Given the reaction:
HCl(g) + H2O(l) → H3O+(aq) + Cl−(aq)
Which reactant acted as a Bronsted-Lowry acid?
A) H2O(l), because it accepted protons
B) H2O(l), because it produced hydronium ions C) HCl(g), because it donated protons
D) HCl(g), because it reacted with chloride ions

The correct answer is option C.

Explanation:

According to the Bronsted-Lowry conjugate acid-base theory:

For the given chemical equation:

Here, is loosing a proton, thus it is considered as an acid and after losing a proton, it forms which is a conjugate base.

And, is gaining a proton, thus it is considered as a base and after gaining a proton, it forms which is a conjugate acid.

Hence,the correct answer is option C.

d.) the average kinetic energy of the gas particles is greater in container b because its particles move faster.

im pretty sure its b