Question

Given the data below for the reaction, 2 A + 2 B + 4 C =>...

Given the data below for the reaction, 2 A + 2 B + 4 C => D + E + 3 F,

Experiment Initial conc of A, mol/L Initial conc of B, mol/L Initial conc of C, mol/L Initial rate, mol/L.s
1 0.1 0.2 0.4 2 x 10-3
2 0.2 0.2 0.4 8 x 10-3
3 0.3 0.4 0.4 1.8 x 10-2
4 0.4 0.6 0.2 1.6 x 10-2


Calculate the value of k to 3 significant figures

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Homework Answers

Answer #1

let the rate equation be,

rate = k[A]^x.[B]^y.[C]^z

with,

k = rate constant

x, y and z are order with respect to [A]. [B] and [C]

From experiment 1 an 2, [B] and [C] are constant

rate1/rate2 = 2 x 10^-3/8 x 10^-3 = (0.1/0.2)^x

taking log of both sides and solving for x,

x = 2

From experiment 2 and 3, [C] is consant,

rate2/rate3 = 8 x 10^-3/1.8 x 10^-2 = (0.2/0.3)^2.(0.2/0.4)^y

taking log of both sides and solving for y,

y = 3

From experiment 3 and 4,

rate3/rate4 = 1.8 x 10^-2/1.6 x 10^-2 = (0.3/0.4)^2.(0.4/0.6)^3.(0.4/0.2)^z

taking log of both sides and solving for z,

z = 1

Thus, the rate equation will be,

rate = k[A]^2.[B]^3.[C]^1

rate constant k = 1.6 x 10^-2/(0.4)^2.(0.6)^3.(0.2) = 2.315

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