320352 A first order reaction is \(25 \%\) completed in 40 minutes. What is the rate constant \(\mathrm{k}\) for the reaction?

320353 The time required for \(60 \%\) completion of a first order reaction is \(50 \mathrm{~min}\). The time required for \(93.6 \%\) completion of the same reaction will be

320354 For a reaction \(\mathrm{A} \rightarrow\) product, rate constant is \(2 \times 10^{-2} \mathrm{~s}^{-1}\). The initial concentration of \(\mathrm{A}\) is \({\text{1}}{\text{.0 mol d}}{{\text{m}}^{{\text{ - 3}}}}\). What is the value of \(\log \dfrac{1}{[\mathrm{~A}]_{\mathrm{t}}}\) after 100 seconds?

320355 The rate constant for a first order reaction is \(4.606 \times 10^{-3} \mathrm{~s}^{-1}\). The time required to reduce \(2.0 \mathrm{~g}\) of the reactant to \(0.2 \mathrm{~g}\) is:

320352 A first order reaction is \(25 \%\) completed in 40 minutes. What is the rate constant \(\mathrm{k}\) for the reaction?

320353 The time required for \(60 \%\) completion of a first order reaction is \(50 \mathrm{~min}\). The time required for \(93.6 \%\) completion of the same reaction will be

320354 For a reaction \(\mathrm{A} \rightarrow\) product, rate constant is \(2 \times 10^{-2} \mathrm{~s}^{-1}\). The initial concentration of \(\mathrm{A}\) is \({\text{1}}{\text{.0 mol d}}{{\text{m}}^{{\text{ - 3}}}}\). What is the value of \(\log \dfrac{1}{[\mathrm{~A}]_{\mathrm{t}}}\) after 100 seconds?

320355 The rate constant for a first order reaction is \(4.606 \times 10^{-3} \mathrm{~s}^{-1}\). The time required to reduce \(2.0 \mathrm{~g}\) of the reactant to \(0.2 \mathrm{~g}\) is:

320352 A first order reaction is \(25 \%\) completed in 40 minutes. What is the rate constant \(\mathrm{k}\) for the reaction?

320353 The time required for \(60 \%\) completion of a first order reaction is \(50 \mathrm{~min}\). The time required for \(93.6 \%\) completion of the same reaction will be

320354 For a reaction \(\mathrm{A} \rightarrow\) product, rate constant is \(2 \times 10^{-2} \mathrm{~s}^{-1}\). The initial concentration of \(\mathrm{A}\) is \({\text{1}}{\text{.0 mol d}}{{\text{m}}^{{\text{ - 3}}}}\). What is the value of \(\log \dfrac{1}{[\mathrm{~A}]_{\mathrm{t}}}\) after 100 seconds?

320355 The rate constant for a first order reaction is \(4.606 \times 10^{-3} \mathrm{~s}^{-1}\). The time required to reduce \(2.0 \mathrm{~g}\) of the reactant to \(0.2 \mathrm{~g}\) is:

320352 A first order reaction is \(25 \%\) completed in 40 minutes. What is the rate constant \(\mathrm{k}\) for the reaction?

320353 The time required for \(60 \%\) completion of a first order reaction is \(50 \mathrm{~min}\). The time required for \(93.6 \%\) completion of the same reaction will be

320354 For a reaction \(\mathrm{A} \rightarrow\) product, rate constant is \(2 \times 10^{-2} \mathrm{~s}^{-1}\). The initial concentration of \(\mathrm{A}\) is \({\text{1}}{\text{.0 mol d}}{{\text{m}}^{{\text{ - 3}}}}\). What is the value of \(\log \dfrac{1}{[\mathrm{~A}]_{\mathrm{t}}}\) after 100 seconds?

320355 The rate constant for a first order reaction is \(4.606 \times 10^{-3} \mathrm{~s}^{-1}\). The time required to reduce \(2.0 \mathrm{~g}\) of the reactant to \(0.2 \mathrm{~g}\) is: