Compounds 'A' and 'B' react according to the following chemical equation :
`A(g)+2" B"(g)to2C(g)`
Concentration of either 'A' or 'B' were changed keeping the concentrations of one of the reactants constant and rates were measured as a function of initial concentration. Following results 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

From expts. 1 and 3, [B] = constant, [A] = doubled, rate is doubled.
Hence, Rate `prop[A]`.
From expts. 1 and 2, [A] = constant, [B] = doubled, rate quadrupled.
Hence, Rate `prop[B]^(2)`.
Combining, Rate `=k[A][B]^(2)`.