Embibe Experts Solutions for Chapter: Thermodynamics, Exercise 3: EXERCISE-II (Previous Year Questions)

The enthalpy and entropy change for the reaction ${\mathrm{Br}}_2 \left(\mathrm{I}\right)+{\mathrm{Cl}}_2 \left(\mathrm{g}\right)\to 2\mathrm{BrCl} \left(\mathrm{g}\right)$ are $30 \mathrm{kJ} {\mathrm{mol}}^{-1}$ and $105 \mathrm{J} {\mathrm{K}}^{-1} {\mathrm{mol}}^{-1}$, respectively. The temperature at which the reaction will be in equilibrium is

The enthalpy of hydrogenation of cyclohexene is$-119.5 \mathrm{KJ} {\mathrm{mol}}^{-1}$. If resonance energy of benzene is$-150.4 \mathrm{KJ} {\mathrm{mol}}^{-1}$, its enthalpy of hydrogenation would be?

If the enthalpy change for the transition of liquid water to steam is $30 \mathrm{kJ} {\mathrm{mol}}^{-1}$ at $27° \mathrm{C}$, the entropy change for the process would be

Which of the following is not thermodynamic function 

Which of the following is intensive property ?

The correct thermodynamic conditions for the spontaneous reaction at all temperatures is

For a given reaction, $\mathrm{\Delta H}=35.5 \mathrm{kJ} {\mathrm{mol}}^{-1}$ and $\mathrm{\Delta S}=83.6{\mathrm{JK}}^{-1} {\mathrm{mol}}^{-1}$.The reaction is spontaneous at :(Assume that $\mathrm{\Delta H}$ and $\mathrm{\Delta S}$ do not vary with temperature)

The heat of combustion of ${\mathrm{C}}_4{\mathrm{H}}_{10}$ is $-2878 \mathrm{kJ}$ ${\mathrm{mol}}^{-1}$. If the heats of formation of ${\mathrm{CO}}_2$ and ${\mathrm{H}}_2\mathrm{O}$ are $-393.5 \mathrm{kJ}{ \mathrm{mol}}^{-1}$ and $-285.8 \mathrm{kJ}{ \mathrm{mol}}^{-1}$ then the heat of formation of ${\mathrm{C}}_4{\mathrm{H}}_{10}$ is :-