A) \[3.2\times {{10}^{-4}}{{s}^{-1}}\]
B) \[6.4\times {{10}^{-4}}{{s}^{-1}}\]
C) \[8.5\times {{10}^{-4}}{{s}^{-1}}\]
D) \[12.8\times {{10}^{-4}}{{s}^{-1}}\]
Correct Answer: B
Solution :
\[2{{N}_{2}}{{O}_{5}}\xrightarrow{{}}4N{{O}_{2}}+{{O}_{2}}\] Since, rate of above reaction is directly proportional to \[[{{N}_{2}}{{O}_{5}}]\], therefore reaction is of first order. rate constant, \[k=\frac{2.303}{t}\log \frac{a}{a-x}\] \[=\frac{2.303}{3600}\log \frac{100}{100-90}\] \[=\frac{2.303}{3600}\log 10\] \[=\frac{2.303}{3600}\times 1=0.00064\] \[=6.4\times {{10}^{-4}}\,\,{{s}^{-1}}\]
You need to login to perform this action.
You will be redirected in
3 sec
