A) \[1\times {{10}^{-4}}M{{s}^{-1}}\]
B) \[4\times {{10}^{-4}}M{{s}^{-1}}\]
C) \[5\times {{10}^{-3}}M{{s}^{-1}}\]
D) \[1\times {{10}^{-3}}M{{s}^{-1}}\]
Correct Answer: A
Solution :
Given, rate\[=2.0\times {{10}^{-4}}M{{s}^{-1}}\] For the reaction, \[{{N}_{2}}(g)+3{{H}_{2}}(g)\xrightarrow[{}]{{}}2N{{H}_{3}}(g)\] \[-\frac{d[{{N}_{2}}]}{dt}=\frac{d[{{H}_{2}}]}{3dt}=+\frac{d[N{{h}_{3}}]}{2dt}\] \[\frac{-d[{{N}_{2}}]}{dt}=\frac{d[N{{H}_{3}}]}{2dt}\] \[=\frac{2.0\times {{10}^{-4}}}{2}=1.0\times {{10}^{-4}}M{{s}^{-1}}\]
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