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 plot of \ln k versus 1/T for a reaction gives a straight line with a slope of -6000\ \mathrm{K}. Calculate the activation energy (E_{a}). (R = 8.314\ \mathrm{J}\ \mathrm{mol}^{-1}\ \mathrm{K}^{-1})
A reaction has a pre-exponential factor (A) of 1.0 \times 10^{13}\ \mathrm{s}^{-1} and an activation energy of 60\ \mathrm{kJ}\ \mathrm{mol}^{-1}. Calculate the rate constant at 300\ \mathrm{K}. (R = 8.314\ \mathrm{J}\ \mathrm{mol}^{-1}\ \mathrm{K}^{-1})
A reaction has a rate constant of 1.2 \times 10^{-4}\ \mathrm{s}^{-1} at 350\ \mathrm{K} and 2.4 \times 10^{-4}\ \mathrm{s}^{-1} at 360\ \mathrm{K}. Calculate the activation energy (E_{a}). (R = 8.314\ \mathrm{J}\ \mathrm{mol}^{-1}\ \mathrm{K}^{-1})
A reaction has an activation energy of 50\ \mathrm{kJ}\ \mathrm{mol}^{-1}. If the temperature is increased from 300\ \mathrm{K} to 320\ \mathrm{K}, will the rate constant increase or decrease?
A reaction has an activation energy of 75\ \mathrm{kJ}\ \mathrm{mol}^{-1}. If the temperature increases, what happens to the rate constant?
Calculate the activation energy (E_{a}) 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.
Describe the difference between activation energy and enthalpy change of a reaction.
Describe the significance of the exponential term e^{-E_{a}/RT} in the Arrhenius equation.
Explain how a catalyst affects the activation energy and the rate of a chemical reaction.
Explain why increasing temperature increases the rate of a chemical reaction according to the Arrhenius equation.
Explain why some reactions with high activation energy can still occur rapidly at high temperatures.
State the Arrhenius equation and explain each term.
The Arrhenius equation is given by k = A e^{-E_{a}/RT}. What does 'A' represent in this equation?
The rate constant for a reaction at 298\ \mathrm{K} is 2.5 \times 10^{-3}\ \mathrm{s}^{-1}. At 308\ \mathrm{K}, it is 5.0 \times 10^{-3}\ \mathrm{s}^{-1}. Calculate the activation energy (E_{a}). (R = 8.314\ \mathrm{J}\ \mathrm{mol}^{-1}\ \mathrm{K}^{-1})
What is activation energy?
What is the effect of increasing temperature on the rate constant according to the Arrhenius equation?
