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The Following Half-Reactions Occur in the Mercury Battery Used in Calculators

question 5

Multiple Choice

The following half-reactions occur in the mercury battery used in calculators. If E $\degree$ 1U1B1cell = 1.357 V, calculate the equilibrium constant for the cell reaction at 25 $\degree$ C. (Assume the stoichiometric coefficients in the cell reaction are all equal to 1.) HgO(s) + H₂O(l) + 2e¯ $The following half-reactions occur in the mercury battery used in calculators. If E \degree 1U1B1cell = 1.357 V, calculate the equilibrium constant for the cell reaction at 25 \degree C. (Assume the stoichiometric coefficients in the cell reaction are all equal to 1.) HgO(s) + H2O(l) + 2e¯ Hg(l) + 2OH¯(aq) ZnO(s) + H2O(l) + 2e¯ Zn(s) + 2OH¯(aq) A) 9.4 * 1022 B) 7.5 *1045 C) 6.4 * 1063 D) 7.8 * 1091 E) > 9.9* 1099$ Hg(l) + 2OH¯(aq)
ZnO(s) + H₂O(l) + 2e¯ $The following half-reactions occur in the mercury battery used in calculators. If E \degree 1U1B1cell = 1.357 V, calculate the equilibrium constant for the cell reaction at 25 \degree C. (Assume the stoichiometric coefficients in the cell reaction are all equal to 1.) HgO(s) + H2O(l) + 2e¯ Hg(l) + 2OH¯(aq) ZnO(s) + H2O(l) + 2e¯ Zn(s) + 2OH¯(aq) A) 9.4 * 1022 B) 7.5 *1045 C) 6.4 * 1063 D) 7.8 * 1091 E) > 9.9* 1099$ Zn(s) + 2OH¯(aq)

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