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For a gaseous phase, first order reactio...

For a gaseous phase, first order reaction,
`A_((g))rarr B_((g))+2C_((g))` (rate constant `K=10^(-2) time^(-1)`)
in a closed vessel of `2` litre containing `5` moles of `A_((g))` at `27^(@)C`. then correct statements:

A

(a) Rate of disappearrance of `A_((g))` is `6.15xx10^(-3) atm t^(-1)`

B

(b) Rate of disappearance of `C_((g))` is `5.0xx10^(-2) mol litre^(-1) t^(-1)`

C

(c ) Rate of disappearance of `B_((g))` is `5.0xx10^(-2) mol litre^(-1) t^(-1)`

D

(d) Rate of disappearance of `A_((g))` is `5.0xx10^(-2) mol^(-1) t^(-1)`

Text Solution

Verified by Experts

The correct Answer is:
a, d
Rate of reaction `=-(d[A])/(dt)+(d[B])/(dt)=+1/2(d[C])/(dt)`
Also rate of reaction,
`-(d[A])/(dt)=K[A]^(1)=10^(-2)xx5/2`
`=2.5xx10^(-2) mol litre^(-1) t^(-1)`
`:' P=CRT`
`:. (-d[A])/(dt)=-1/(RT).(d[P])/(dt)`
`:. (-d[P_(A)])/(dt)=RT(d[A])/(dt)`
`=0.0821xx300xx2.5xx10^(-2)`
`=6.15xx10^(-1) atm t^(-1)`
`-(d[A])/(dt)=-(d[n])/(V. dt)`
`:. -(d[n_(A)])/(dt)=V.(d[A])/(dt)=2xx2.5xx10^(-2)`
`=5.0xx10^(-2) mol t^(-1)`
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