| \[{{N}_{2}}{{O}_{5}}(g)\xrightarrow{{}}2N{{O}_{2}}(g)+1/2\,{{O}_{2}}(g)\] the value of rate of disappearance of \[{{N}_{2}}{{O}_{5}}\] is given as \[6.25\times {{10}^{-3}}mol\,{{L}^{-1}}{{s}^{-1}}\]. The rate of formation of \[N{{O}_{2}}\] and \[{{O}_{2}}\] is given respectively as: |
A) \[6.25\times {{10}^{-3}}mol\text{ }{{L}^{-1}}{{s}^{-1}}\] and \[6.25\times {{10}^{-3}}mol\text{ }{{L}^{-1}}{{s}^{-1}}\]
B) \[1.25\times {{10}^{-2}}mol\text{ }{{L}^{-1}}{{s}^{-1}}\] and \[3.125\times {{10}^{-3}}mol\text{ }{{L}^{-1}}{{s}^{-1}}\]
C) \[6.25\times {{10}^{-3}}mol\text{ }{{L}^{-1}}{{s}^{-1}}\] and \[3.125\times {{10}^{-3}}mol\text{ }{{L}^{-1}}{{s}^{-1}}\]
D) \[1.125\times {{10}^{-2}}mol\text{ }{{L}^{-1}}{{s}^{-1}}\]and \[6.25\times {{10}^{-3}}mol\text{ }{{L}^{-1}}{{s}^{-1}}\]
Correct Answer: B
Solution :
[b] \[{{N}_{2}}{{O}_{5}}\left( g \right)\xrightarrow{{}}2N{{O}_{2}}\left( g \right)+1/2{{O}_{2}}\left( g \right)\] \[-\frac{d}{dt}[{{N}_{2}}{{O}_{5}}]=+\frac{1}{2}\frac{d}{dt}[N{{O}_{2}}]=2\frac{d}{dt}[{{O}_{2}}]\] \[\frac{d}{dt}[N{{O}_{2}}]=1.25\times {{10}^{-2}}mol{{L}^{-1}}{{s}^{-1}}\] and \[\frac{d}{dt}[{{O}_{2}}]=3.125\times {{10}^{-3}}mol\,{{L}^{-1}}{{s}^{-1}}\]
You need to login to perform this action.
You will be redirected in
3 sec
