Using the Gibb's energy change, $\Delta $Go = +63.3 kJ, for the following reaction, Ag2CO3(s) $\rightleftharpoons$ 2 Ag+(aq) + CO32$-$ (aq) the Ksp of Ag2CO3(s) in water at 25oC is (R = 8.314 J K$-$1 mol$-$1)

Question

Using the Gibb's energy change, $\Delta $G^o = +63.3 kJ, for the following reaction,

Ag₂CO_3(s) $\rightleftharpoons$ 2 Ag⁺_(aq) + CO₃^2$-$ _(aq)
the K_sp of Ag₂CO_3(s) in water at 25^oC is
(R = 8.314 J K^$-$1 mol^$-$1)

3.2 $ \times $ 10^$-$26

8.0 $ \times $ 10^$-$12

2.9 $ \times $ 10^$-$3

7.9 $ \times $ 10^$-$2

Solution

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