Hydrogen peroxide, H2O2\text{H}_2\text{O}_2H2O2, decomposes at room temperature to produce oxygen gas, O2\text{O}_2O2, and water, H2O\text{H}_2\text{O}H2O. This reaction is very slow but can be speeded up using a catalyst.
Write the balanced symbol equation for the catalytic decomposition of hydrogen peroxide.
A student investigates the rate of this decomposition using two different catalysts, X\text{X}X and Y\text{Y}Y. In each experiment, they use 40 cm340\text{ cm}^340 cm3 of hydrogen peroxide solution and 0.2 g0.2\text{ g}0.2 g of the catalyst. Below is a table showing the volume of oxygen gas collected over time:
| Time (seconds) | Volume of oxygen for Catalyst X\text{X}X (cm3\text{cm}^3cm3) | Volume of oxygen for Catalyst Y\text{Y}Y (cm3\text{cm}^3cm3) |
|---|---|---|
| 0 | 0.0 | 0.0 |
| 10 | 6.0 | 8.0 |
| 20 | 12.0 | 16.0 |
| 30 | 18.0 | 22.0 |
| 40 | 22.0 | 24.0 |
| 50 | 23.5 | 24.0 |
| 60 | 24.0 | 24.0 |
| 70 | 24.0 | 24.0 |
Explain why Catalyst Y\text{Y}Y is a more effective catalyst than Catalyst X\text{X}X. Refer to specific measurements from the table in your answer.
Explain why the final volume of oxygen gas collected (24.0 cm324.0\text{ cm}^324.0 cm3) is the same for both catalysts.
The student decides to repeat the experiment using 0.6 g0.6\text{ g}0.6 g of Catalyst X\text{X}X instead of 0.2 g0.2\text{ g}0.2 g. Predict the final volume of oxygen gas that will be collected at the end of the reaction, and explain your reasoning.