The production of water proceeds according to the following equation:
[tex]$2 H_2(g)+O_2(g) \rightarrow 2 H_2 O(g)$[/tex]
Which describes a way to speed up the collisions between hydrogen and oxygen molecules to produce more water?
A. Use a less-intense source of heat on the reactants.
B. Maintain the same temperature of the reactants.
C. Place the reactants in a smaller container.
D. Reduce the concentration of the reactants.
Answer (1)
Placing reactants in a smaller container increases their concentration.
Higher concentration leads to more frequent collisions between molecules.
Increased collisions speed up the reaction.
Therefore, placing the reactants in a smaller container is the correct answer.
Explanation
Analyzing the Options Let's analyze the options to determine which one speeds up collisions between hydrogen and oxygen molecules.
Use a less-intense source of heat on the reactants: Heating reactants increases their kinetic energy, leading to more frequent and energetic collisions. A less intense heat source would decrease the collision rate, so this option is incorrect.
Maintain the same temperature of the reactants: Maintaining the same temperature would keep the collision rate constant, not speed it up. This option is also incorrect.
Place the reactants in a smaller container: Placing the reactants in a smaller container increases their concentration. With more molecules in a smaller space, the frequency of collisions increases. This option seems promising.
Reduce the concentration of the reactants: Reducing the concentration means fewer molecules are present in the same volume, leading to fewer collisions. This option is incorrect.
Determining the Correct Option Based on the analysis, placing the reactants in a smaller container increases the concentration of the reactants, leading to more frequent collisions between hydrogen and oxygen molecules.
Conclusion Therefore, the correct answer is placing the reactants in a smaller container.
Examples
In a crowded room, people bump into each other more often than in an empty room. Similarly, increasing the concentration of reactants in a chemical reaction, like hydrogen and oxygen, by placing them in a smaller container, increases the likelihood of collisions and speeds up the reaction. This principle is used in industrial processes to optimize reaction rates and improve efficiency.
