Dependence of Rate on Temperature
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CHXII04:CHEMICAL KINETICS

320269 Which of the following statements is in accordance with the Arrhenius equation?

1 Rate of a reaction decrease with increase in temperature
2 Rate of reaction does not change with increase in activation energy
3 Rate constant decreases exponentially with increase in temperature
4 Rate of a reaction increases with decrease in activation energy
CHXII04:CHEMICAL KINETICS

320270 The first order rate constant for the decomposition of ethyl iodide is given by the reaction
\({{\text{C}}_{\text{2}}}{{\text{H}}_{\text{5}}}{\text{I(g)}} \to {{\text{C}}_{\text{2}}}{{\text{H}}_{\text{4}}}{\text{(g)}} + {\text{HI(g)}}\)
at \(600 \mathrm{~K}\) is \(1.60 \times 10^{-5} \mathrm{~s}^{-1}\). Its energy of activation is \(209 \mathrm{~kJ} \mathrm{~mol}^{-1}\). What is the rate constant of the reaction at \(700 \mathrm{~K}\) ?

1 \(6.36 \times 10^{3} \mathrm{~s}^{-1}\)
2 \(6.36 \times 10^{-3} \mathrm{~s}^{-1}\)
3 \(6.36 \times 10^{3} \mathrm{~s}\)
4 \(6.36 \times 10^{-3} \mathrm{~s}\)
CHXII04:CHEMICAL KINETICS

320271 What is the activation energy for a reaction if its rate doubles when the temperature is raised from \(20^{\circ} \mathrm{C}\) to \(35^{\circ} \mathrm{C} ?\left(R=8.314 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}\right)\)

1 \({\rm{15}}\,{\rm{.1}}\,{\rm{kJ}}\,{\rm{mo}}{{\rm{l}}^{{\rm{ - 1}}}}\)
2 \(342 \mathrm{~kJ} \mathrm{~mol}^{-1}\)
3 \(269 \mathrm{~kJ} \mathrm{~mol}^{-1}\)
4 \(34.7 \mathrm{~kJ} \mathrm{~mol}^{-1}\)
KCET - 2012
CHXII04:CHEMICAL KINETICS

320272 For the equilibrium,
\({\text{A}}{\mkern 1mu} {\text{(g)}} \rightleftharpoons {\text{B}}{\mkern 1mu} {\text{(g),}}\,\) \({\rm{\Delta H = - 40}}\;{\rm{kJ/mol}}\). If the ratio of the activation energies of the forward \(\left( {{{\text{E}}_{\text{f}}}} \right)\) and reverse \(\left( {{{\text{E}}_{\text{b}}}} \right)\) reactions is \(\frac{{\text{2}}}{{\text{3}}}\) then

1 \({{\text{E}}_{\text{f}}}{\text{ = 30}}\;{\text{kJ/mol,}}{{\text{E}}_{\text{b}}}{\text{ = 70}}\;{\text{kJ/mol}}\)
2 \({{\text{E}}_{\text{f}}}{\text{ = 70}}\;{\text{kJ/mol,}}{{\text{E}}_{\text{b}}}{\text{ = 30}}\;{\text{kJ/mol}}\)
3 \({{\text{E}}_{\text{f}}}{\text{ = 80}}\;{\text{kJ/mol,}}{{\text{E}}_{\text{b}}}{\text{ = 120}}\;{\text{kJ/mol}}\)
4 \({{\text{E}}_{\text{f}}}{\text{ = 60}}\;{\text{kJ/mol,}}{{\text{E}}_{\text{b}}}{\text{ = 100}}\;{\text{kJ/mol}}\)
CHXII04:CHEMICAL KINETICS

320273 A molecule of gas is struck by another molecule of the same gas, the first molecule shows:

1 An exchange of potential energy
2 An exchange of kinetic energy
3 An exchange of chemical energy
4 No exchange of energy
NEET DIGITAL LIBRARY
CHXII04:CHEMICAL KINETICS

320269 Which of the following statements is in accordance with the Arrhenius equation?

1 Rate of a reaction decrease with increase in temperature
2 Rate of reaction does not change with increase in activation energy
3 Rate constant decreases exponentially with increase in temperature
4 Rate of a reaction increases with decrease in activation energy
CHXII04:CHEMICAL KINETICS

320270 The first order rate constant for the decomposition of ethyl iodide is given by the reaction
\({{\text{C}}_{\text{2}}}{{\text{H}}_{\text{5}}}{\text{I(g)}} \to {{\text{C}}_{\text{2}}}{{\text{H}}_{\text{4}}}{\text{(g)}} + {\text{HI(g)}}\)
at \(600 \mathrm{~K}\) is \(1.60 \times 10^{-5} \mathrm{~s}^{-1}\). Its energy of activation is \(209 \mathrm{~kJ} \mathrm{~mol}^{-1}\). What is the rate constant of the reaction at \(700 \mathrm{~K}\) ?

