Magnesium metal reacts with dilute hydrochloric acid to produce hydrogen gas, H2\text{H}_2H2, and magnesium chloride.
Write the balanced symbol equation for this reaction.
A student investigates the rate of this reaction using two different catalysts, A and B. In each experiment, they use 40 cm340\text{ cm}^340 cm3 of hydrochloric acid and 0.1 g0.1\text{ g}0.1 g of catalyst. The volume of hydrogen gas collected over time is shown in the table below:
| Time (seconds) | Volume of hydrogen with Catalyst A (cm3\text{cm}^3cm3) | Volume of hydrogen with Catalyst B (cm3\text{cm}^3cm3) |
|---|---|---|
| 0 | 0.0 | 0.0 |
| 10 | 15.0 | 22.0 |
| 20 | 30.0 | 44.0 |
| 30 | 45.0 | 60.0 |
| 40 | 58.0 | 64.0 |
| 50 | 63.0 | 64.0 |
| 60 | 64.0 | 64.0 |
| 70 | 64.0 | 64.0 |
Explain why Catalyst B is a more effective catalyst than Catalyst A. Use data from the table to support your explanation.
The final volume of hydrogen gas collected in both experiments is 64.0 cm364.0\text{ cm}^364.0 cm3. Explain why this maximum volume is the same in both cases.
The student repeats the experiment using Catalyst A but increases its mass from 0.1 g0.1\text{ g}0.1 g to 0.4 g0.4\text{ g}0.4 g. What is the total volume of hydrogen gas produced at the end of this experiment?
Describe an experiment the student could do, and the results they would expect, to show that the reaction is faster at 50∘C50^\circ\text{C}50∘C than at 25∘C25^\circ\text{C}25∘C.