SATHEE: Redox Reactions And Electrochemistry Ques 570

Redox Reactions And Electrochemistry Ques 570

Question: Use the following standand electrode potentials, calculate $Δ G^{\circ}$ in kJ/ mol for the indicated reaction:

$5 C e^{4 +} (a q) + M n^{2 +} (a q) + 4 H_{2} O (l) \overset{}{\to}$ $5 C e^{3 +} (a q) + M n O_{4}^{-} (a q) + 8 H^{+} (a q)$ $M n O_{4}^{-} (a q) + 8 H^{+} (a q) + 5 e^{-} \overset{}{\to}$ $M n^{2 +} (a q) + 4 H_{2} O (l); E^{\circ} = + 1.51 V$ $C e^{4 +} (a q) + e^{-} \overset{}{\to} C e^{3 +} (a q); E^{\circ} = + 1.61, V$

Options:

A) $- 9.65$

B) $- 24.3$

C) $- 48.25$

D) $- 35.2$

Show Answer

Answer:

Correct Answer: C

Solution:

[c] $E_{c e l l}^{^{\circ}} = E_{R} P^{^{\circ}} (R H S) - E_{R} P^{^{\circ}} (L H S)$ $= 1.61 - 1.51 \Rightarrow 0.10 V$ $Δ G^{\circ} = - n F E^{\circ} \Rightarrow - 5 \times 96500 \times 0.10 J$ $Δ G^{\circ} = - 48.25 k J m o l^{- 1}$

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Redox Reactions And Electrochemistry Ques 570

Question: Use the following standand electrode potentials, calculate ΔG∘ in kJ/ mol for the indicated reaction:

Options:

Answer:

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Question: Use the following standand electrode potentials, calculate $Δ G^{\circ}$ in kJ/ mol for the indicated reaction: