Concentration-Time Graphs (OCR A Level Chemistry A): Revision Note

Concentration-Time Graphs

Reaction Order Using Concentration-Time Graphs

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

  • This means that the reactant concentration decreases as time increases

  • The graph is a straight line going down as shown:

Concentration-time graph of a zero-order reaction

• The gradient of the line is the rate of reaction

  • Calculating the gradient at different points on the graph, will give a constant value for the rate of reaction

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

• Therefore:

Rate = k

• This equation means that the gradient of the graph is the rate of reaction as well as the rate constant, k

• 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 a first-order reaction

  • The graph is a steeper curve going downwards:

Concentration-time graph of a second-order reaction

Concentration-Time Graphs & Half-Life

Order of reaction from half-life

• The order of a reaction can also be deduced from its half-life (t_1/2 )

• For a zero-order reaction the successive half-lives decrease with time

  • This means that it would take less time for the concentration of reactant to halve as the reaction progresses

• The half-life of a first-order reaction remains constant throughout the reaction

  • The amount of time required for the concentration of reactants to halve will be the same during the entire reaction

• For a second-order reaction, the half-life increases with time

  • This means that as the reaction is taking place, it takes more time for the concentration of reactants to halve

Half-lives of zero, first and second-order reactions