For the following reaction: A+2B+3C+D --> E , the kinetics expression has been experimentally determined to be: rate = k[A]^2[B][C]^0.5

Question

a) What is the reaction order with respect to each of the reactants (A,B,C, and D)?

b) What is the overall order of the reaction?

c) If you were to double the initial concentration of A, half the initial concentration of B, quadruple the initial concentration of C, and double the initial concentration of D, how would the initial reaction rate be affected?

d) What do the brackets around the species mean?

e) Both equilibrium and kinetics expression use the same letters for their constants. How can you tell the difference between them if just shown the letter?

Answer 1

a) 2nd order with respect to A

1st order with respect to B

1/2 order with respect to C

zero order with respect to D

b) overall order = 3.5

c) doubling A = 4x increase

halving B = 1/2

quadrupling C = 2x increase

doubling D = no effect

Overall effect = 4 x 0.5 x 2 = 4 times increase in rate

d) brackets [ ] mean concentration, usually in moles/liter

e) I'm not sure I understand the question, but if they are referring to the constants, then equilibrium expressions use a capital K and kinetics use a small k.