Question

A student performs the reaction shown below.

NaOH + HCl → NaCl + H2O
She increases the concentrations of NaOH and HCl, and finds that NaCl is produced much more quickly. Which explains the outcome of her experiment?

NaOH and HCl molecules collide more frequently at higher concentrations. (I think it's this one)

NaCl requires a high concentration for any reaction to occur.

HCl acts as a catalyst, but only at high concentrations.

The higher concentrations create a higher temperature in the solution.

Answer 1

Answer: Option (a) is the correct answer.

Step-by-step explanation:

According to collision theory, more is the number of collisions more will be the rate of reaction, that is, more quickly product will be formed.

Therefore, when we increase the concentration of reactants then there will be increase in number of reactant molecules. Hence, more will be the reactant molecules more will be the collisions.

Thus, we can conclude that in the given reaction NaOH and HCl molecules collide more frequently at higher concentrations.

Answer 2

I believe the correct answer from the choices listed above is the first option. The outcome is best explained by the statement that NaOH and HCl molecules collide more frequently at higher concentrations. This is because more reactant molecules are present and available to have a reaction. Hope this helps. Have a nice day.