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For the reaction, 2A + B+C rarr A(2)B+C ...

For the reaction, `2A + B+C rarr A_(2)B+C`
The rate `= k[A][B]^(2)` with `K = 2.0 xx 10^(-6) M^(-2) s^(-1)`. Calculate the initial rate of the reaction when `[A] = 0.1M, [B] = 0.2M` and `[C] = 0.8M`. IF the rate of reverse reaction is negligible then calculate the rate of reaction after `[A]` is reduced to `0.06M`.

Text Solution

Verified by Experts

Rate `=K[A][B]^(2)`
`[A]=0.1 M, [B]=0.2M, K=2.0xx10^(-6)`
`:.` Initial rate `=2.0xx10^(-6)xx0.1xx(0.2)^(2)`
`=8xx10^(-9) mol litre^(-1) time^(-1)`
New rate when `A` is reduced to `0.06 M` and `B` is `0.18M`. See stoichiometry of reaction.
Rate=`2.0xx10^(-6)xx(0.06)xx(0.18)^(2)`
`=3.89xx10^(-9) mol litre^(-1) time^(-1)`
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