To speed up the collisions between hydrogen and oxygen molecules and produce more water, we need to consider the factors that influence the frequency and energy of these collisions. Here's a step-by-step analysis of each option:
1. Use a less-intense source of heat on the reactants.
- Heat increases the kinetic energy of molecules, which in turn increases the frequency and energy of collisions. Using a less-intense source of heat would actually decrease the energy available for collisions, thus slowing down the reaction rate. This option is not effective in speeding up the collisions.
2. Maintain the same temperature of the reactants.
- Keeping the temperature constant means that the kinetic energy and frequency of collisions remain unchanged. This approach does not increase the number of collisions nor their energy, and thus does not speed up the reaction. This option is neutral in terms of effect.
3. Place the reactants in a smaller container.
- Placing the reactants in a smaller container increases the concentration of molecules in a given space. Higher concentration means that molecules are closer to each other, leading to more frequent collisions. This increase in collision frequency enhances the rate of reaction, thereby producing more water. This option effectively speeds up the reaction.
4. Reduce the concentration of the reactants.
- Reducing the concentration of reactants means that there are fewer molecules in a given volume. This reduction decreases the frequency of collisions between hydrogen and oxygen molecules, slowing down the reaction rate. This option is counterproductive for speeding up the reaction.
Based on this step-by-step analysis, the most effective way to speed up the collisions between hydrogen and oxygen molecules is:
Place the reactants in a smaller container.
Therefore, the correct choice is: 3. Place the reactants in a smaller container.
