TS EAMCET · Chemistry · Chemical Kinetics
The reaction \(2 \mathrm{~A} \rightarrow 2 \mathrm{~B}+\mathrm{C}\) has a rate constant of \(1.2 \times 10^{-2} \mathrm{~s}^{-1}\). Which of the following is correct?
- A Plot of \([\mathrm{A}]\) vs \(" \frac{1}{t}\) " will be straight line
- B Plot of \(\frac{1}{[\mathrm{~A}]}\) vs \(t^2\) will be a straight line
- C Plot of \(\ln [\mathrm{A}]\) vs \(t\) will be a straight line
- D Plot of [A] vs \(t^2\) will be a straight line
Answer & Solution
Correct Answer
(C) Plot of \(\ln [\mathrm{A}]\) vs \(t\) will be a straight line
Step-by-step Solution
Detailed explanation
\(\mathrm{K}=1.2 \times 10^{-2} \mathrm{~s}^{-1}\); This is a 1 st order reaction. Hence, \([\mathrm{A}]=[\mathrm{A}]_0 \mathrm{e}^{-\mathrm{kt}} ; \ln [\mathrm{A}]=\ln [\mathrm{A}]_0-\mathrm{kt}\) \(\therefore \quad \ln [\mathrm{A}]\) vs \(\mathrm{t}\) is a straight line with…
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