Answer the following questions: For a given first order reaction, it takes 5 minutes for the…
Answer the following questions:
(i)
For a given first order reaction, it takes 5 minutes for the initial concentration of $0\cdot6\text{ moles litre}^{-1}$ to become $0\cdot2\text{ moles litre}^{-1}$. Calculate the rate constant for this reaction.
(ii)
Find the overall order of the reactions which have the following rate law equations:
(a) $\text{Rate} = k[A]^{1/2}[B]^{3/2}$
(b) $\text{Rate} = k[A]^{3/2}[B]^{-1}$
Answer
Answer (i)
AIWritten by AI (gemini) - it can contain mistakes.
For a first order reaction:
$k = \frac{2\cdot303}{t} \log \frac{[A]_0}{[A]} = \frac{2\cdot303}{5} \log \frac{0\cdot6}{0\cdot2} = \frac{2\cdot303}{5} \log 3 = \frac{2\cdot303 \times 0\cdot4771}{5} = 0\cdot2198\text{ min}^{-1}$
Final answer: 0.2198 min-1
Final answer: 0.2198 min-1
Answer (ii)
AIWritten by AI (gemini) - it can contain mistakes.
Overall order:
(a) $\text{Rate} = k[A]^{1/2}[B]^{3/2} \Rightarrow \text{Overall order} = \frac{1}{2} + \frac{3}{2} = 2$ (second order).
(b) $\text{Rate} = k[A]^{3/2}[B]^{-1} \Rightarrow \text{Overall order} = \frac{3}{2} - 1 = \frac{1}{2}$ (half order).
From ISC 2027 Specimen Chemistry Paper 1, question 13.