Question:
Using the Gibbs energy change, \(△G° = + 63.3\ kJ\), for the following reaction,
\(Ag_2CO_3 (g) ⇋ 2Ag+ (aq) + CO_3^{2–} (aq)\)
the \(K_{sp}\) of \(Ag_2CO_3 \)(s) in water at \(25°C\) is :
\((R = 8.314\ J K^{–1} mol^{–1})\)
Using the Gibbs energy change, \(△G° = + 63.3\ kJ\), for the following reaction,
\(Ag_2CO_3 (g) ⇋ 2Ag+ (aq) + CO_3^{2–} (aq)\)
the \(K_{sp}\) of \(Ag_2CO_3 \)(s) in water at \(25°C\) is :
\((R = 8.314\ J K^{–1} mol^{–1})\)
\(Ag_2CO_3 (g) ⇋ 2Ag+ (aq) + CO_3^{2–} (aq)\)
the \(K_{sp}\) of \(Ag_2CO_3 \)(s) in water at \(25°C\) is :
\((R = 8.314\ J K^{–1} mol^{–1})\)
Updated On: Apr 20, 2026
- \(8 .0 \times 10^{–12}\)
- \(2.9 \times 10^{–3}\)
- \(7.9 \times 10^{–2}\)
- \(3.2 \times 10^{–36}\)
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The Correct Option is A
Solution and Explanation
The correct option (A): \(8 .0 \times 10^{–12}\).
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