Zinc metal reacts with dilute sulfuric acid to produce hydrogen gas, H2\text{H}_2H2, and zinc sulfate.
Write the balanced symbol equation for this reaction.
A student investigates the rate of this reaction using two different catalysts, X and Y. In each experiment, they use 50 cm350\text{ cm}^350 cm3 of sulfuric acid and 0.2 g0.2\text{ g}0.2 g of catalyst. The volume of hydrogen gas collected over time is shown in the table below:
| Time (minutes) | Volume of hydrogen with Catalyst X (cm3\text{cm}^3cm3) | Volume of hydrogen with Catalyst Y (cm3\text{cm}^3cm3) |
|---|---|---|
| 0 | 0.0 | 0.0 |
| 2 | 10.0 | 12.0 |
| 4 | 20.0 | 24.0 |
| 6 | 30.0 | 36.0 |
| 8 | 40.0 | 41.0 |
| 10 | 44.0 | 45.0 |
| 12 | 45.0 | 45.0 |
| 14 | 45.0 | 45.0 |
Explain why Catalyst Y is a more effective catalyst than Catalyst X. Use data from the table to support your explanation.
The final volume of hydrogen gas collected in both experiments is 45.0 cm345.0\text{ cm}^345.0 cm3. Explain why this maximum volume is the same in both cases.
The student repeats the experiment using Catalyst X but increases the mass from 0.2 g0.2\text{ g}0.2 g to 0.6 g0.6\text{ g}0.6 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 40∘C40^\circ\text{C}40∘C than at 20∘C20^\circ\text{C}20∘C.