The electrode potential E$_{\left(\frac{Zn^{2+}}{Zn}\right)}$ of a zinc electrode at 25$^{\circ}$C with an aqueous solution of 0.1M $ZnSO_4$ is
(E$^{\circ}$$_{\left(\frac{Zn^{2+}}{Zn}\right)}$ = -0.76 V. Assume $\frac{2.303RT}{F} =$ 0.06 at 298 K)
- 0.73
- -0.79
- -0.82
- -0.7
The Correct Option is B
Solution and Explanation
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For the reaction:
\[ 2A + B \rightarrow 2C + D \]
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The total order and order in [B] for the reaction are respectively:
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Concepts Used:
Nernst Equation
This equation relates the equilibrium cell potential (also called the Nernst potential) to its concentration gradient across a membrane. If there is a concentration gradient for the ion across the membrane, an electric potential will form, and if selective ion channels exist the ion can cross the membrane.
