AP EAMCET · Chemistry · Chemical Equilibrium
Observe the following equations
\(\begin{aligned}
& \mathrm{NH}_3+\mathrm{Ag}^{+} \rightleftharpoons\left[\mathrm{Ag}\left(\mathrm{NH}_3\right)\right]^{+}, \quad K_1=1.6 \times 10^3 \\
& {\left[\mathrm{Ag}\left(\mathrm{NH}_3\right)\right]^{+}+\mathrm{NH}_3 \rightleftharpoons\left[\mathrm{Ag}\left(\mathrm{NH}_3\right)_2\right]^{+},} \\
& K_2=6.8 \times 10^3
\end{aligned}\)
The equilibrium constant for the following reaction, \(\mathrm{Ag}^{+}+2 \mathrm{NH}_3 \rightleftharpoons\left[\mathrm{Ag}\left(\mathrm{NH}_3\right)_2\right]^{+}\)is
- A \(6.008 \times 10^3\)
- B \(1.088 \times 10^7\)
- C \(1.088 \times 10^6\)
- D \(1.028 \times 10^3\)
Answer & Solution
Correct Answer
(B) \(1.088 \times 10^7\)
Step-by-step Solution
Detailed explanation
When silver ion reacts with \(\mathrm{NH}_3\), then diammine silver (I) ion is formed. \(\left[\mathrm{Ag}\left(\mathrm{NH}_3\right)\right]^{+}+\mathrm{NH}_3 \rightleftharpoons\left[\mathrm{Ag}\left(\mathrm{NH}_3\right)_2\right]^{+}\), The equilibrium constant for the following…
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