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.

Options

A. Rate `= K[A]^(2)[B]`
B. Rate `= K[A][B]^(2)`
C. Rate `= K[A][B]`
D. Rate `= K[A]^(2)[B]^(0)`

Answer

B

Explanation

Rate of reactions 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)}`
`" "(0.14)/(0.40) = ([0.30]^(x))/([0.60]^(y))`
`" " (1)/(4) = [(1)/(4)]^(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`
`therefore " ""Rate " = k [A]^(x) [B]^(y)`
`" ""Rate" = k[A]^(1)[B]^(2)`