A reaction in which a, b, and c react to form products is zero order in a, one-half order in b, and second order in

c. by what factor does the reaction rate change if [b] is doubled (and the other reactant concentrations are held constant) ? - g

For the reaction: A + B + C = products

when the rate law is:

r = K [A]^0 [B]^0.5 [C]^2

= K [B]^0.5 [C]^2

so the overall order of the reaction is 0 + 0.5 + 2 = 2.5

when the concentration of B is doubled and the concentrations of A and C are held constant so,

r1 = [B (1) ]^0.5 and r2 = [B (2) ]^0.5

∴ r2/r1 = [B (2) ]^0.5 / [B (1) ]^0.5 = 2^0.5 / 1^0.5 = 1.414

∴ the reaction will speed up 1.414 times