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The following data were obtained on the initial rates of a reaction of a d-metal complex in aqueous solution. What is (a) the order of reaction with respect to the complex and the reactant Y, (b) the rate constant? For the experiments a [Y]=2.7 mmol dm 3 and for experiments (b) [Y]=6.1 mmoldm (complex]/(mmol dm-3) v/mol dm-35-1) (a) (b) 8.01 125 640 9.22 144 730 12.11 190 960

Answer :

a) The order of the reaction with respect to the complex is 1 and order with respect to Y is 2.

b) The rate constant for reaction is 2.2 × 10⁹ mol⁻²dm⁶s⁻¹.

What is order of reaction and rate constant?

The order of reaction is defined as sum of the power raised to the concentration terms . The rate constant defined as the relation between concentration and rate of the reaction, and it is also temperature dependent.

Using Rate = K [complex]ᵃ [Y]ᵇ

a)  125 = K (8.01) ᵃ (2.7) ᵇ

144= K (9.22) ᵃ (2.7) ᵇ

Divide these two equations

125/144 = (8.01/ 9.22) ᵃ

(0.868) = (0.868) ᵃ

⇒ a= 1 order with respect to complex is 1

b)  R₂=K(complex)ᵃ(Y)ᵇ

125=K (8.01) (2.7) ᵇ

640=K (8.01) 6.1) ᵇ

Divide these two equations

we get, 0.195 = (0.443)ᵇ

⇒ b= 2 order with respect to Y is 2.

Now Rate constant

125=K (8.01) ¹ (2.7) ²

K = 2.2 ₓ 10⁹mol⁻²dm⁶s⁻¹.

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