Question

Describe possible way(s) to shift the equilibrium to the right for the following reaction:

2AB (s) arrow 2A (s) + B2(g). Justify your answer. ΔH = +298 kJ
(Points : 5)

Answer 1

Well, what causes shifts in equilibrium?

Answer 2

Increases or decreases in reactants or products

Answer 3

Okay, good.

If there is a disturbance which favors the Reactants, which way does equilibrium shift?
If there is a disturbance which favors the Products, which way does equilibrium shift?

Once you answer these questions, you will be able to think of a few scenarios that will cause the equilibrium to shift to the right (favoring the products, the forward reaction).

And as for justification, you already know why :)

Answer 4

I there is a disturbance which favors reactants there will be a shift right, if thee is a disturbance in products it will shift left.

I am not sure how to manipulate the equation to show those shifts

Answer 5

Okay, so disturbances that favor the reactant will cause equilibrium to shift right.

Define the term "Favors" and apply it to the reactants (left side).

Answer 6

3AB(s)-->2A(s)+B2(g)

Answer 7

In that case the equation would be unbalanced.

You don't necessarily have to manipulate the equation (because it's given).

I think you meant to increase the [concentration] of the reactant. In that case, if you increase the concentration of AB, the equilibrium would shift to the right.

There are a few other ways to create a disturbance.

Answer 8

Is the concentration in the parenthesis?

Answer 9

Concentration as in 0.1 Molar, 2.00 Molar, 12.00 Molar

Answer 10

I am sorry but I completely do not understand.. I didn't get the mole thing at all

Answer 11

In theory if you increased the molarity of the reactants (favoring the reactant side), the equilibrium would have to shift to the right in order to restore balance.

Answer 12

right I understood that part I just do not know where I would write an increase in the mole