Dependence of Rate on Temperature
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CHXII04:CHEMICAL KINETICS

320218 The activation energy for a reaction at the temperature TK was found to be \({\rm{2}}{\rm{.303}}\,\,{\rm{RTJ}}\,\,{\rm{mo}}{{\rm{l}}^{{\rm{ - 1}}}}\). The ratio of the rate constant to Arrhenius factor is

1 \(10^{-1}\)
2 \(10^{-2}\)
3 \(2 \times 10^{-3}\)
4 \(2 \times 10^{-2}\)
CHXII04:CHEMICAL KINETICS

320219 Two reactions \({{\rm{R}}_{\rm{1}}}\,\,{\rm{and}}\,\,{{\rm{R}}_{\rm{2}}}\) have identical preexponential factors. Activation energy of \({{\rm{R}}_{\rm{1}}}\) exceeds that of \({{\text{R}}_{\text{2}}}{\mkern 1mu} {\mkern 1mu} {\text{by10}}\;{\text{kJ}}\;{\text{mo}}{{\text{l}}^{{\text{ - 1}}}}\).
If \({{\text{k}}_{\text{1}}}\) and \({{\text{k}}_{\text{2}}}\) and \({{\text{R}}_{\text{2}}}\) are rate constants for reaction \({{\rm{R}}_{\rm{1}}}\,\,{\rm{and}}\,\,{{\rm{R}}_{\rm{2}}}\) respectively at 300 k, then \({\rm{in}}\left( {{{\rm{k}}_{\rm{2}}}{\rm{/}}{{\rm{k}}_{\rm{1}}}} \right)\) is equal to :- \(\left( {{\rm{R = 8}}{\rm{.314\;J\;mo}}{{\rm{l}}^{{\rm{ - 1}}}}{\rm{\;}}{{\rm{K}}^{{\rm{ - 1}}}}} \right)\)

1 6
2 12
3 8
4 4
CHXII04:CHEMICAL KINETICS

320220 The rate constant of a reaction at temperature \(200 \mathrm{~K}\) is 10 times less than the rate constant at \(400 \mathrm{~K}\). What is the activation energy of the reaction?

1 \(1842.4\,{\text{R}}\)
2 \(460.6\,{\text{R}}\)
3 \(230.3\,{\text{R}}\)
4 \(921.2\,{\text{R}}\)
CHXII04:CHEMICAL KINETICS

320221 Which of the following is incorrect from the theory of Arrhenius's equation?

1 The number of effective collisions is proportional to the number of molecules above a certain threshold energy.
2 As the temperature increases, the number of molecules with energies exceeding the threshold energy increases.
3 The rate constant is a function of temperature
4 Activation energy and pre-exponential factors are temperature-dependent.
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CHXII04:CHEMICAL KINETICS

320218 The activation energy for a reaction at the temperature TK was found to be \({\rm{2}}{\rm{.303}}\,\,{\rm{RTJ}}\,\,{\rm{mo}}{{\rm{l}}^{{\rm{ - 1}}}}\). The ratio of the rate constant to Arrhenius factor is

1 \(10^{-1}\)
2 \(10^{-2}\)
3 \(2 \times 10^{-3}\)
4 \(2 \times 10^{-2}\)
CHXII04:CHEMICAL KINETICS

320219 Two reactions \({{\rm{R}}_{\rm{1}}}\,\,{\rm{and}}\,\,{{\rm{R}}_{\rm{2}}}\) have identical preexponential factors. Activation energy of \({{\rm{R}}_{\rm{1}}}\) exceeds that of \({{\text{R}}_{\text{2}}}{\mkern 1mu} {\mkern 1mu} {\text{by10}}\;{\text{kJ}}\;{\text{mo}}{{\text{l}}^{{\text{ - 1}}}}\).
If \({{\text{k}}_{\text{1}}}\) and \({{\text{k}}_{\text{2}}}\) and \({{\text{R}}_{\text{2}}}\) are rate constants for reaction \({{\rm{R}}_{\rm{1}}}\,\,{\rm{and}}\,\,{{\rm{R}}_{\rm{2}}}\) respectively at 300 k, then \({\rm{in}}\left( {{{\rm{k}}_{\rm{2}}}{\rm{/}}{{\rm{k}}_{\rm{1}}}} \right)\) is equal to :- \(\left( {{\rm{R = 8}}{\rm{.314\;J\;mo}}{{\rm{l}}^{{\rm{ - 1}}}}{\rm{\;}}{{\rm{K}}^{{\rm{ - 1}}}}} \right)\)

1 6
2 12
3 8
4 4
CHXII04:CHEMICAL KINETICS

320220 The rate constant of a reaction at temperature \(200 \mathrm{~K}\) is 10 times less than the rate constant at \(400 \mathrm{~K}\). What is the activation energy of the reaction?

