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12 Dec 2019

Using standard electrode potentials calculate ΔG∘rxn and use its value to estimate the equilibrium constant for each of the reactions at 25 ∘C.

Calculate K

MnO2(s)+4H+(aq)+Cu(s)→Mn2+(aq)+2H2O(l)+Cu2+(aq)

Express your answer using one significant figure.

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Tod Thiel
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13 Dec 2019

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Related questions

Exercise 18.65

Use tabulated half-cell potentials to calculate ΔG∘rxn for each of the following reactions at 25 ∘C.

Part A

Pb2+(aq)+Mg(s)→Pb(s)+Mg2+(aq)
ΔG∘rxn = kJ

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Part B

Br2(l)+2Cl−(aq)→2Br−(aq)+Cl2(g)

Express your answer using two significant figures.
ΔG∘rxn = kJ

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Part C

MnO2(s)+4H+(aq)+Cu(s)→Mn2+(aq)+2H2O(l)+Cu2+(aq)

Express your answer using two significant figures.
ΔG∘rxn = kJ

Show transcribed image text

Use the Ɛ° from the standard reduction table to calculate ∆G° and Keq for each of the following reactions at 25°C (298K)

a) Pb+2(aq) + Mg(s)→Pb(s) + Mg+2(aq)

b) Br2(l) + 2 Cl-(aq)→Cl2(g) + 2 Br-(aq)

c) O2(g)+2 H2O(l) +2 Cu(s)→4 OH- (aq) + 2 Cu+2

d) MnO2 (s) + 4 H+(aq) +Cu(s)→Mn+2(aq) + 2 H2O(l)+Cu+2(aq)

From standard reduction table:

Pb2+(aq) + 2e- → Pb(s) ε^ο(v) = -0.13
Mg2+(aq) + 2e- → Mg(s) ε^ο(v) = -2.37

Br2(l) + 2e- → 2Br-(aq) ε^ο(v) = +1.07
Cl2(g) + 2e- → 2Cl-(aq) ε^ο(v) = +1.36

O2(g) + 2H2O(l ) + 4e- → 4OH-(aq) ε^ο(v) = +0.40
Cu+2(aq) + 2e- → Cu(s) ε^ο(v) = +0.34

MnO2(s) + 4H+(aq) + 2e- → Mn+2(aq) + 2H2O(l) ε^ο(v) = +1.23
Cu+2(aq) + 2e- → Cu(s) ε^ο(v) = +0.34

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