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Compounds 'A' and 'B' react according ...

Compounds 'A' and 'B' react according to the following chemical equation.
`A(g) to 2B(g) to 2C(g)`
Concentration of either 'A' or 'B' were changed Keeping the concentration of one of the reactants constant and rates were measured as a function of initial concentration. Following result were obtained.
Choose the correct option for the rate equations for this reaction.

A

Rate = `k[A]^(2)[B]`

B

Rate = `k[A][B]^(2)`

C

Rate = `k[A][B]`

D

Rate = `k[A]^(2)[B]^(0)`

Text Solution

Verified by Experts

The correct Answer is:
B
Rate of reaction is change in concentration of reactant with respect to time .
`r=k[A]^(x)[B]^(y)`
`("Rate of exp".1)/("Rate of exp".2)=([0.30]^(x)[0.30]^(y))/([0.30]^(x)[0.60]^(y))`
`(0.10)/(0.40)=([0.30]^(y))/([0.60]^(y))`
`(1)/(4)=[(1)/(2)]^(y)`
`[(1)/(2)]^(2)=[(1)/(2)]^(y)`
`y=2`
`("Rate of exp".1)/("Rate of exp".3)=([0.30]^(x)[0.30]^(y))/([0.60]^(x)[0.30]^(y))`
`(0.10)/(0.20)=[(0.30)/(0.60)]^(x)[(0.30)/(0.30)]^(y)`
`(1)/(2)=[(1)/(2)]^(x)[1]^(y)`
`(1)/(2)=[(1)/(2)]^(x)`
i.e., `x=1`
:. Rate = `k[A]^(x)[B]^(y)`
Rate = `K[A]^(1)[B]^(2)`
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