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for the reaction N(2)O(5)(g) to 2NO(2...

for the reaction
`N_(2)O_(5)(g) to 2NO_(2)(g)+(1)/(2)O_(2)(g)`
the value of rate of disappearance of `N_(2)O_(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

A

`6.25xx10^(-3)mol L^(-1)S^(-1) and 6.25xx10^(-3)mol L^(-1)S^(-1)`

B

`1.25xx10^(-3)mol L^(-1)S^(-1) and 3.125xx10^(-3)mol L^(-1)S^(-1)`and

C

`6.25xx10^(-3)mol L^(-1)S^(-1) and 3.125xx10^(-3)mol L^(-1)S^(-1)`and

D

`1.25xx10^(-3)mol L^(-1)S^(-1) and 6.25xx10^(-3)mol L^(-1)S^(-1)`and

Text Solution

Verified by Experts

The correct Answer is:
B
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)`
`therefore (d[NO_(2)])/(dt)=-(2d[N_(2)O_(5)])/(dt)=1.25xx10^(-2)molL^(-1)S^(-)`
`therefore (d[O_(2)])/(dt)=-(1)/(2)(d[N_(2)O_(5)])/(dt)`
`=3.12510^(-3)molL^(-1)S^(-1)`
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