Final answer:
The rate of production of hydrogen gas decreases as the reaction between zinc and hydrochloric acid proceeds due to a decrease in the concentration of the reactants. This decrease in concentration leads to fewer collisions between zinc particles and hydrochloric acid molecules, resulting in a slower rate of gas production.
Step-by-step explanation:
The rate of production of hydrogen gas decreases as the reaction between zinc and hydrochloric acid proceeds due to a decrease in the concentration of the reactants. In a chemical reaction, the rate of reaction is directly proportional to the concentration of the reactants. As the reaction progresses, the concentration of zinc and hydrochloric acid decreases, leading to a decrease in the rate of hydrogen gas production.
For example, in the reaction Zn(s) + 2HCl(aq) → ZnCl₂(aq) + H₂(g), if there is less zinc and hydrochloric acid available, fewer collisions between zinc particles and hydrochloric acid molecules will occur, resulting in a slower rate of gas production.
Furthermore, the reaction may also be limited by another factor, such as temperature or the presence of impurities. These factors can affect the reaction rate and contribute to a decrease in the rate of hydrogen gas production.