1 \(1842.4\,{\text{R}}\)
2 \(460.6\,{\text{R}}\)
3 \(230.3\,{\text{R}}\)
4 \(921.2\,{\text{R}}\)
CHXII04:CHEMICAL KINETICS

320221 Which of the following is incorrect from the theory of Arrhenius's equation?

1 The number of effective collisions is proportional to the number of molecules above a certain threshold energy.
2 As the temperature increases, the number of molecules with energies exceeding the threshold energy increases.
3 The rate constant is a function of temperature
4 Activation energy and pre-exponential factors are temperature-dependent.
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CHXII04:CHEMICAL KINETICS

320218 The activation energy for a reaction at the temperature TK was found to be \({\rm{2}}{\rm{.303}}\,\,{\rm{RTJ}}\,\,{\rm{mo}}{{\rm{l}}^{{\rm{ - 1}}}}\). The ratio of the rate constant to Arrhenius factor is

1 \(10^{-1}\)
2 \(10^{-2}\)
3 \(2 \times 10^{-3}\)
4 \(2 \times 10^{-2}\)
CHXII04:CHEMICAL KINETICS

320219 Two reactions \({{\rm{R}}_{\rm{1}}}\,\,{\rm{and}}\,\,{{\rm{R}}_{\rm{2}}}\) have identical preexponential factors. Activation energy of \({{\rm{R}}_{\rm{1}}}\) exceeds that of \({{\text{R}}_{\text{2}}}{\mkern 1mu} {\mkern 1mu} {\text{by10}}\;{\text{kJ}}\;{\text{mo}}{{\text{l}}^{{\text{ - 1}}}}\).
If \({{\text{k}}_{\text{1}}}\) and \({{\text{k}}_{\text{2}}}\) and \({{\text{R}}_{\text{2}}}\) are rate constants for reaction \({{\rm{R}}_{\rm{1}}}\,\,{\rm{and}}\,\,{{\rm{R}}_{\rm{2}}}\) respectively at 300 k, then \({\rm{in}}\left( {{{\rm{k}}_{\rm{2}}}{\rm{/}}{{\rm{k}}_{\rm{1}}}} \right)\) is equal to :- \(\left( {{\rm{R = 8}}{\rm{.314\;J\;mo}}{{\rm{l}}^{{\rm{ - 1}}}}{\rm{\;}}{{\rm{K}}^{{\rm{ - 1}}}}} \right)\)

1 6
2 12
3 8
4 4
CHXII04:CHEMICAL KINETICS

320220 The rate constant of a reaction at temperature \(200 \mathrm{~K}\) is 10 times less than the rate constant at \(400 \mathrm{~K}\). What is the activation energy of the reaction?

1 \(1842.4\,{\text{R}}\)
2 \(460.6\,{\text{R}}\)
3 \(230.3\,{\text{R}}\)
4 \(921.2\,{\text{R}}\)
CHXII04:CHEMICAL KINETICS

320221 Which of the following is incorrect from the theory of Arrhenius's equation?

1 The number of effective collisions is proportional to the number of molecules above a certain threshold energy.
2 As the temperature increases, the number of molecules with energies exceeding the threshold energy increases.
3 The rate constant is a function of temperature
4 Activation energy and pre-exponential factors are temperature-dependent.
For More Updates join with Us
CHXII04:CHEMICAL KINETICS

320218 The activation energy for a reaction at the temperature TK was found to be \({\rm{2}}{\rm{.303}}\,\,{\rm{RTJ}}\,\,{\rm{mo}}{{\rm{l}}^{{\rm{ - 1}}}}\). The ratio of the rate constant to Arrhenius factor is

1 \(10^{-1}\)
2 \(10^{-2}\)
3 \(2 \times 10^{-3}\)
4 \(2 \times 10^{-2}\)
CHXII04:CHEMICAL KINETICS

320219 Two reactions \({{\rm{R}}_{\rm{1}}}\,\,{\rm{and}}\,\,{{\rm{R}}_{\rm{2}}}\) have identical preexponential factors. Activation energy of \({{\rm{R}}_{\rm{1}}}\) exceeds that of \({{\text{R}}_{\text{2}}}{\mkern 1mu} {\mkern 1mu} {\text{by10}}\;{\text{kJ}}\;{\text{mo}}{{\text{l}}^{{\text{ - 1}}}}\).
If \({{\text{k}}_{\text{1}}}\) and \({{\text{k}}_{\text{2}}}\) and \({{\text{R}}_{\text{2}}}\) are rate constants for reaction \({{\rm{R}}_{\rm{1}}}\,\,{\rm{and}}\,\,{{\rm{R}}_{\rm{2}}}\) respectively at 300 k, then \({\rm{in}}\left( {{{\rm{k}}_{\rm{2}}}{\rm{/}}{{\rm{k}}_{\rm{1}}}} \right)\) is equal to :- \(\left( {{\rm{R = 8}}{\rm{.314\;J\;mo}}{{\rm{l}}^{{\rm{ - 1}}}}{\rm{\;}}{{\rm{K}}^{{\rm{ - 1}}}}} \right)\)

1 6
2 12
3 8
4 4
CHXII04:CHEMICAL KINETICS

320220 The rate constant of a reaction at temperature \(200 \mathrm{~K}\) is 10 times less than the rate constant at \(400 \mathrm{~K}\). What is the activation energy of the reaction?

1 \(1842.4\,{\text{R}}\)
2 \(460.6\,{\text{R}}\)
3 \(230.3\,{\text{R}}\)
4 \(921.2\,{\text{R}}\)
CHXII04:CHEMICAL KINETICS

320221 Which of the following is incorrect from the theory of Arrhenius's equation?

1 The number of effective collisions is proportional to the number of molecules above a certain threshold energy.
2 As the temperature increases, the number of molecules with energies exceeding the threshold energy increases.
3 The rate constant is a function of temperature
4 Activation energy and pre-exponential factors are temperature-dependent.
NEET DIGITAL LIBRARY