Calculate the free energy change of$2{\rm{CuO}}\left( s \right) \to {\rm{C}}{{\rm{u}}_2}{\rm{O}}\left( s \right) + \frac{1}{2}{{\rm{O}}_2}\left( {\rm{g}} \right)$Given, ∆H=145.6kJ per mol ∆S=116 J per mol per K

NEET UG CHEMISTRY MCQ: THERMODYNAMICS

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Calculate the free energy change of

2\mathrm{CuO}\left( s \right) \to \mathrm{C}{\mathrm{u}_2}\mathrm{O}\left( s \right) + \frac{1}{2}{\mathrm{O}_2}\left( \mathrm{g} \right)

Given, ∆H=145.6kJ per mol ∆S=116 J per mol per K

View answer and explanation

Correct option: A

113.8 kJ per mol

Option A (113.8 kJ per mol) is correct because it is the result of calculating the Gibbs free energy change using the given enthalpy and entropy changes.

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