320252 The activation energy for a simple chemical
reaction \(\mathrm{A} \rightarrow \mathrm{B}\) is \(\mathrm{E}_{\mathrm{a}}\) in forward direction. The
activation energy for reverse reaction

320253 The decomposition of\({{\text{N}}_{\text{2}}}{\text{O}}\,\,{\text{into }}{{\text{N}}_{\text{2}}}\) and in presence gaseous argon follow second order kinetics with \({\rm{k = }}\left( {{\rm{5}}{\rm{.0 \times 1}}{{\rm{0}}^{{\rm{11}}}}\,{\rm{L}}\,{\rm{mo}}{{\rm{l}}^{{\rm{ - 1}}}}\;{{\rm{s}}^{{\rm{ - 1}}}}} \right){{\rm{e}}^{{\rm{ - }}\frac{{{\rm{41570}}}}{{\rm{T}}}}}{\rm{K}}\) stands for Kelvin units). The energy of activation of the reaction is

320254 For a reaction, the value of rate constant at 300 \(\mathrm{K}\) is \(6.0 \times 10^{5} \mathrm{~s}^{-1}\). The value of Arrhenius factor \(\mathrm{A}\), at infinitely high temperature is:

320255 A plot of \({\mathrm{\ln k}}\) versus \({\mathrm{\dfrac{1}{T}}}\) for a reaction gives the slope \({\mathrm{-2.0 \times 10^{3} \mathrm{~K}}}\). The energy of activation for the reaction is ____ \({\mathrm{\mathrm{kJ} \mathrm{mol}^{-1}}}\).

320256 If for two reactions \(\mathrm{E}_{\mathrm{a}_{1}}>\mathrm{E}_{\mathrm{a}_{2}}\) and \(\mathrm{TC}_{1}\) and \(\mathrm{TC}_{2}\) are temperature coefficient respectively, then which alternative is correct?

320252 The activation energy for a simple chemical
reaction \(\mathrm{A} \rightarrow \mathrm{B}\) is \(\mathrm{E}_{\mathrm{a}}\) in forward direction. The
activation energy for reverse reaction

320253 The decomposition of\({{\text{N}}_{\text{2}}}{\text{O}}\,\,{\text{into }}{{\text{N}}_{\text{2}}}\) and in presence gaseous argon follow second order kinetics with \({\rm{k = }}\left( {{\rm{5}}{\rm{.0 \times 1}}{{\rm{0}}^{{\rm{11}}}}\,{\rm{L}}\,{\rm{mo}}{{\rm{l}}^{{\rm{ - 1}}}}\;{{\rm{s}}^{{\rm{ - 1}}}}} \right){{\rm{e}}^{{\rm{ - }}\frac{{{\rm{41570}}}}{{\rm{T}}}}}{\rm{K}}\) stands for Kelvin units). The energy of activation of the reaction is

320254 For a reaction, the value of rate constant at 300 \(\mathrm{K}\) is \(6.0 \times 10^{5} \mathrm{~s}^{-1}\). The value of Arrhenius factor \(\mathrm{A}\), at infinitely high temperature is:

320255 A plot of \({\mathrm{\ln k}}\) versus \({\mathrm{\dfrac{1}{T}}}\) for a reaction gives the slope \({\mathrm{-2.0 \times 10^{3} \mathrm{~K}}}\). The energy of activation for the reaction is ____ \({\mathrm{\mathrm{kJ} \mathrm{mol}^{-1}}}\).

320256 If for two reactions \(\mathrm{E}_{\mathrm{a}_{1}}>\mathrm{E}_{\mathrm{a}_{2}}\) and \(\mathrm{TC}_{1}\) and \(\mathrm{TC}_{2}\) are temperature coefficient respectively, then which alternative is correct?

320252 The activation energy for a simple chemical
reaction \(\mathrm{A} \rightarrow \mathrm{B}\) is \(\mathrm{E}_{\mathrm{a}}\) in forward direction. The
activation energy for reverse reaction

320253 The decomposition of\({{\text{N}}_{\text{2}}}{\text{O}}\,\,{\text{into }}{{\text{N}}_{\text{2}}}\) and in presence gaseous argon follow second order kinetics with \({\rm{k = }}\left( {{\rm{5}}{\rm{.0 \times 1}}{{\rm{0}}^{{\rm{11}}}}\,{\rm{L}}\,{\rm{mo}}{{\rm{l}}^{{\rm{ - 1}}}}\;{{\rm{s}}^{{\rm{ - 1}}}}} \right){{\rm{e}}^{{\rm{ - }}\frac{{{\rm{41570}}}}{{\rm{T}}}}}{\rm{K}}\) stands for Kelvin units). The energy of activation of the reaction is

320254 For a reaction, the value of rate constant at 300 \(\mathrm{K}\) is \(6.0 \times 10^{5} \mathrm{~s}^{-1}\). The value of Arrhenius factor \(\mathrm{A}\), at infinitely high temperature is:

320255 A plot of \({\mathrm{\ln k}}\) versus \({\mathrm{\dfrac{1}{T}}}\) for a reaction gives the slope \({\mathrm{-2.0 \times 10^{3} \mathrm{~K}}}\). The energy of activation for the reaction is ____ \({\mathrm{\mathrm{kJ} \mathrm{mol}^{-1}}}\).

