NEET UG CHEMISTRY MCQ: THERMODYNAMICS

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Which of the following relationships is correct

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Correct option: C

\ln \mathrm{k}=\frac{\mathrm{T} \Delta \mathrm{S}^{\circ}-\Delta \mathrm{H}^{\circ}}{\mathrm{RT}}

Option C (

\ln \mathrm{k}=\frac{\mathrm{T} \Delta \mathrm{S}^{\circ}-\Delta \mathrm{H}^{\circ}}{\mathrm{RT}}

) is correct because it represents the correct relationship between the equilibrium constant (k), Gibbs free energy change (∆G°), enthalpy change (∆H°), entropy change (∆S°), and temperature (T).

More Questions from THERMODYNAMICS

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The internal energy of one mole of a gas is: An ideal gas is allowed to expand both reversibly and irreversibly in an isolated system. If

{T_i}

is the initial temperature and

{T_f}

is the final temperature, which of the following statements is correct? For which of the process, ∆S is negative? The work done by a weightless piston in causing an expansion ∆V (at constant temperature), when the opposing pressure, P is variable, is given by: Assertion :- At constant pressure of the change

\mathrm{H}_2 \mathrm{O}(\mathrm{s}) \rightarrow \mathrm{H}_2 \mathrm{O}(\mathrm{g})

work done is negative.

Reason :- During phase transition work done is always negative. For the reaction,

\mathrm{X}_2 \mathrm{O_4(l}) \longrightarrow 2 \mathrm{XO}_2(\mathrm{g}), \Delta U=2.1 \mathrm{~kcal}, \Delta S=20 \mathrm{~cal} \mathrm{~K}^{-1}

300 \mathrm{~K}

. Hence,

\Delta G