For a first order reaction, intercept of the graph between $\log…
For a first order reaction, intercept of the graph between $\log \left(\frac{[\mathrm{A}]_0}{[\mathrm{~A}]_{\mathrm{t}}} \mathrm{Y}\right.$-axis) and time. (X-axis) is equal to
$-\frac{\mathrm{k}}{2.303 \mathrm{~K}}$
$-\log [\mathrm{A}]_0$
zero
$\frac{2.303}{\mathrm{~K}}$
Solution
For $1^{\text {st }}$ order reaction,
$2.303 \log \frac{[\mathrm{A}]_0}{[\mathrm{~A}]_{\mathrm{t}}}=\mathrm{kt}$
$\log \frac{[\mathrm{A}]_0}{[\mathrm{~A}]_{\mathrm{t}}}=\frac{\mathrm{k}}{2.303} \cdot \mathrm{t}, \mathrm{y}=\mathrm{mx} ; \quad \mathrm{C}=0[\text { Intercept }=0]$