For the reaction $2A + B \to 2C + D$, rate = $6 \times 10^{-4}$ mol dm⁻³ s⁻¹ at $[A] = [B] = 0.3$ M. If the reaction is first order in A and zero order in B, $k$ equals:
A$6 \times 10^{-3}$ s⁻¹
B$1 \times 10^{-3}$ s⁻¹
C$3 \times 10^{-3}$ s⁻¹
D$2 \times 10^{-3}$ s⁻¹
Answer & Solution
Correct answer: D. $2 \times 10^{-3}$ s⁻¹
rate = $k[A]$ ⇒ $k = (6\times10^{-4})/0.3 = 2\times10^{-3}$ s⁻¹.
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