Consider the following redox reaction : {\MnO}_4^{-}+ {\H}^{+}+ {\H}_2 {\C}_2 {\O}_4 ⇌ {\Mn}^{2+}+ {\H}_2 {\O}+ {\CO}_2 The standard reduction potentials are given as below ( {\E}_{\text{red }}^{\circ}) {\E}_{ {\MnO}_4^{-} \/ {\Mn}^{2+}}^{\circ}=+1.51 {\V} {\E}_{ {\CO}_2 \/ {\H}_2 {\C}_2 {\O}_4}^{\circ}=-0.49 {\V} If the equilibrium constant of the above reaction is given as {\K}_{ {\eq}}=10^{ {\x}}, then the value of {\x}=_____ (nearest integer) [1-Feb-2024 Shift 2]

Electrochemistry Part 2

Section: Chemistry

Question : 54 of 117

Marks: +1, -0

Consider the following redox reaction :
MnO4−+H++H2C2O4⇌Mn2++H2O+CO2
The standard reduction potentials are given as below (E‌red ‌∘)
EMnO4−∕Mn2+∘=+1.51V
ECO2∕H2C2O4∘=−0.49V
If the equilibrium constant of the above reaction is given as Keq=10x, then the value of x=_____ (nearest integer)

[1-Feb-2024 Shift 2]

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