The following results were obtained during kinetic studies of the reaction : 2A + B → Products Experiment I: [A] = 0.10 mol L⁻¹, [B] = 0.20 mol L⁻¹, Initial Rate of reaction = 6.93 × 10⁻³ mol L⁻¹ min⁻¹ Experiment II: [A] = 0.10 mol L⁻¹, [B] = 0.25 mol L⁻¹, Initial Rate of reaction = 6.93 ×

Question

The following results were obtained during kinetic studies of the reaction : 2A + B → Products Experiment I: [A] = 0.10 mol L⁻¹, [B] = 0.20 mol L⁻¹, Initial Rate of reaction = 6.93 × 10⁻³ mol L⁻¹ min⁻¹ Experiment II: [A] = 0.10 mol L⁻¹, [B] = 0.25 mol L⁻¹, Initial Rate of reaction = 6.93 × 10⁻³ mol L⁻¹ min⁻¹ Experiment III: [A] = 0.20 mol L⁻¹, [B] = 0.30 mol L⁻¹, Initial Rate of reaction = 1.386 × 10⁻² mol L⁻¹ min⁻¹ The time (in minutes) required to consume half of A is -

Accepted Answer

100. The correct option is 100 minutes because the rate of reaction is directly related to the concentration of reactants. Given the initial rates and concentrations, it indicates that the reaction is slow, and thus a longer time is needed to consume half of reactant A.

Solution

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