During the kinetic study of the reaction, 2A + B → C + D, following results were obtained:

Run | [A]/mol L⁻¹ | [B]/mol L⁻¹ | Initial rate of formation of D/mol L⁻¹ min⁻¹
I | 0.1 | 0.1 | 6.0 × 10⁻³
II | 0.3 | 0.2 | 7.2 × 10⁻²
III | 0.3 | 0.3

Question

During the kinetic study of the reaction, 2A + B → C + D, following results were obtained:

Run | [A]/mol L⁻¹ | [B]/mol L⁻¹ | Initial rate of formation of D/mol L⁻¹ min⁻¹
I   | 0.1         | 0.1         | 6.0 × 10⁻³
II  | 0.3         | 0.2         | 7.2 × 10⁻²
III | 0.3         | 0.3         | 2.88 × 10⁻¹
IV  | 0.4         | 0.1         | 2.40 × 10⁻²

Based on the above data which one of the following is correct?

Accepted Answer

rate = k[A]²[B]. By analyzing the data, the rate is proportional to [A]² and [B]. Doubling [A] quadruples the rate, and doubling [B] doubles the rate, confirming rate = k[A]²[B].

Solution

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