320282 The temperature dependence of rate constant \((\mathrm{k})\) of a chemical reaction is written in terms of Arrhenius equation \(\mathrm{k}=\mathrm{Ae}^{-\mathrm{E}_{\mathrm{a}} / \mathrm{RT}}\). Activation energy \(\left(E_{a}\right)\) of the reaction can be calculated by plotting.

320283 Oxygen is available in plenty in air yet fuels do not burn by themselves at room temperature. Because

320284 The rate constant \((\mathrm{k})\) for a particular reaction is \(1.3 \times 10^{-4} \mathrm{M}^{-1} \mathrm{~s}^{-1}\) at \(\quad 100^{\circ} \mathrm{C}, \quad\) and \(1.3 \times 10^{-3} \mathrm{M}^{-1} \mathrm{~s}^{-1}\) at \(150^{\circ} \mathrm{C}\). What is the energy of activation \(\left(\mathrm{E}_{\mathrm{a}}\right)\) (in \(\mathrm{kJ}\) ) for the reaction? \(\left(\mathrm{R}=8.314 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}\right)\)

320285 A chemical reaction was carried out at \(300 \mathrm{~K}\) and \(280 \mathrm{~K}\). The rate constants were found to be \({{\text{k}}_1}\) and \({{\text{k}}_2}\) respectively. Then

320286 Following are two first order reactions with their half-life times given at \({\mathrm{25^{\circ} \mathrm{C}}}\).
\({\mathrm{\mathrm{A} \xrightarrow{t / 2=30 \mathrm{~min}}}}\) Products
\({\mathrm{\mathrm{B} \xrightarrow{t_{1 / 2}=40 \mathrm{~min}}}}\) Products
The temperature coefficients of their reaction rates are 3 and 2 , respectively, between \({\mathrm{25^{\circ} \mathrm{C}}}\) and \({\mathrm{35^{\circ} \mathrm{C}}}\). If the above two reactions are carried out taking 0.4 M of each reactant but at different temperatures: \({\mathrm{25^{\circ} \mathrm{C}}}\) for the first order reaction and \({\mathrm{35^{\circ} \mathrm{C}}}\) for the second order reaction, find the ratio of the concentrations of \({\mathrm{A}}\) and \({\mathrm{B}}\) after an hour.

320282 The temperature dependence of rate constant \((\mathrm{k})\) of a chemical reaction is written in terms of Arrhenius equation \(\mathrm{k}=\mathrm{Ae}^{-\mathrm{E}_{\mathrm{a}} / \mathrm{RT}}\). Activation energy \(\left(E_{a}\right)\) of the reaction can be calculated by plotting.

320283 Oxygen is available in plenty in air yet fuels do not burn by themselves at room temperature. Because

320284 The rate constant \((\mathrm{k})\) for a particular reaction is \(1.3 \times 10^{-4} \mathrm{M}^{-1} \mathrm{~s}^{-1}\) at \(\quad 100^{\circ} \mathrm{C}, \quad\) and \(1.3 \times 10^{-3} \mathrm{M}^{-1} \mathrm{~s}^{-1}\) at \(150^{\circ} \mathrm{C}\). What is the energy of activation \(\left(\mathrm{E}_{\mathrm{a}}\right)\) (in \(\mathrm{kJ}\) ) for the reaction? \(\left(\mathrm{R}=8.314 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}\right)\)

320285 A chemical reaction was carried out at \(300 \mathrm{~K}\) and \(280 \mathrm{~K}\). The rate constants were found to be \({{\text{k}}_1}\) and \({{\text{k}}_2}\) respectively. Then

320286 Following are two first order reactions with their half-life times given at \({\mathrm{25^{\circ} \mathrm{C}}}\).
\({\mathrm{\mathrm{A} \xrightarrow{t / 2=30 \mathrm{~min}}}}\) Products
\({\mathrm{\mathrm{B} \xrightarrow{t_{1 / 2}=40 \mathrm{~min}}}}\) Products
The temperature coefficients of their reaction rates are 3 and 2 , respectively, between \({\mathrm{25^{\circ} \mathrm{C}}}\) and \({\mathrm{35^{\circ} \mathrm{C}}}\). If the above two reactions are carried out taking 0.4 M of each reactant but at different temperatures: \({\mathrm{25^{\circ} \mathrm{C}}}\) for the first order reaction and \({\mathrm{35^{\circ} \mathrm{C}}}\) for the second order reaction, find the ratio of the concentrations of \({\mathrm{A}}\) and \({\mathrm{B}}\) after an hour.

320282 The temperature dependence of rate constant \((\mathrm{k})\) of a chemical reaction is written in terms of Arrhenius equation \(\mathrm{k}=\mathrm{Ae}^{-\mathrm{E}_{\mathrm{a}} / \mathrm{RT}}\). Activation energy \(\left(E_{a}\right)\) of the reaction can be calculated by plotting.

