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In the reaction , A+2Bto6C+2D, if the in...

In the reaction , `A+2Bto6C+2D`, if the initial rate `-(d[A])/(dt)` at t= 0 is `2.6xx10^(-2)Msec^(-1)`, what will be the value of `-(d[B])/(dt)` at t=0?

A

`8.5 xx 10^(-2)m sec^(-1)`

B

`2.5 xx 10^(-2) msec^(-1)`

C

`5.2 xx 10^(-2) m sec^(-1)`

D

`7.5 xx 10^(-2) m sec^(-1)`

Text Solution

Verified by Experts

The correct Answer is:
C
From the reaction it is evident that when a mole of A is reacting, 2 moles of B must react. Hence the decrease in the concentration of B must be twice that of A
`:. -(d[B])/(dt)= 2 [ - (d[A])/(dt)] = 2 xx 10^(-2) = 5.2 xx 10^(-2) sec^(-1)`
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