Calculating Rates of Reactions (AQA GCSE Chemistry: Combined Science)

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Calculating rates of reactions

  • Reactions take place at different rates depending on the chemicals involved and the conditions
    • Some are extremely slow e.g. rusting and others are extremely fast e.g. explosives
  • The rate of reaction can be measured in two different ways:
    • How fast a reactant is used up
    • How fast a product is made
  • Three methods used to determine the rate of reaction are:
    • Mass loss - measuring the mass loss in the reactants over time
    • Gas collection - measuring the amount of a gas formed over time
    • Precipitation - measure the formation of a precipitate over time
  • Depending on the method used, the rate of reaction can be calculated using the appropriate equation:

Rate = fraction numerator bold amount bold space bold of bold space bold reactant bold space bold used over denominator bold time bold space bold taken end fraction   OR   Rate = fraction numerator bold amount bold space bold of bold space bold product bold space bold made over denominator bold time bold space bold taken end fraction

Formula triangle for calculating the rate of reaction

Rate of Reaction - Formula Triangle, IGCSE & GCSE Chemistry revision notes

This formula triangle can help with rearranging rate equations for calculations 

Measurements for rate

  • Time is always measured when determining the rate of a chemical reaction
    • Time is usually in seconds as many reactions studied in the lab are quite quick
  • The amount of reactant used up or product formed is the other measurement 
    • Several of these measurements are made to ensure that there is sufficient data to establish a conclusion 
    • Measuring the amount of product forming is usually easier than measuring the amount of reactant being used up
  • The calculation and units for rate depend on the reaction
    • If mass is being measured in grams, then the units for rate would be g/s
    • If volume is being measured in cm3 or dm3, then the units for volume would be cm3/s or dm3/s

Mass loss method

  • When a gas is produced in a reaction it usually escapes from the reaction vessel, so the mass decreases
  • For example, the reaction of calcium carbonate with hydrochloric acid producing carbon dioxide:

Calcium carbonate + hydrochloric acid → calcium chloride + water + carbon dioxide 

  • The mass is measured every few seconds and the change in mass over time is recorded as the gas escapes
  • The reaction is typically performed in a conical flask placed on top of a balance to measure the loss in mass 
    • Cotton wool can be placed in the neck of the flask to allow the gas to escape while stopping any materials from being ejected  

The set-up for measuring the reaction rate by mass loss

Using mass loss to measure the rate of a chemical reaction

A timer is started when the reactants are combined and the mass is recorded over time

  • However, one limitation of this method is the gas must be sufficiently dense or the change in mass is too small to measure on a 2 or 3 decimal place balance
    • So, carbon dioxide would be suitable (Mr = 44) but hydrogen would not (Mr = 2)

Gas collection method

  • When a gas is produced in a reaction, it can be trapped and its volume measured over time
    • This method can be used for any reaction that produces a gas but is particularly useful when the gaseous product is hydrogen or another gas with a small relative formula mass, Mr
  • For example, the reaction of magnesium with hydrochloric acid producing hydrogen:

Magnesium + hydrochloric acid → magnesium chloride + hydrogen  

  • The volume of gas produced over time is recorded
  • One gas collection set-up involves collecting a gas through water using an inverted measuring cylinder 
    • This technique is called the downward displacement of water

The set-up for measuring the reaction rate by gas collection

Gas collection using an inverted measuring cylinder

The gas displaces the water from the inverted measuring cylinder and the volume of gas produced is recorded over time 

  • Alternatively, the gas could be captured in a gas syringe which measures its volume

Alternative set-up for measuring the reaction rate by gas collection

Gas collection using a gas syringe

The gas fills the gas syringe and the volume of gas produced is recorded over time 

Precipitation method

  • Precipitation reactions form a solid precipitate when two clear solutions are mixed together
  • The precipitate clouds the reaction mixture so if the flask is placed over a piece of paper with a cross on it, the time it takes for the cross to disappear from view (due to the formation of the precipitate) can be measured
  • For example, the reaction of sodium thiosulfate and hydrochloric acid:

Sodium thiosulfate + hydrochloric acid → sodium chloride + sulfur dioxide + water + sulfur

  • The time taken for the cross to disappear is measured 

The disappearing cross experiment

The Disappearing Cross Experiment

The chemicals are mixed which forms a a precipitate. The time taken for the precipitate to block the cross from view is recorded

  • This method is susceptible to error though as they are subjective, given that different people may not agree on the exact moment that the cross disappears
  • Another disadvantage is that only one data point is produced per experiment, so a rate of reaction graph cannot be plotted

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Stewart

Author: Stewart

Expertise: Chemistry Lead

Stewart has been an enthusiastic GCSE, IGCSE, A Level and IB teacher for more than 30 years in the UK as well as overseas, and has also been an examiner for IB and A Level. As a long-standing Head of Science, Stewart brings a wealth of experience to creating Exam Questions and revision materials for Save My Exams. Stewart specialises in Chemistry, but has also taught Physics and Environmental Systems and Societies.