Sodium hypochlorite, NaClO\text{NaClO}NaClO, decomposes slowly at room temperature to produce oxygen gas, O2\text{O}_2O2, and sodium chloride, NaCl\text{NaCl}NaCl. This reaction can be accelerated significantly using transition metal oxide catalysts.
Write the balanced symbol equation for the catalytic decomposition of sodium hypochlorite.
A student investigates the rate of this decomposition using two different catalysts, P\text{P}P and Q\text{Q}Q. In each experiment, they use 50 cm350\text{ cm}^350 cm3 of sodium hypochlorite solution and 0.15 g0.15\text{ g}0.15 g of the catalyst. Below is a table showing the volume of oxygen gas collected over time:
| Time (seconds) | Volume of oxygen for Catalyst P\text{P}P (cm3\text{cm}^3cm3) | Volume of oxygen for Catalyst Q\text{Q}Q (cm3\text{cm}^3cm3) |
|---|---|---|
| 0 | 0.0 | 0.0 |
| 15 | 9.0 | 12.0 |
| 30 | 18.0 | 24.0 |
| 45 | 27.0 | 33.0 |
| 60 | 33.0 | 36.0 |
| 75 | 35.5 | 36.0 |
| 90 | 36.0 | 36.0 |
| 105 | 36.0 | 36.0 |
Explain why Catalyst Q\text{Q}Q is a more effective catalyst than Catalyst P\text{P}P. Refer to specific measurements from the table in your answer.
Explain why the final volume of oxygen gas collected (36.0 cm336.0\text{ cm}^336.0 cm3) is the same for both catalysts.
The student decides to repeat the experiment using 0.45 g0.45\text{ g}0.45 g of Catalyst P\text{P}P instead of 0.15 g0.15\text{ g}0.15 g. Predict the final volume of oxygen gas that will be collected at the end of the reaction, and explain your reasoning.