1 \(6.36 \times 10^{3} \mathrm{~s}^{-1}\)
2 \(6.36 \times 10^{-3} \mathrm{~s}^{-1}\)
3 \(6.36 \times 10^{3} \mathrm{~s}\)
4 \(6.36 \times 10^{-3} \mathrm{~s}\)
CHXII04:CHEMICAL KINETICS

320271 What is the activation energy for a reaction if its rate doubles when the temperature is raised from \(20^{\circ} \mathrm{C}\) to \(35^{\circ} \mathrm{C} ?\left(R=8.314 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}\right)\)

1 \({\rm{15}}\,{\rm{.1}}\,{\rm{kJ}}\,{\rm{mo}}{{\rm{l}}^{{\rm{ - 1}}}}\)
2 \(342 \mathrm{~kJ} \mathrm{~mol}^{-1}\)
3 \(269 \mathrm{~kJ} \mathrm{~mol}^{-1}\)
4 \(34.7 \mathrm{~kJ} \mathrm{~mol}^{-1}\)
KCET - 2012
CHXII04:CHEMICAL KINETICS

320272 For the equilibrium,
\({\text{A}}{\mkern 1mu} {\text{(g)}} \rightleftharpoons {\text{B}}{\mkern 1mu} {\text{(g),}}\,\) \({\rm{\Delta H = - 40}}\;{\rm{kJ/mol}}\). If the ratio of the activation energies of the forward \(\left( {{{\text{E}}_{\text{f}}}} \right)\) and reverse \(\left( {{{\text{E}}_{\text{b}}}} \right)\) reactions is \(\frac{{\text{2}}}{{\text{3}}}\) then

1 \({{\text{E}}_{\text{f}}}{\text{ = 30}}\;{\text{kJ/mol,}}{{\text{E}}_{\text{b}}}{\text{ = 70}}\;{\text{kJ/mol}}\)
2 \({{\text{E}}_{\text{f}}}{\text{ = 70}}\;{\text{kJ/mol,}}{{\text{E}}_{\text{b}}}{\text{ = 30}}\;{\text{kJ/mol}}\)
3 \({{\text{E}}_{\text{f}}}{\text{ = 80}}\;{\text{kJ/mol,}}{{\text{E}}_{\text{b}}}{\text{ = 120}}\;{\text{kJ/mol}}\)
4 \({{\text{E}}_{\text{f}}}{\text{ = 60}}\;{\text{kJ/mol,}}{{\text{E}}_{\text{b}}}{\text{ = 100}}\;{\text{kJ/mol}}\)
CHXII04:CHEMICAL KINETICS

320273 A molecule of gas is struck by another molecule of the same gas, the first molecule shows:

1 An exchange of potential energy
2 An exchange of kinetic energy
3 An exchange of chemical energy
4 No exchange of energy
Join With Us for More Updates
CHXII04:CHEMICAL KINETICS

320269 Which of the following statements is in accordance with the Arrhenius equation?

1 Rate of a reaction decrease with increase in temperature
2 Rate of reaction does not change with increase in activation energy
3 Rate constant decreases exponentially with increase in temperature
4 Rate of a reaction increases with decrease in activation energy
CHXII04:CHEMICAL KINETICS

320270 The first order rate constant for the decomposition of ethyl iodide is given by the reaction
\({{\text{C}}_{\text{2}}}{{\text{H}}_{\text{5}}}{\text{I(g)}} \to {{\text{C}}_{\text{2}}}{{\text{H}}_{\text{4}}}{\text{(g)}} + {\text{HI(g)}}\)
at \(600 \mathrm{~K}\) is \(1.60 \times 10^{-5} \mathrm{~s}^{-1}\). Its energy of activation is \(209 \mathrm{~kJ} \mathrm{~mol}^{-1}\). What is the rate constant of the reaction at \(700 \mathrm{~K}\) ?

1 \(6.36 \times 10^{3} \mathrm{~s}^{-1}\)
2 \(6.36 \times 10^{-3} \mathrm{~s}^{-1}\)
3 \(6.36 \times 10^{3} \mathrm{~s}\)
4 \(6.36 \times 10^{-3} \mathrm{~s}\)
CHXII04:CHEMICAL KINETICS

320271 What is the activation energy for a reaction if its rate doubles when the temperature is raised from \(20^{\circ} \mathrm{C}\) to \(35^{\circ} \mathrm{C} ?\left(R=8.314 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}\right)\)

1 \({\rm{15}}\,{\rm{.1}}\,{\rm{kJ}}\,{\rm{mo}}{{\rm{l}}^{{\rm{ - 1}}}}\)
2 \(342 \mathrm{~kJ} \mathrm{~mol}^{-1}\)
3 \(269 \mathrm{~kJ} \mathrm{~mol}^{-1}\)
4 \(34.7 \mathrm{~kJ} \mathrm{~mol}^{-1}\)
KCET - 2012
CHXII04:CHEMICAL KINETICS

