A chemical reaction `2A rarr 4B` +C in gas phase occurs in a closed vessel the concentration of B is found to increase by `2.5 xx10^(-3) mol L^(-1)` in 5 second calculate (i) the rate of appearance of B (ii) the rate of disappearance of A

Explanation

Average of reaction w.r.t B=`(triangle[B])/(trianglet)`
Hence `triangle[B]=2.5 xx10^(-3) mol L^(-1)` and `triangle t=5s`
Average rate of reaction =`1/2 (triangle[A])/(trianglet)=1/4 (triangle[B])/(trianglet)=(triangle[C])/(trianglet)`
The average rate of disappearance of `A =(d[A])/(dt)=2xx` Average rate of reaction
`=2xx1.25 xx10^(-4) mol L^(-1) s^(-1) =2.5 xx10^(-4) mol L^(-1) s^(-1)`