For the reaction `N_(2)O_(5) rarr 2NO_(2) + (1)/(2) O_(2)`, the rate of disappearance of `N_(2)O_(5)` is `6.25 xx 10^(-3) "mol L"^(-1) s^(-1)`. The rate of formation of `NO_(2)` and `O_(2)` will be respectively.

Options

A. `1.25 xx 10^(-2) "mol L"^(-1) s^(-1) and 6.25 xx 10^(-3) "mol L"^(-1)s^(-1)`
B. `6.25 xx 10^(-3) "mol L"^(-1) s^(-1) and 6.25 xx 10^(-3) "mol L"^(-1)s^(-1)`
C. `1.25 xx 10^(-2) "mol L"^(-1)s^(-1) and 3.125 xx 10^(-3) L^(-1)s^(-1)`
D. `6.25 xx 10^(-3) "mol L"^(-1) s^(-1) and 3.125 xx 10^(-3) "mol L"^(-1) s^(-1)`

Answer

C

Explanation

Rate `= (-d[N_(2)O_(5)])/(dt)=+(1)/(2)(d[NO_(2)])/(dt)=(2d[O_(2)])/(dt)`
Given `(-d[N_(2)O_(5)])/(dt)=6.25xx10^(-3)"mol L"^(-1)s^(-1)`
Rate of formation of `NO_(2)`
`(d[NO_(2)])/(dt)=-2(d[N_(2)O_(5)])/(dt)`
`=2xx6.25xx10^(-3)"mol L"^(-1)"s"^(-1)`
`=12.50xx10^(-3)"mol L"^(-1)s^(-1)`
`=1.25xx10^(-2)"mol L"^(-1)s^(-1)`
Rate of formation on `O_(2)`
`(d[O_(2)])/(dt)=-(1)/(2)(d[N_(2)O_(5)])/(dt)`
`=1//2xx6.25xx10^(-3)"mol L"^(-1)s^(-1)`
`=2.125xx10^(-3)xx10^(-3)"mol L"^(-1)s^(-1)`.