Consider the following standard electrode potentials and calculate the equilibrium constant at 25° C for the indicated disproportionation reaction: 3 Mn 2+( aq ) longrightarrow Mn ( s )+2 Mn 3+( aq ) Mn 3+( aq )+ e - longrightarrow Mn 2+( aq ) ; E°=1.51 V Mn 2+( aq )+2 e - longrightarrow Mn ( s ) ; E°=-1.185 V

Question

Consider the following standard electrode potentials and calculate the equilibrium constant at 25° C for the indicated disproportionation reaction: 3 Mn 2+( aq ) longrightarrow Mn ( s )+2 Mn 3+( aq ) Mn 3+( aq )+ e - longrightarrow Mn 2+( aq ) ; E°=1.51 V Mn 2+( aq )+2 e - longrightarrow Mn ( s ) ; E°=-1.185 V (A) 1.2 × 10-43 (B) 2.4 × 10-73 (C) 6.3 × 10-92 (D) 1.5 × 10-62

Tardigrade Admin · Accepted Answer

Correct answer is (c) 6.3 × 10-92

$1.2 \times 1 0^{- 43}$

$2.4 \times 1 0^{- 73}$

$6.3 \times 1 0^{- 92}$

$1.5 \times 1 0^{- 62}$

Correct answer is (c) $6.3 \times 1 0^{- 92}$

Q. Consider the following standard electrode potentials and calculate the equilibrium constant at 25∘C for the indicated disproportionation reaction : 3Mn2+(aq)⟶Mn(s)+2Mn3+(aq) Mn3+(aq)+e−⟶Mn2+(aq);E∘=1.51V Mn2+(aq)+2e−⟶Mn(s);E∘=−1.185V

1.2×10−43

2.4×10−73

6.3×10−92

1.5×10−62

Correct answer is (c) 6.3×10−92

$1.2 \times 1 0^{- 43}$

$2.4 \times 1 0^{- 73}$

$6.3 \times 1 0^{- 92}$

$1.5 \times 1 0^{- 62}$

Correct answer is (c) $6.3 \times 1 0^{- 92}$