Concentration-Time Graphs (AQA A Level Chemistry)

Concentration-Time Graphs

Order of reaction from concentration-time graphs

• In a zero-order the concentration of the reactant is inversely proportional to time

  • This means that the concentration of the reactant decreases with increasing time

  • The graph is a straight line going down

Concentration-time graph of a zero-order reaction

• In a first-order reaction the concentration of the reactant decreases with time

  • The graph is a curve going downwards and eventually plateaus

Concentration-time graph of a first-order reaction

• In a second-order reaction the concentration of the reactant decreases more steeply with time

  • The concentration of reactant decreases more with increasing time compared to in a first-order reaction

  • The graph is a steeper curve going downwards

Concentration-time graph of a second-order reaction

Initial Rates Method

The Initial Rate Method

• The initial rate method is used to gather experimental data, to determine the order with respect to the reactants in the reaction

• The initial rate of a reaction is the rate right at the start of the reaction

  • This is used because right at the start of the reaction, we know the exact concentration of the reactants used

• The method involves setting up a series of experiments

• When carrying out the experiments:

  • The temperature must remain constant

  • For each experiment, the concentration of only of the reactants is altered - the rest must remain constant

  • The experiments are planned so that when the results are collected, they can be used to determine the order with respect to each reactant

  • For each experiment, a concentration-time graph is drawn

  • From each graph, the initial rate is calculated by drawing a tangent to the line at t = 0 and calculating the gradient

  • The gradient at t = 0 is the initial rate for that reaction

General Example

• Let's take the following general reaction as an example

2A + B + C → C + D

• We need to run a series of experiments at different concentrations of A, B and C, to determine how each affects the initial rate of the reaction

• Firstly, complete the experiment using the same concentration of A, B and C

• In another experiment, change the concentration of A but keep the concentrations of B and C the same as in experiment 1

• In a third experiment, change the concentration of B but keep the concentrations of A and C the same as in experiment 1

• And so on, until you have completed a series of experiments and collected the results

• Draw graphs for each experiment, draw a tangent at t=0 and calculate the gradient (the initial rate) for each graph

• Tabulate all of your results, and then use these to determine the order with respect to each reactant, to determine the rate equation for the reaction

A graph to show how to find the initial rate of a reaction (t=0)

Table of the results collected for the reaction

Rate Constant & Zero Order Graphs

Finding the Rate Constant of a Zero Order Reaction

• As shown above, a zero order reaction will give the following concentration-time graph

Concentration-time graph of a zero-order reaction

• The rate of the reaction isn't changing - if you were to calculate the gradient at different points on the graph, you would achieve a constant value

• Since the order with respect to the reactant is 0, a change in the concentration of the reactant will have no effect on the rate of the reaction

• Therefore:

Rate = k

• The rate of the reaction is the gradient of the graph, meaning that the rate constant, k, for the reaction will also be the gradient of the graph