For the reaction, `N_2O_5(g) rarr 2NO_2(g)+1//2O_2(g)`, the value of rate of disappearance of `N_2O_5` is given as `6.25xx10^(-3) "mol L"^(-1)s^(-1)`. The rate of formation of `NO_2 and O_2` is given respectively as

Options

A. `1.25xx10^(-2)molL^(-1)S^(-1)` and `6.25xx10^(-3)molL^(-1)S^(-1)`
B. `6.25xx10^(-3)molL^(-1)S^(-1)` and `6.25xx10^(-3)molL^(-1)S^(-1)`
C. `1.25xx10^(-2)molL^(-1)S^(-1)` and `3.125xx10^(-3)molL^(-1)S^(-1)`
D. `6.25xx10^(-3)molL^(-1)S^(-1)` and `3.125xx10^(-3)molL^(-1)S^(-1)`

Answer

C

Explanation

Given `(-d[N_(2)O_(5)])/(dt)=6.25xx10^(-3)molL^(-1)S^(-1)`
For the reaction, `N_(2)O_(5) to 2NO_(2)+(1)/(2)O_(2)`
`(-d[N_(2)O_(5)])/(dt)=(1)/(2)(d[NO_(2)])/(dt)=(2d[O_(2)])/(dt)`
`:.(d[NO_(2)])/(dt)=-(2d[N_(2)O_(5)])/(dt)=1.25xx10^(-2)molL^(-1)S^(-1)`
`:.(d[O_(2)])/(dt)=-(1)/(2)(d[N_(2)O_(5)])/(dt)=3.125xx10^(-3)molL^(-1)S^(-1)`.