A) \[1.4\]
B) \[1.2\]
C) \[0.8\]
D) \[0.04\]
Correct Answer: C
Solution :
For the first order reaction, \[2{{N}_{2}}{{O}_{5}}\xrightarrow{{}}4N{{O}_{2}}+{{O}_{2}}\] Rate \[\frac{dx}{dt}=K[{{N}_{2}}{{O}_{5}}]\] ?...(1) Given, \[\frac{dx}{dt}=2.40\times {{10}^{-5}}mol\,litr{{e}^{-1}}{{\sec }^{-1}}\] \[K=3.0\times {{10}^{-5}}{{\sec }^{-1}}\] \[[{{N}_{2}}{{O}_{5}}]=?\] Substituting these value in equation (1) \[2.4\times {{10}^{-5}}mol\,litr{{e}^{-1}}{{\sec }^{-1}}\] \[=3\times {{10}^{-5}}{{\sec }^{-1}}\times [{{N}_{2}}{{O}_{5}}]\] or \[[{{N}_{2}}{{O}_{5}}]=\frac{2.4\times {{10}^{-5}}\,mol\,litr{{e}^{-1}}\,{{\sec }^{-1}}}{3.0\times {{10}^{-5}}{{\sec }^{-1}}}\] \[=0.8\,mol\,litr{{e}^{-1}}\]You need to login to perform this action.
You will be redirected in
3 sec