When zinc reacts with hydrochloric acid, it produces hydrogen gas. as the reaction proceeds, why does the rate of production of hydrogen gas decrease?

a. the concentration of hydrogen gas decreases.
b. the concentration of the reactants decreases.
c. the hydrogen gas formed inhibits the reaction.
d. the hydrogen gas also reacts with the zinc metal.

b. The concentration of the reactants decreases.

Explanation: Rate law says that rate of a reaction is directly proportional to the concentration of the reactants each raised to a stoichiometric coefficient determined experimentally called as order.

k= rate constant

x = order with respect to

y = order with respect to

Thus when concentration of reactants decrease, the rate of the reaction decreases.

"among the transition metal elements, manganese and zinc have a slight lowering of electronegativities. the reason behind this is that the nuclear charges of these elements are slightly weaker than the other transition metal elements due to the way their valence electrons are filled up. both manganese and zinc have their valence electrons filled up to the 4th shell with 1 pair of electrons (4s2) completely occupying it. although the electrons in the 3rd shell (3d) are yet to be paired since the outer most shell is filled up, the ability of the nucleus to attract electrons is lessened. hence,   the electronegativity (or the ability to attract electrons) is lessened."

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