Rate of Reaction - Calcium Carbonate & Hydrochloric Acid (OCR A Level Chemistry)

Revision Note

Test yourself
Richard

Author

Richard

Last updated

PAG 9.2: Rate of Reaction - Calcium Carbonate & Hydrochloric Acid

The Reaction of Calcium Carbonate and Hydrochloric Acid

  • At GCSE level, this reaction is a standard experiment to see the effect of changing the surface area of a reactant on the rate of reaction
    • Three sizes of calcium carbonate (marble) are commonly used:
      • Large chips
      • Small chips
      • Powder
  • The reaction itself cannot change

CaCO3 (s) + 2HCl (aq) → CaCl2 (aq) + H2O (l) + CO2 (g)

  • However, the application and analysis of the results shifts more towards the mathematical skills of accurately plotting graphs, drawing tangents and calculating gradients
  • This reaction can be monitored by measuring:
    1. The volume of carbon dioxide gas produced
    2. The mass loss from the reaction vessel

Method 1 - Volume of CO2 produced

  1. Support a gas syringe with a stand, boss and clamp.
  2. Add 50 cm3 of dilute hydrochloric acid to a conical flask
  3. Loosely connect the gas syringe 
  4. Measure 0.40 g of calcium carbonate
  5. Add the 0.40 g of calcium carbonate into the conical flask, replace the gas syringe and start the stopwatch
  6. Record the volume of gas produced every 10 seconds. Continue timing until no more carbon dioxide appears to be given off
  • Another method to achieve these results would be the downward displacement of water method, where an upturned measuring cylinder of water is placed in a water trough
    • This method still records the volume of carbon dioxide produced

Specimen results 1 - Volume of CO2 produced

  • Here is a set of typical results for this experiment

Rate of carbon dioxide production in the reaction of calcium carbonate and hydrochloric acid table

Time (s) 10 20 30 40 50 60
Volume of CO2 produced (cm3) 34 57 69 71 72 72

Graphing the results 1 - Volume of CO2 produced

1-4-2-caco3-and-hcl-reaction-rate-graph-1

Analysis 1 - Volume of CO2 produced

  • The curve of best fit is drawn on the graph
  • A tangent can then drawn starting from (0,0) to find the initial rate of reaction
  • The gradient of the tangent is calculated
    • This is the rate of reaction

1-4-2-caco3-and-hcl-reaction-rate-graph-2

  • In the example above, the rate of reaction is:
    • Gradient equals space fraction numerator straight capital delta y over denominator straight capital delta x end fraction space equals space 72 over 20 space equals space3.6 cm3 s-1 

Method 2 - Mass of the reaction vessel

  1. Measure 0.40 g of calcium carbonate into a weighing boat
  2. Add 50 cm3 of dilute hydrochloric acid to a conical flask
  3. Place the conical flask of hydrochloric acid AND the weighing boat of calcium carbonate onto the balance
  4. Measure the combined mass and record this as the t = 0 result
  5. Add the 0.40 g of calcium carbonate into the conical flask, replace the weighing boat onto the balance and start the stopwatch
  6. Record the mass every 10 seconds. Continue timing until no further mass is lost
  • It may be necessary to use more dilute concentrations of hydrochloric acid because it may not be realistically possible to record the mass every second
  • A data logger could be connected to the balance (if available) and this can track the mass over time 

Specimen results 2 - Mass of the reaction vessel

  • Here is a set of typical results for this experiment

Rate of change in mass in the reaction of calcium carbonate and hydrochloric acid table

Time (s) 0 10 20 30 40 50 60
Mass (g) 302.700 302.650 302.600 302.580 302.568 302.568 302.568

Graphing the results 2 - Mass of the reaction vessel

1-4-2-caco3-and-hcl-mass-reaction-rate-graph-1

Analysis 2 - Mass of the reaction vessel

  • The curve of best fit is drawn on the graph
  • A tangent can then drawn starting from (0,0) to find the initial rate of reaction
  • The gradient of the tangent is calculated
    • This is the rate of reaction

1-4-2-caco3-and-hcl-mass-reaction-rate-graph-2

  • In the example above, the rate of reaction is:
    • Gradient equals space fraction numerator straight capital delta y over denominator straight capital delta x end fraction space equals space fraction numerator 0.2 over denominator 38 end fraction space equals space(a loss of) 5.26 x 10-3 g s-1 
  • A simpler version of this practical can be done by hitting the TARE / reset button on the balance when the calcium carbonate is added
    • This then records the mass lost and can be used to give a graph with a curve more like the volume of CO2 produced graph

You've read 0 of your 5 free revision notes this week

Sign up now. It’s free!

Join the 100,000+ Students that ❤️ Save My Exams

the (exam) results speak for themselves:

Did this page help you?

Richard

Author: Richard

Expertise: Chemistry

Richard has taught Chemistry for over 15 years as well as working as a science tutor, examiner, content creator and author. He wasn’t the greatest at exams and only discovered how to revise in his final year at university. That knowledge made him want to help students learn how to revise, challenge them to think about what they actually know and hopefully succeed; so here he is, happily, at SME.