320272 For the equilibrium,
\({\text{A}}{\mkern 1mu} {\text{(g)}} \rightleftharpoons {\text{B}}{\mkern 1mu} {\text{(g),}}\,\) \({\rm{\Delta H = - 40}}\;{\rm{kJ/mol}}\). If the ratio of the activation energies of the forward \(\left( {{{\text{E}}_{\text{f}}}} \right)\) and reverse \(\left( {{{\text{E}}_{\text{b}}}} \right)\) reactions is \(\frac{{\text{2}}}{{\text{3}}}\) then

1 \({{\text{E}}_{\text{f}}}{\text{ = 30}}\;{\text{kJ/mol,}}{{\text{E}}_{\text{b}}}{\text{ = 70}}\;{\text{kJ/mol}}\)
2 \({{\text{E}}_{\text{f}}}{\text{ = 70}}\;{\text{kJ/mol,}}{{\text{E}}_{\text{b}}}{\text{ = 30}}\;{\text{kJ/mol}}\)
3 \({{\text{E}}_{\text{f}}}{\text{ = 80}}\;{\text{kJ/mol,}}{{\text{E}}_{\text{b}}}{\text{ = 120}}\;{\text{kJ/mol}}\)
4 \({{\text{E}}_{\text{f}}}{\text{ = 60}}\;{\text{kJ/mol,}}{{\text{E}}_{\text{b}}}{\text{ = 100}}\;{\text{kJ/mol}}\)
CHXII04:CHEMICAL KINETICS

320273 A molecule of gas is struck by another molecule of the same gas, the first molecule shows:

1 An exchange of potential energy
2 An exchange of kinetic energy
3 An exchange of chemical energy
4 No exchange of energy
For More Updates join with Us
CHXII04:CHEMICAL KINETICS

320269 Which of the following statements is in accordance with the Arrhenius equation?

1 Rate of a reaction decrease with increase in temperature
2 Rate of reaction does not change with increase in activation energy
3 Rate constant decreases exponentially with increase in temperature
4 Rate of a reaction increases with decrease in activation energy
CHXII04:CHEMICAL KINETICS

320270 The first order rate constant for the decomposition of ethyl iodide is given by the reaction
\({{\text{C}}_{\text{2}}}{{\text{H}}_{\text{5}}}{\text{I(g)}} \to {{\text{C}}_{\text{2}}}{{\text{H}}_{\text{4}}}{\text{(g)}} + {\text{HI(g)}}\)
at \(600 \mathrm{~K}\) is \(1.60 \times 10^{-5} \mathrm{~s}^{-1}\). Its energy of activation is \(209 \mathrm{~kJ} \mathrm{~mol}^{-1}\). What is the rate constant of the reaction at \(700 \mathrm{~K}\) ?

1 \(6.36 \times 10^{3} \mathrm{~s}^{-1}\)
2 \(6.36 \times 10^{-3} \mathrm{~s}^{-1}\)
3 \(6.36 \times 10^{3} \mathrm{~s}\)
4 \(6.36 \times 10^{-3} \mathrm{~s}\)
CHXII04:CHEMICAL KINETICS

320271 What is the activation energy for a reaction if its rate doubles when the temperature is raised from \(20^{\circ} \mathrm{C}\) to \(35^{\circ} \mathrm{C} ?\left(R=8.314 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}\right)\)

1 \({\rm{15}}\,{\rm{.1}}\,{\rm{kJ}}\,{\rm{mo}}{{\rm{l}}^{{\rm{ - 1}}}}\)
2 \(342 \mathrm{~kJ} \mathrm{~mol}^{-1}\)
3 \(269 \mathrm{~kJ} \mathrm{~mol}^{-1}\)
4 \(34.7 \mathrm{~kJ} \mathrm{~mol}^{-1}\)
KCET - 2012
CHXII04:CHEMICAL KINETICS

320272 For the equilibrium,
\({\text{A}}{\mkern 1mu} {\text{(g)}} \rightleftharpoons {\text{B}}{\mkern 1mu} {\text{(g),}}\,\) \({\rm{\Delta H = - 40}}\;{\rm{kJ/mol}}\). If the ratio of the activation energies of the forward \(\left( {{{\text{E}}_{\text{f}}}} \right)\) and reverse \(\left( {{{\text{E}}_{\text{b}}}} \right)\) reactions is \(\frac{{\text{2}}}{{\text{3}}}\) then

