question_answer

For the reaction \[\underset{(g)}{\mathop{{{N}_{2}}{{O}_{5}}}}\,\xrightarrow{{}}\underset{(g)}{\mathop{2N{{O}_{2}}}}\,+\underset{(g)}{\mathop{\frac{1}{2}{{O}_{2}}}}\,,\] the rate of disappearance of \[{{N}_{2}}{{O}_{5}}\]is\[6.25\times {{10}^{-3}}\,mol\,{{L}^{-1}}{{s}^{-1}}\].  The rate of formation of \[N{{O}_{2}}\]and \[{{O}_{2}}\] will be respectively.

A) \[6.25\times {{10}^{-3}}\,mol\,{{L}^{-1}}{{s}^{-1}}\]and \[6.25\times {{10}^{-3}}\,mol\,{{L}^{-1}}{{s}^{-1}}\]

B)  \[1.25\times {{10}^{-2}}mol\,{{L}^{-1}}{{s}^{-1}}\]and \[3.125\times {{10}^{-3}}\]\[mol{{L}^{-1}}{{s}^{-1}}\]

C)  \[6.25\times {{10}^{-3}}mol{{L}^{-1}}{{s}^{-1}}\]and \[3.125\times {{10}^{-3}}\]\[mol\,{{L}^{-1}}{{s}^{-1}}\]

D)  \[1.25\times {{10}^{-2}}mol{{L}^{-1}}{{s}^{-1}}\]and \[6.25\times {{10}^{-3}}mol\,{{L}^{-1}}{{s}^{-1}}\]