Chemistry · Thermodynamics & Thermochemistry

JEE Advanced 2018 — Paper 2 — Question 25

Consider an electrochemical cell: A(s)∣An+(aq,2M)∥B2n+(aq,1M)∣B(s)\mathrm{A}(\mathrm{s})\left|\mathrm{A}^{\mathrm{n}+}(\mathrm{aq}, 2 \mathrm{M}) \| \mathrm{B}^{2 \mathrm{n}+}(\mathrm{aq}, 1 \mathrm{M})\right| \mathrm{B}(\mathrm{s}). The value of ΔH⊖\Delta \mathrm{H}^{\ominus} for the

cell reaction is twice that of ΔG⊖\Delta \mathrm{G}^{\ominus} at 300 K . If the emf of the cell is zero, the ΔS⊖\Delta \mathrm{S}^{\ominus} (in JK−1 mol−1\mathrm{J} \mathrm{K}^{-1} \mathrm{~mol}^{-1} ) of the

cell reaction per mole of B formed at 300 K is ____\_\_\_\_ .

(Given: ln⁡(2)=0.7\ln (2)=0.7, R (universal gas constant) =8.3 J K−1 mol−1.H,S=8.3 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1} . H, S and GG are enthalpy, entropy

and Gibbs energy, respectively.)

Answer: -11.62

Numerical answer — enter this value.

Step-by-step solution

A(s)∣An+(aq,2M)∥B2n+(aq,1M)∣B(s)\mathrm{A}(\mathrm{s})\left|\mathrm{A}^{\mathrm{n}+}(\mathrm{aq}, 2 \mathrm{M}) \| \mathrm{B}^{2 \mathrm{n}+}(\mathrm{aq}, 1 \mathrm{M})\right| \mathrm{B}(\mathrm{s})

2 A( s)⟶2 An++2ne−2 \mathrm{~A}(\mathrm{~s}) \longrightarrow 2 \mathrm{~A}^{\mathrm{n}+}+2 \mathrm{ne}^{-}

B2n++2ne−⟶B(s)\mathrm{B}^{2 \mathrm{n}+}+2 \mathrm{ne}^{-} \longrightarrow \mathrm{B}(\mathrm{s})

2 A( s)+B2n+⟶2 An++B(s)2 \mathrm{~A}(\mathrm{~s})+\mathrm{B}^{2 \mathrm{n}+} \longrightarrow 2 \mathrm{~A}^{\mathrm{n}+}+\mathrm{B}(\mathrm{s})

Q=[An+]2[ B2n+]=2×21=4\mathrm{Q}=\frac{\left[\mathrm{A}^{\mathrm{n}+}\right]^{2}}{\left[\mathrm{~B}^{2 \mathrm{n}+}\right]}=\frac{2 \times 2}{1}=4

ΔG∘=ΔH∘−TΔS∘\Delta \mathrm{G}^{\circ}=\Delta \mathrm{H}^{\circ}-\mathrm{T} \Delta \mathrm{S}^{\circ}

ΔH∘=2ΔG∘\Delta \mathrm{H}^{\circ}=2 \Delta \mathrm{G}^{\circ}

Ecell 0=RT2nFln⁡4\mathrm{E}_{\text {cell }}^{0}=\frac{\mathrm{RT}}{2 \mathrm{nF}} \ln 4

ΔG0=−2n×F×RT2nFln⁡4\Delta \mathrm{G}^{0}=-2 \mathrm{n} \times \mathrm{F} \times \frac{\mathrm{RT}}{2 \mathrm{nF}} \ln 4

ΔG0=−RTln⁡4\Delta \mathrm{G}^{0}=-\mathrm{RT} \ln 4

ΔS0=ΔH0−ΔG0 T=ΔG0 T=−RTln⁡4 T\Delta \mathrm{S}^{0}=\frac{\Delta \mathrm{H}^{0}-\Delta \mathrm{G}^{0}}{\mathrm{~T}}=\frac{\Delta \mathrm{G}^{0}}{\mathrm{~T}}=-\frac{\mathrm{RT} \ln 4}{\mathrm{~T}}

ΔS0=−8.314×1.4\Delta \mathrm{S}^{0}=-8.314 \times 1.4

=−11.62 J mol−1 K−1=-11.62 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}

Answer key and solution verified before publishing.

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Exam
JEE Advanced 2018
Paper
Paper 2
Subject
Chemistry
Chapter
Thermodynamics & Thermochemistry
Topic
Gibbs Free Energy - Relation with Equilibrium, Metallurgy and Electrochemistry
Consider an electrochemical cell: A ( s ) A n + ( aq , 2 M ) \ B 2 n… | JEE Advanced 2018 PYQ with Solution · DhiX AI