Question

In the reaction of Zn(s) + 2HCl (aq) arrow ZnCl2 (aq) + H2 (g), if [HCl] increases from 2.6 M to 8.2 M:
(Points : 3)

The rate at which Zn disappears decreases.


The rate at which H2 appears decreases.


The rate at which ZnCl2 appears increases.


The concentration of Zn (s) also increases.

Answer 1

If the concentration of one of the reactants increase, how will this disturb equilibrium?

What change is needed to restore equilibrium?

Answer 2

The other would decrease so to restore equilibrium the other would have to increase?

Answer 3

Reactants vs. Products

If Reactants increase, to restore balance what must happen?

Answer 4

Decrease?

Answer 5

On the product side, to restore equilibrium, the products are made faster.

Answer 6

Think of a see-saw, if the left side is heavier, you must add more to the right to restore balance.

Answer 7

I am confused lol

Answer 8

If the [HCl] increases, it becomes easier to yield products. The rate of appearance of the products will increase.

Answer 9

Okay that makes more sense

Answer 10

But only in the case where you have an arbitrary amount of both reactants and products (this example).

If they give you a specific amount of reactants, the reaction will only reach equilibrium faster and it will level off, the unused reactant becomes excess and the other becomes limiter.

Answer 11

okay, I said the rate at which ZnCl2 appears increases

Answer 12

Yes :)

Answer 13

YaY! thank you!