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
