Reaction kinetics

You will be able to

• Use experimental data to calculate the rate of a reaction, as an initial rate or from the gradient of a tangent.
• Convert a gradient in cm³ s⁻¹ to a rate in mol dm⁻³ s⁻¹ using the molar volume of a gas.
• Explain why only initial rates measured with one factor changed give a fair comparison.

You will be able to

• Define activation energy, Ea, as the minimum energy required for a collision to be effective.
• Sketch and use the Boltzmann distribution to explain the effect of a temperature change on the rate of a reaction.
• Explain, in terms of the Boltzmann distribution, how a catalyst with a lower activation energy increases the rate.