A student performs the reaction shown below:
NaOH + HCl → NaCI + H20
She increases the concentrations of NaOH and HCl, and finds that NaCl is produced much more quickly. Which explains the outcome of her experiment?
The higher concentrations create a higher temperature in the solution.
NaCi requires a high concentration for any reaction to occur.
HOl acts as a catalyst, but only at high concentrations.
NoOH and HCl molecules collide more frequently at higher concentrations.
The correct explanation for the outcome of the student's experiment is: NoOH and HCl molecules collide more frequently at higher concentrations.
When the concentrations of NaOH and HCl are increased, there are more particles present in the solution. As a result, there is a higher chance of molecular collisions occurring. Increased collisions between NaOH and HCl increase the likelihood of successful reactions taking place, leading to a faster production of NaCl.
The other options are not accurate explanations for this outcome. The higher concentrations do not necessarily create a higher temperature in the solution, and NaCl does not require a high concentration for the reaction to occur. Moreover, there is no mention of HOl acting as a catalyst in the given reaction equation.