A student investigates the reaction between two different samples of magnesium carbonate, MgCO3\text{MgCO}_3MgCO3, Sample A and Sample B, with excess hydrochloric acid, HCl\text{HCl}HCl. Magnesium carbonate reacts with hydrochloric acid to produce magnesium chloride, MgCl2\text{MgCl}_2MgCl2, water, and carbon dioxide.
Write a balanced symbol equation for this reaction.
The student reacts Sample A with 50 cm3 of excess hydrochloric acid, measuring the volume of carbon dioxide gas produced every 30 seconds30\text{ seconds}30 seconds for 150 seconds150\text{ seconds}150 seconds. They repeat the experiment using Sample B and a fresh 50 cm3 sample of the same hydrochloric acid. The table shows their results:
| Time (seconds) | Volume of gas for Sample A (cm3\text{cm}^3cm3) | Volume of gas for Sample B (cm3\text{cm}^3cm3) |
|---|---|---|
| 0 | 0 | 0 |
| 30 | 25 | 20 |
| 60 | 40 | 35 |
| 90 | 40 | 46 |
| 120 | 40 | 52 |
| 150 | 40 | 52 |
What is the final volume of gas produced by Sample A at the end of the experiment?
Sample A contains less magnesium carbonate than Sample B. Describe how the results in the table show this.
The rate of reaction can be increased by using a more concentrated solution of hydrochloric acid or by increasing the temperature of the acid. Explain how each of these methods increases the rate of the reaction. Use ideas about collisions between particles.