Activation Energy and Arrhenius Equation
Chemistry ⇒ Chemical Kinetics and Equilibrium
Activation Energy and Arrhenius Equation starts at 11 and continues till grade 12.
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A reaction has a frequency factor of 2.0 \times 10^{12}\ \mathrm{s}^{-1} and an activation energy of 80\ \mathrm{kJ}/\mathrm{mol}. Calculate the rate constant at 298\ \mathrm{K}. (R = 8.314\ \mathrm{J}\ \mathrm{mol}^{-1}\ \mathrm{K}^{-1})
A reaction has a rate constant of 1.5 \times 10^{-2}\ \mathrm{s}^{-1} at 350\ \mathrm{K} and 3.0 \times 10^{-2}\ \mathrm{s}^{-1} at 360\ \mathrm{K}. Calculate the activation energy.
A reaction has a rate constant of 2.0 \times 10^{-3}\ \mathrm{s}^{-1} at 300\ \mathrm{K} and 4.0 \times 10^{-3}\ \mathrm{s}^{-1} at 310\ \mathrm{K}. Calculate the activation energy.
Calculate the activation energy if the rate constant doubles when the temperature increases from 300\ \mathrm{K} to 310\ \mathrm{K}. (R = 8.314\ \mathrm{J}\ \mathrm{mol}^{-1}\ \mathrm{K}^{-1})
Describe how you would determine the activation energy of a reaction experimentally using the Arrhenius equation.
Describe the effect of a catalyst on the activation energy and the rate constant of a reaction.
Describe the physical meaning of the exponential factor in the Arrhenius equation.
Explain how the rate constant changes with temperature according to the Arrhenius equation.
Explain the significance of the pre-exponential factor (A) in the Arrhenius equation.
Explain why a catalyst does not affect the equilibrium position of a reaction, even though it lowers the activation energy.
Explain why reactions with low activation energies are generally faster than those with high activation energies.
If a reaction has an activation energy of 50\ \mathrm{kJ}/\mathrm{mol}, what is the effect of increasing the temperature from 300\ \mathrm{K} to 310\ \mathrm{K} on the rate constant?
If the activation energy of a reaction is high, what does this imply about the rate of the reaction at a given temperature?
If the activation energy of a reaction is zero, how does the rate constant change with temperature?
If the frequency factor (A) is 1.0 \times 10^{13}\ \mathrm{s}^{-1}, the activation energy is 60\ \mathrm{kJ}/\mathrm{mol}, and the temperature is 300\ \mathrm{K}, calculate the rate constant k. (R = 8.314\ \mathrm{J}\ \mathrm{mol}^{-1}\ \mathrm{K}^{-1})
The activation energy for a reaction is 100\ \mathrm{kJ}/\mathrm{mol}. If the rate constant at 400\ \mathrm{K} is 2.0 \times 10^{-4}\ \mathrm{s}^{-1}, what is the rate constant at 410\ \mathrm{K}? (R = 8.314\ \mathrm{J}\ \mathrm{mol}^{-1}\ \mathrm{K}^{-1})
The activation energy for a reaction is 75\ \mathrm{kJ}/\mathrm{mol}. What is the effect on the rate constant if the temperature is increased from 298\ \mathrm{K} to 308\ \mathrm{K}?
The activation energy of a reaction is 40\ \mathrm{kJ}/\mathrm{mol}. If the temperature is doubled, what happens to the rate constant?
What is the Arrhenius equation?
A certain reaction has a rate constant of 5.0 \times 10^{-3}\ \mathrm{s}^{-1} at 290\ \mathrm{K} and 2.0 \times 10^{-2}\ \mathrm{s}^{-1} at 310\ \mathrm{K}. Calculate the activation energy for the reaction. (R = 8.314\ \mathrm{J}\ \mathrm{mol}^{-1}\ \mathrm{K}^{-1})
