For a first order reaction A→ProductsA \rightarrow \text{Products}A→Products, initial concentration of AAA is 0.1 M0.1 \text{ M}0.1 M, which becomes 0.001 M0.001 \text{ M}0.001 M after 5 minutes5 \text{ minutes}5 minutes. Rate constant for the reaction in min−1\text{min}^{-1}min−1 is
1.38181.38181.3818
0.92120.92120.9212
0.46060.46060.4606
0.23030.23030.2303
For a first order reaction, k=2.303tlog[A]0[A]tk = \frac{2.303}{t} \log \frac{[A]_0}{[A]_t}k=t2.303log[A]t[A]0. Given [A]0=0.1 M[A]_0 = 0.1 \text{ M}[A]0=0.1 M, [A]t=0.001 M[A]_t = 0.001 \text{ M}[A]t=0.001 M, t=5 mint = 5 \text{ min}t=5 min. k=2.3035log0.10.001=2.3035log(100)=2.303×25=4.6065=0.9212 min−1k = \frac{2.303}{5} \log \frac{0.1}{0.001} = \frac{2.303}{5} \log(100) = \frac{2.303 \times 2}{5} = \frac{4.606}{5} = 0.9212 \text{ min}^{-1}k=52.303log0.0010.1=52.303log(100)=52.303×2=54.606=0.9212 min−1.
Join thousands of students and practice with AI-generated mock tests.