Embibe Experts Solutions for Chapter: Thermodynamics, Exercise 1: Assam CEE 2016

The bond dissociation enthalpy of gaseous ${\mathrm{H}}_2, {\mathrm{Cl}}_2$ and $\mathrm{HCl}$ are $435.243$ and $431 \mathrm{kJ} {\mathrm{mol}}^{-1}$ respectively. In the same unit, enthalpy of formation of $\mathrm{HCl}$ gas is

The entropy of a perfectly crystalline solid at absolute zero temperature is:

$365$ calorie heat is required to evaporate one gram water at $100{}^{\circ }\mathrm{C}$. If the work done by the system is $651.3$ calorie, then the increase in internal energy per mole of water will be

For a reaction, $\mathrm{\Delta G}=-67.2 \mathrm{kJ}$ and $\mathrm{\Delta H}=-42 \mathrm{kJ}$ at $300 \mathrm{K}$ temperature. The entropy change is

The standard enthalpy of combustion of carbon is $393.5 \mathrm{kJ}{ \mathrm{mol}}^{-1}$. The amount of heat released when carbon and oxygen gas produce $35.2 \mathrm{g}$ of ${\mathrm{CO}}_2$ is

The volume of one mole of an ideal gas is increased to $10$ times of its initial volume isothermally and reversibly. The change in entropy is

A reaction to be spontaneous at all temperatures, $\mathrm{\Delta H}$ and $\mathrm{\Delta S}$ must be respectively

Given that bond energies of $\mathrm{H}-\mathrm{H}$ and $\mathrm{Cl}-\mathrm{Cl}$ are $430 \mathrm{kJ} {\mathrm{mol}}^{-1}$ and $240 \mathrm{kJ}{ \mathrm{mol}}^{-1}$ respectively and ${\mathrm{\Delta H}}_{\mathrm{f}}$ for $\mathrm{HCl}$ is $-90 \mathrm{kJ}{ \mathrm{mol}}^{-1}$. The bond energy of $\mathrm{HCl}$ is