A) \[1.732\,mol\,{{L}^{-1}}\]
B) \[3\,mol\,{{L}^{-1}}\]
C) \[1.02\times {{10}^{-4}}\,mol\,{{L}^{-1}}\]
D) \[3.2\times {{10}^{5}}\,mol\,{{L}^{-1}}\]
Correct Answer: B
Solution :
For reaction, \[2{{N}_{2}}{{O}_{5}}\xrightarrow{{}}4N{{O}_{2}}+{{O}_{2}}\] Given that, \[K=3.4\times {{10}^{-5}}{{\sec }^{-1}}\] (i.e., reaction is of 1st order, as its unit is\[{{\sec }^{-1}}\]) \[r=1.02\times {{10}^{-4}}\,mol\,{{L}^{-1}}{{s}^{-1}}\] We know that, \[r=K\cdot [{{N}_{2}}{{O}_{5}}]\] (for 1st order reaction) \[\therefore \] \[[{{N}_{2}}{{O}_{5}}]=\frac{1.02\times {{10}^{-4}}}{3.4\times {{10}^{-5}}}=3\,mol\,{{L}^{-1}}\]
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