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The rate equation for the decomposition ...

The rate equation for the decomposition of `N_(2)O_(5)` in `"CC"l_(4)` is rate `=K[N_(2)O_(4)]` where `K=6.3x10^(-4)s^(-1)` at 320 K. what would be the initial rate of decompositioni of `N_(2)O_(5)` in a 1.10 M solution of `N_(2)O_(4)`?

A

`6.3xx10^(-5)` mol `"litre"^(-1)s^(-1)`

B

`0.63xx10^(-6)` mol `"litre"^(-1)s^(-1)`

C

`6.3xx10^(-5)` mol `"litre"^(-1)s^(-1)`

D

`0.63xx10^(-4)` mol `"litre"^(-1)s^(-1)`

Text Solution

Verified by Experts

The correct Answer is:
C, D
`r=K.[N_(2)O_(5)]=6.3xx10^(-4)xx(0.10)^(1)=6.3xx10^(-5)`
`1N_(2)O_(5)to2NO_(2)+1/2O_(2)`
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