How to Determine Order of Reaction

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Knowing how different concentrations of chemicals influence the speed of a reaction is imperative for many chemical processes. The term 'reaction order' (or order of reaction) refers to how the concentration of one or more reactants (chemicals) affects the rate of the reaction. The overall order of any reaction is the sum of the order of all present reactants. Though looking at a balanced chemical equation will not help you determine the order of the reaction, you can gain this information by looking at the rate equation or by graphing the reaction in question.

Method 1
Method 1 of 3:

Analyzing the Rate Equation

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  1. The rate equation can help you determine the order of the reaction. This equation shows the increase or decrease of a particular substance with respect to time. Other equations related to the chemical reaction will not help you identify the order of the reaction. [1]
  2. Each reactant listed in the rate equation will have an exponent of either 0, 1, or 2 (above 2 is very rare). That exponent denotes the order of that reactant. Looking at each exponent: [2]
    • A zero means that the concentration for that reactant has no bearing on the rate of reaction.
    • A one means that increasing the concentration of this reactant will increase the rate of the reaction in a linear way (doubling the reactant doubles the rate).
    • A two means that the rate of the reaction will increase by the square of the increased concentration (doubling the reactant will increase the rate by four times).
    • Zero order reactants are often not listed in the rate equation, since any number to the zeroth power is equal to one.
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  3. The overall order of a reaction is the sum of each reactants' orders. Add the exponents of each reactant to find the overall reaction order. This number is usually less than or equal to two. [3]
    • For example, if reactant one is first order (an exponent of 1) and reactant two is first order (an exponent of 1) then the overall reaction would be a second order reaction.
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Method 2
Method 2 of 3:

Graphing Data Points

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  1. A linear graph refers to a graph that has a constant rate of change. In other words, the dependent variable will change as much in the first second as it does the second, third, and so on. A linear graph looks like a straight line on the page. [4]
  2. This will indicate how much reactant remains at any given point during the reaction. If this graph is linear, it means that the concentration of the reactant has no bearing on the rate at which the reaction proceeds. In this case, the reactant is a zeroth order reactant. [5]
  3. If graphing the natural log of the reactant results in a linear graph, the reactant is a first order reactant. This means that the concentration of the reactant impacts the rate of reaction. If the graph is not linear, you must graph test for a second order reaction. [6]
  4. A linear graph of [1/concentration of reactant] indicates a second order reaction. This means that the rate of the reaction will increase by the square of any increase in reactant. If this graph is not linear, you must try graphing zeroth and first order reactions. [7]
  5. Once you have found a linear graph for each reactant, you will know the order of each reactant. This allows you to calculate the overall reaction order. Add all reactant orders together. This is your reaction order for the whole reaction. [8]
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Method 3
Method 3 of 3:

Solving Practice Problems

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  1. You must know that if doubling the concentration of a reactant causes the rate to double, then that reactant is of the first order. In this case, both reactants are first order. The sum of two first order reactants is a second order reaction. [9]
  2. If changing the concentration of a reactant produces no change in rate, that reactant is said to be of the zeroth order. In this case, both reactants are of the zeroth order. Reacting two zeroth order reactions gives you an overall reaction order of zero. [10]
  3. The reactant that impacts the reaction rate is of the second order. The second reactant has no impact on rate and is of the zeroth order. The sum of orders is two, thus this is a second order reaction. [11]
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  • Question
    How do I write rate law of a chemical equation?
    Aquaeika
    Community Answer
    If you have measurements of rates, you can compare the rates from different experiments measured from different conditions. If this is homework and a series of elementary steps is given to you, you need to combine them to get rid of intermediates. Note that rate law NEVER contains intermediate.
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  • Question
    How do I know the order of reaction from equation?
    Aquaeika
    Community Answer
    If your equation refers to a rate law, your order is the sum of all the power of species present in the rate law. If your equation refers to a chemical equation, then it will equal to the number of molecules of reactants, only if it was an elementary step. Otherwise, rate law (and thus order of reaction) cannot be derived from just chemical equation alone.
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      References

      1. ↑ http://www.chemguide.co.uk/physical/basicrates/orders.html
      2. ↑ http://www.chemguide.co.uk/physical/basicrates/orders.html
      3. ↑ http://www.chemguide.co.uk/physical/basicrates/orders.html
      4. ↑ https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Supplemental_Modules_(Physical_and_Theoretical_Chemistry)/Kinetics/05%3A_Experimental_Methods/5.02%3A_Methods_of_Determining_Reaction_Order
      5. ↑ https://www.sparknotes.com/chemistry/kinetics/ratelaws/section2/page/3/
      6. ↑ https://www.sparknotes.com/chemistry/kinetics/ratelaws/section2/page/3/
      7. ↑ https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Supplemental_Modules_(Physical_and_Theoretical_Chemistry)/Kinetics/05%3A_Experimental_Methods/5.02%3A_Methods_of_Determining_Reaction_Order
      8. ↑ https://laude.cm.utexas.edu/courses/ch302/others/order.pdf
      9. ↑ https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Supplemental_Modules_(Physical_and_Theoretical_Chemistry)/Kinetics/03%3A_Rate_Laws/3.03%3A_The_Rate_Law/3.3.03%3A_Reaction_Order
      1. ↑ https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Supplemental_Modules_(Physical_and_Theoretical_Chemistry)/Kinetics/03%3A_Rate_Laws/3.03%3A_The_Rate_Law/3.3.03%3A_Reaction_Order
      2. ↑ https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Supplemental_Modules_(Physical_and_Theoretical_Chemistry)/Kinetics/03%3A_Rate_Laws/3.03%3A_The_Rate_Law/3.3.03%3A_Reaction_Order

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      To determine the order of reaction in a chemical equation, identify the rate equation from the reaction. Identify the order of each reactant based on its exponent, but do not include reactants with an exponent of 0. Add the order of all of the reactants together to find the overall reaction order. This number is usually less than or equal to 2. To find the order of reaction by graphic data points, read on!

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