The enthalpy and entropy change for the reaction,${\rm{B}}{{\rm{r}}_2}\left( l \right) + {\rm{C}}{{\rm{l}}_2}\left( {\rm{g}} \right) \to 2{\rm{BrCl}}\left( {\rm{g}} \right)$Are 30 kJ${\rm{mo}}{{\rm{l}}^{ - 1}}$and$105{\rm{J}}{{\rm{K}}^{ - 1}}{\rm{mo}}{{\rm{l}}^{ - 1}}$respectively. The temperature at which the reaction will be in equilibrium is:

NEET UG CHEMISTRY MCQ: THERMODYNAMICS

1 Medium

1 of 1

Application +4 | -1

The enthalpy and entropy change for the reaction,

\mathrm{B}{\mathrm{r}_2}\left( l \right) + \mathrm{C}{\mathrm{l}_2}\left( \mathrm{g} \right) \to 2\mathrm{BrCl}\left( \mathrm{g} \right)

Are 30 kJ

\mathrm{mo}{\mathrm{l}^{ - 1}}

and

105\mathrm{J}{\mathrm{K}^{ - 1}}\mathrm{mo}{\mathrm{l}^{ - 1}}

respectively. The temperature at which the reaction will be in equilibrium is:

View answer and explanation

Correct option: C

285.7 K

Option C (285.7 K) is correct because the equilibrium temperature is calculated using T = ∆H/∆S.