Seneca
Sign up

Orders, Rate Constants & Equations

Chemistry: Cambridge International A Level, topic 1.9.2

Rate Equations

You can calculate rates of reactions by finding their rate equations. These link the concentration of each reactant to the rate of the equation.

Physical basis

Physical basis

  • Reactions happen when molecules collide into one another.
  • In a reaction between molecule A and B, the rate will be proportional to the number of collisions between A and B.
  • If you double the concentration of B, you should have double the collisions between A and B.
  • So, you would expect the reaction rate to double.
  • In reality, this is an over-simplification because you have multiple steps in most reactions, which may or may not involve each molecule.
The rate equation

The rate equation

  • A rate equation is always written of the form:
  • Rate = k × [A]m[B]n
  • k is called the rate constant.
  • The numbers m and n tell you how the rate depends on the reactants.
  • They are called the order of the reaction with respect to each reactant.
The order of reaction

The order of reaction

  • Just as we define an order for the reactants, we define an overall order for the reaction.
  • The overall order is given by m + n.
  • You very rarely get any value above 2 for an order with respect to a reactant, or less than zero.
The rate constant

The rate constant

  • The rate constant k has a few key features:
  • It’s temperature dependent.
  • It has different units for different reactions.
  • The units of the reaction rate have to be concentration over time.
  • But the units of the product of the reactants are never that, so you need to assign units to k to sort it out.
  • The larger the rate constant, the faster the reaction.

Calculations of Rate Equations

You need to be able to do a whole bunch of calculations with rate equations.

Calculating the rate of reactions

Calculating the rate of reactions

  • The rate of a reaction can be calculated if you know its rate constant, the reactant concentrations, and the order of the reaction with respect to each reactant.
  • E.g. if a reaction obeys the equation:
  • Rate = k[A][B], where the rate constant is 0.5dm3mol-1t-1, and the reactant concentrations are both 2moldm-3
  • The rate is 2moldm-3 × 2moldm-3 × 0.5dm3mol-1t-1 = 2moldm-3t-1
Calculating the rate constant

Calculating the rate constant

  • You can be given a rate equation and told to calculate the rate constant given some concentration data.
  • E.g. the rate equation for the production of I-Cl is: Rate = k[I2]1[Cl2]1
  • Given that the concentrations of I2 and Cl2 are 1moldm-3, and the rate of reaction is 40moldm-3t-1, what is the value of k?
  • k = 40moldm-3t-1 ÷ (1moldm-3)2 = 40mol-1dm3t-1

Test yourself on Orders, Rate Constants & Equations

  • In a reaction between molecule A and B, what will the rate be proportional to?

  • What happens if we double the amount of B molecules present in a reaction?

  • Which form is the rate equation always written in?

  • In the production of I-Cl: Rate = k[I2]1[Cl2]1
    The concentrations of I2 and Cl2 are 2 (ignoring units).
    If the rate of reaction is 80, what is the value of k?

  • For a given reaction, k = 40moldm-3t-1 ÷ (1moldm-3)2.
    What are the units of k?

Practise this topic for free