## Chemistry: Molecular Approach (4th Edition)

The answers are: a. Rate =$k [B]^{1/2}[C] ^2$ b. 2.5 c. 1 d. 1.4 e. 4 f. 5.6
a. Rate of reaction = $k [A]^0[B] ^{1/2}[C]^2$ = $k [B]^{1/2}[C] ^2$ b. Overall order of reaction = sum of individual orders = 0+1/2+2 = 2.5 c. The reaction is zeroth order in $A$. So, doubling the concentration of $A$ increases the rate by 1 times. d. The reaction is 1/2 order in $B$. So, doubling the concentration of $B$ increases the rate by $2^{1/2}$ = 1.4 times. e. The reaction is second order in $C$. So, doubling the concentration of $C$ increases the rate by $2^2$ = 4 times. f. The reaction is 2.5 order overall. So, doubling the concentration of all reactants increases the rate by $2^{2.5}$ = 5.6 times.