Question

Under standard conditions, will the following reaction proceed spontaneously as written?

$\mathrm{Fumarate}+\mathrm{NADH}+{\mathrm{H}}^{+}\rightleftharpoons \mathrm{succinate}+{\mathrm{NAD}}^{+}$

Short answer

The reaction will unfold spontaneously as written.

Step-by-step solution

Concept introduction

A chemical reaction is a procedure that causes one group of chemical components to change chemically into another.

Explanation

If $∆G^{o^{\text{'}}}$ is known to be negative, the reaction then will proceed as described. By expression, $∆G^{o^{\text{'}}}$ is linked to electromotive force $∆{\xi }^{o^{\text{'}}}$.

$∆G^{o^{\text{'}}}=-nF∆{\xi }^{o^{\text{'}}}$

If the reaction's role="math" localid="1663577937953" $∆{\xi }^{o^{\text{'}}}$ is said to be positive, the reaction's $∆G^{o^{\text{'}}}$ will be negative, which is a requirement for spontaneity.

$∆{\xi }^{o^{\text{'}}}=-0.040V$is the reduction of fumarate.

While $∆{\xi }^{o^{\text{'}}}=0.315V$ is the oxidation of $NADH$. The total electromotive force is positive,$∆{\xi }^{o^{\text{'}}}=0.355V$ .

Hence, the reaction is spontaneous.