1 \({{\text{E}}_{\text{f}}}{\text{ = 30}}\;{\text{kJ/mol,}}{{\text{E}}_{\text{b}}}{\text{ = 70}}\;{\text{kJ/mol}}\)
2 \({{\text{E}}_{\text{f}}}{\text{ = 70}}\;{\text{kJ/mol,}}{{\text{E}}_{\text{b}}}{\text{ = 30}}\;{\text{kJ/mol}}\)
3 \({{\text{E}}_{\text{f}}}{\text{ = 80}}\;{\text{kJ/mol,}}{{\text{E}}_{\text{b}}}{\text{ = 120}}\;{\text{kJ/mol}}\)
4 \({{\text{E}}_{\text{f}}}{\text{ = 60}}\;{\text{kJ/mol,}}{{\text{E}}_{\text{b}}}{\text{ = 100}}\;{\text{kJ/mol}}\)
CHXII04:CHEMICAL KINETICS

320273 A molecule of gas is struck by another molecule of the same gas, the first molecule shows:

1 An exchange of potential energy
2 An exchange of kinetic energy
3 An exchange of chemical energy
4 No exchange of energy
NEET DIGITAL LIBRARY
CHXII04:CHEMICAL KINETICS

320269 Which of the following statements is in accordance with the Arrhenius equation?

1 Rate of a reaction decrease with increase in temperature
2 Rate of reaction does not change with increase in activation energy
3 Rate constant decreases exponentially with increase in temperature
4 Rate of a reaction increases with decrease in activation energy
CHXII04:CHEMICAL KINETICS

320270 The first order rate constant for the decomposition of ethyl iodide is given by the reaction
\({{\text{C}}_{\text{2}}}{{\text{H}}_{\text{5}}}{\text{I(g)}} \to {{\text{C}}_{\text{2}}}{{\text{H}}_{\text{4}}}{\text{(g)}} + {\text{HI(g)}}\)
at \(600 \mathrm{~K}\) is \(1.60 \times 10^{-5} \mathrm{~s}^{-1}\). Its energy of activation is \(209 \mathrm{~kJ} \mathrm{~mol}^{-1}\). What is the rate constant of the reaction at \(700 \mathrm{~K}\) ?

1 \(6.36 \times 10^{3} \mathrm{~s}^{-1}\)
2 \(6.36 \times 10^{-3} \mathrm{~s}^{-1}\)
3 \(6.36 \times 10^{3} \mathrm{~s}\)
4 \(6.36 \times 10^{-3} \mathrm{~s}\)
CHXII04:CHEMICAL KINETICS

320271 What is the activation energy for a reaction if its rate doubles when the temperature is raised from \(20^{\circ} \mathrm{C}\) to \(35^{\circ} \mathrm{C} ?\left(R=8.314 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}\right)\)

1 \({\rm{15}}\,{\rm{.1}}\,{\rm{kJ}}\,{\rm{mo}}{{\rm{l}}^{{\rm{ - 1}}}}\)
2 \(342 \mathrm{~kJ} \mathrm{~mol}^{-1}\)
3 \(269 \mathrm{~kJ} \mathrm{~mol}^{-1}\)
4 \(34.7 \mathrm{~kJ} \mathrm{~mol}^{-1}\)
KCET - 2012
CHXII04:CHEMICAL KINETICS

320272 For the equilibrium,
\({\text{A}}{\mkern 1mu} {\text{(g)}} \rightleftharpoons {\text{B}}{\mkern 1mu} {\text{(g),}}\,\) \({\rm{\Delta H = - 40}}\;{\rm{kJ/mol}}\). If the ratio of the activation energies of the forward \(\left( {{{\text{E}}_{\text{f}}}} \right)\) and reverse \(\left( {{{\text{E}}_{\text{b}}}} \right)\) reactions is \(\frac{{\text{2}}}{{\text{3}}}\) then

1 \({{\text{E}}_{\text{f}}}{\text{ = 30}}\;{\text{kJ/mol,}}{{\text{E}}_{\text{b}}}{\text{ = 70}}\;{\text{kJ/mol}}\)
2 \({{\text{E}}_{\text{f}}}{\text{ = 70}}\;{\text{kJ/mol,}}{{\text{E}}_{\text{b}}}{\text{ = 30}}\;{\text{kJ/mol}}\)
3 \({{\text{E}}_{\text{f}}}{\text{ = 80}}\;{\text{kJ/mol,}}{{\text{E}}_{\text{b}}}{\text{ = 120}}\;{\text{kJ/mol}}\)
4 \({{\text{E}}_{\text{f}}}{\text{ = 60}}\;{\text{kJ/mol,}}{{\text{E}}_{\text{b}}}{\text{ = 100}}\;{\text{kJ/mol}}\)
CHXII04:CHEMICAL KINETICS

320273 A molecule of gas is struck by another molecule of the same gas, the first molecule shows:

1 An exchange of potential energy
2 An exchange of kinetic energy
3 An exchange of chemical energy
4 No exchange of energy