Calculate the value of the reaction quotient, Q, for the voltaic cell constructed from the following two half-reactions when the Zn²⁺ion concentration is 0.0110 M and the Ag⁺ ion concentration is 1.27 M?
$\mathrm { Zn } ^ { 2 + } ( \mathrm { aq } ) + 2 \mathrm { e } ^ { - }$ ? $\mathrm { Zn } ( \mathrm { s } ) ; E ^ { \circ } = - 0.76 \mathrm {~V}$ $\mathrm { Ag } ^ { + } ( \mathrm { aq } ) + \mathrm { e } ^ { - }$ ? $\mathrm { Ag } ( \mathrm { s } ) ; E ^ { \circ } = 0.80 \mathrm {~V}$

Question

Calculate the value of the reaction quotient, Q, for the voltaic cell constructed from the following two half-reactions when the Zn²⁺ion concentration is 0.0110 M and the Ag⁺ ion concentration is 1.27 M?

\mathrm { Zn } ^ { 2 + } ( \mathrm { aq } ) + 2 \mathrm { e } ^ { - }

?

\mathrm { Zn } ( \mathrm { s } ) ; E ^ { \circ } = - 0.76 \mathrm {~V}

\mathrm { Ag } ^ { + } ( \mathrm { aq } ) + \mathrm { e } ^ { - }

?

\mathrm { Ag } ( \mathrm { s } ) ; E ^ { \circ } = 0.80 \mathrm {~V}

Quizplus · Accepted Answer

The Answer of Calculate the value of the reaction quotient, Q, for the voltaic cell constructed from the following two half-reactions when the Zn²⁺ion concentration is 0.0110 M and the Ag⁺ ion concentration is 1.27 M? $\mathrm { Zn } ^ { 2 + } ( \mathrm { aq } ) + 2 \mathrm { e } ^ { - }$ ? $\mathrm { Zn } ( \mathrm { s } ) ; E ^ { \circ } = - 0.76 \mathrm {~V}$ $\mathrm { Ag } ^ { + } ( \mathrm { aq } ) + \mathrm { e } ^ { - }$ ? $\mathrm { Ag } ( \mathrm { s } ) ; E ^ { \circ } = 0.80 \mathrm {~V}$

Calculate the Value of the Reaction Quotient, Q, for the Voltaic