$ ksp is -9.80 . The value of $$\Delta\mathrm{G}^{\circ}$$ for the process, $$\mathrm{AgCl}(\mathrm{s})+\mathrm{aq} \rightleftharpoons \mathrm{Ag}^{+}(\mathrm{aq})+\mathrm{Cl}^{-}(\mathrm{aq})$$ is –

Which of the following process involves decrease in the entropy of system –

The bond enthalpies of $$\mathrm{H}_{2}, \mathrm{X}_{2}$$ and HX are in the ratio of $$2: 1: 2$$. if the enthalpy for formation of HX is $$-50 \mathrm{~kJ} \mathrm{~mol}^{-1}$$, the bond enthalpy if $$\mathrm{H}_{2}$$ is –

$$\Delta \mathrm{S}^{\circ}$$ and $$\Delta \mathrm{H}^{\circ}$$ for combustion of methane are $$186 \mathrm{JK}^{-1}$$ and $$-74.8 \mathrm{~kJ} \mathrm{~mol}^{-1}$$ respectively. The value of $$\Delta \mathrm{U}^{\circ}$$ for the process would be –

The standard free energy change $$\Delta G^{\circ}$$ is related to equilibrium constant, $$K_{p}$$ as –