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The rate law for a reaction of A, B and ...

The rate law for a reaction of A, B and C has been found to be rate `= [A]^(2)[B][L]^((3)/(2))`. How would the rate of reaction change when
Concentration of [A] is halved

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When `[A]=[(A)/(2)]`
Rate `=k[(A)/(2)]^(2)[B][L]^(3//2)`
Rate `=(1)/(4)(k[A^(2)][B][L]^(3//2)) " "` …(4)
Comparing (1) and (4) , rate is reduced to `(1)/(4)` times.
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