320283 Oxygen is available in plenty in air yet fuels do not burn by themselves at room temperature. Because

320284 The rate constant \((\mathrm{k})\) for a particular reaction is \(1.3 \times 10^{-4} \mathrm{M}^{-1} \mathrm{~s}^{-1}\) at \(\quad 100^{\circ} \mathrm{C}, \quad\) and \(1.3 \times 10^{-3} \mathrm{M}^{-1} \mathrm{~s}^{-1}\) at \(150^{\circ} \mathrm{C}\). What is the energy of activation \(\left(\mathrm{E}_{\mathrm{a}}\right)\) (in \(\mathrm{kJ}\) ) for the reaction? \(\left(\mathrm{R}=8.314 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}\right)\)

320285 A chemical reaction was carried out at \(300 \mathrm{~K}\) and \(280 \mathrm{~K}\). The rate constants were found to be \({{\text{k}}_1}\) and \({{\text{k}}_2}\) respectively. Then

320286 Following are two first order reactions with their half-life times given at \({\mathrm{25^{\circ} \mathrm{C}}}\).
\({\mathrm{\mathrm{A} \xrightarrow{t / 2=30 \mathrm{~min}}}}\) Products
\({\mathrm{\mathrm{B} \xrightarrow{t_{1 / 2}=40 \mathrm{~min}}}}\) Products
The temperature coefficients of their reaction rates are 3 and 2 , respectively, between \({\mathrm{25^{\circ} \mathrm{C}}}\) and \({\mathrm{35^{\circ} \mathrm{C}}}\). If the above two reactions are carried out taking 0.4 M of each reactant but at different temperatures: \({\mathrm{25^{\circ} \mathrm{C}}}\) for the first order reaction and \({\mathrm{35^{\circ} \mathrm{C}}}\) for the second order reaction, find the ratio of the concentrations of \({\mathrm{A}}\) and \({\mathrm{B}}\) after an hour.

320282 The temperature dependence of rate constant \((\mathrm{k})\) of a chemical reaction is written in terms of Arrhenius equation \(\mathrm{k}=\mathrm{Ae}^{-\mathrm{E}_{\mathrm{a}} / \mathrm{RT}}\). Activation energy \(\left(E_{a}\right)\) of the reaction can be calculated by plotting.

320283 Oxygen is available in plenty in air yet fuels do not burn by themselves at room temperature. Because

320284 The rate constant \((\mathrm{k})\) for a particular reaction is \(1.3 \times 10^{-4} \mathrm{M}^{-1} \mathrm{~s}^{-1}\) at \(\quad 100^{\circ} \mathrm{C}, \quad\) and \(1.3 \times 10^{-3} \mathrm{M}^{-1} \mathrm{~s}^{-1}\) at \(150^{\circ} \mathrm{C}\). What is the energy of activation \(\left(\mathrm{E}_{\mathrm{a}}\right)\) (in \(\mathrm{kJ}\) ) for the reaction? \(\left(\mathrm{R}=8.314 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}\right)\)

320285 A chemical reaction was carried out at \(300 \mathrm{~K}\) and \(280 \mathrm{~K}\). The rate constants were found to be \({{\text{k}}_1}\) and \({{\text{k}}_2}\) respectively. Then

320286 Following are two first order reactions with their half-life times given at \({\mathrm{25^{\circ} \mathrm{C}}}\).
\({\mathrm{\mathrm{A} \xrightarrow{t / 2=30 \mathrm{~min}}}}\) Products
\({\mathrm{\mathrm{B} \xrightarrow{t_{1 / 2}=40 \mathrm{~min}}}}\) Products
The temperature coefficients of their reaction rates are 3 and 2 , respectively, between \({\mathrm{25^{\circ} \mathrm{C}}}\) and \({\mathrm{35^{\circ} \mathrm{C}}}\). If the above two reactions are carried out taking 0.4 M of each reactant but at different temperatures: \({\mathrm{25^{\circ} \mathrm{C}}}\) for the first order reaction and \({\mathrm{35^{\circ} \mathrm{C}}}\) for the second order reaction, find the ratio of the concentrations of \({\mathrm{A}}\) and \({\mathrm{B}}\) after an hour.

320282 The temperature dependence of rate constant \((\mathrm{k})\) of a chemical reaction is written in terms of Arrhenius equation \(\mathrm{k}=\mathrm{Ae}^{-\mathrm{E}_{\mathrm{a}} / \mathrm{RT}}\). Activation energy \(\left(E_{a}\right)\) of the reaction can be calculated by plotting.

320283 Oxygen is available in plenty in air yet fuels do not burn by themselves at room temperature. Because

320284 The rate constant \((\mathrm{k})\) for a particular reaction is \(1.3 \times 10^{-4} \mathrm{M}^{-1} \mathrm{~s}^{-1}\) at \(\quad 100^{\circ} \mathrm{C}, \quad\) and \(1.3 \times 10^{-3} \mathrm{M}^{-1} \mathrm{~s}^{-1}\) at \(150^{\circ} \mathrm{C}\). What is the energy of activation \(\left(\mathrm{E}_{\mathrm{a}}\right)\) (in \(\mathrm{kJ}\) ) for the reaction? \(\left(\mathrm{R}=8.314 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}\right)\)

320285 A chemical reaction was carried out at \(300 \mathrm{~K}\) and \(280 \mathrm{~K}\). The rate constants were found to be \({{\text{k}}_1}\) and \({{\text{k}}_2}\) respectively. Then

320286 Following are two first order reactions with their half-life times given at \({\mathrm{25^{\circ} \mathrm{C}}}\).
\({\mathrm{\mathrm{A} \xrightarrow{t / 2=30 \mathrm{~min}}}}\) Products
\({\mathrm{\mathrm{B} \xrightarrow{t_{1 / 2}=40 \mathrm{~min}}}}\) Products
The temperature coefficients of their reaction rates are 3 and 2 , respectively, between \({\mathrm{25^{\circ} \mathrm{C}}}\) and \({\mathrm{35^{\circ} \mathrm{C}}}\). If the above two reactions are carried out taking 0.4 M of each reactant but at different temperatures: \({\mathrm{25^{\circ} \mathrm{C}}}\) for the first order reaction and \({\mathrm{35^{\circ} \mathrm{C}}}\) for the second order reaction, find the ratio of the concentrations of \({\mathrm{A}}\) and \({\mathrm{B}}\) after an hour.