A) \[1.08\times {{10}^{-7}}\]
B) \[1.08\times {{10}^{-5}}\]
C) \[1.08\times {{10}^{-9}}\]
D) \[None\]
Correct Answer: A
Solution :
[b] \[1.08\times {{10}^{-5}}\] As the reaction takes place in two steps. \[A{{g}^{+}}+N{{H}_{3}}{{[Ag\,(N{{H}_{3}})]}^{+}}\] \[{{[Ag\,(N{{H}_{3}})]}^{+}}+NH\,{{[Ag\,{{(N{{H}_{3}})}_{2}}]}^{+}}\] \[k={{k}_{1}}\times {{k}_{2}}\] \[=(6.8\times {{10}^{-3}})\times (1.6\times {{10}^{-3}})\] \[=10.8\times {{10}^{-6}}=1.08\times {{10}^{-5}}\]You need to login to perform this action.
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