320256 If for two reactions \(\mathrm{E}_{\mathrm{a}_{1}}>\mathrm{E}_{\mathrm{a}_{2}}\) and \(\mathrm{TC}_{1}\) and \(\mathrm{TC}_{2}\) are temperature coefficient respectively, then which alternative is correct?

320252 The activation energy for a simple chemical
reaction \(\mathrm{A} \rightarrow \mathrm{B}\) is \(\mathrm{E}_{\mathrm{a}}\) in forward direction. The
activation energy for reverse reaction

320253 The decomposition of\({{\text{N}}_{\text{2}}}{\text{O}}\,\,{\text{into }}{{\text{N}}_{\text{2}}}\) and in presence gaseous argon follow second order kinetics with \({\rm{k = }}\left( {{\rm{5}}{\rm{.0 \times 1}}{{\rm{0}}^{{\rm{11}}}}\,{\rm{L}}\,{\rm{mo}}{{\rm{l}}^{{\rm{ - 1}}}}\;{{\rm{s}}^{{\rm{ - 1}}}}} \right){{\rm{e}}^{{\rm{ - }}\frac{{{\rm{41570}}}}{{\rm{T}}}}}{\rm{K}}\) stands for Kelvin units). The energy of activation of the reaction is

320254 For a reaction, the value of rate constant at 300 \(\mathrm{K}\) is \(6.0 \times 10^{5} \mathrm{~s}^{-1}\). The value of Arrhenius factor \(\mathrm{A}\), at infinitely high temperature is:

320255 A plot of \({\mathrm{\ln k}}\) versus \({\mathrm{\dfrac{1}{T}}}\) for a reaction gives the slope \({\mathrm{-2.0 \times 10^{3} \mathrm{~K}}}\). The energy of activation for the reaction is ____ \({\mathrm{\mathrm{kJ} \mathrm{mol}^{-1}}}\).

320256 If for two reactions \(\mathrm{E}_{\mathrm{a}_{1}}>\mathrm{E}_{\mathrm{a}_{2}}\) and \(\mathrm{TC}_{1}\) and \(\mathrm{TC}_{2}\) are temperature coefficient respectively, then which alternative is correct?

320252 The activation energy for a simple chemical
reaction \(\mathrm{A} \rightarrow \mathrm{B}\) is \(\mathrm{E}_{\mathrm{a}}\) in forward direction. The
activation energy for reverse reaction

320253 The decomposition of\({{\text{N}}_{\text{2}}}{\text{O}}\,\,{\text{into }}{{\text{N}}_{\text{2}}}\) and in presence gaseous argon follow second order kinetics with \({\rm{k = }}\left( {{\rm{5}}{\rm{.0 \times 1}}{{\rm{0}}^{{\rm{11}}}}\,{\rm{L}}\,{\rm{mo}}{{\rm{l}}^{{\rm{ - 1}}}}\;{{\rm{s}}^{{\rm{ - 1}}}}} \right){{\rm{e}}^{{\rm{ - }}\frac{{{\rm{41570}}}}{{\rm{T}}}}}{\rm{K}}\) stands for Kelvin units). The energy of activation of the reaction is

320254 For a reaction, the value of rate constant at 300 \(\mathrm{K}\) is \(6.0 \times 10^{5} \mathrm{~s}^{-1}\). The value of Arrhenius factor \(\mathrm{A}\), at infinitely high temperature is:

320255 A plot of \({\mathrm{\ln k}}\) versus \({\mathrm{\dfrac{1}{T}}}\) for a reaction gives the slope \({\mathrm{-2.0 \times 10^{3} \mathrm{~K}}}\). The energy of activation for the reaction is ____ \({\mathrm{\mathrm{kJ} \mathrm{mol}^{-1}}}\).

320256 If for two reactions \(\mathrm{E}_{\mathrm{a}_{1}}>\mathrm{E}_{\mathrm{a}_{2}}\) and \(\mathrm{TC}_{1}\) and \(\mathrm{TC}_{2}\) are temperature coefficient respectively, then which alternative is correct?