Answer
The answers are:
a. Rate =$ k [B]^{1/2}[C] ^2$
b. 2.5
c. 1
d. 1.4
e. 4
f. 5.6
Work Step by Step
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.
