# Question #ac0af

Jul 6, 2017

1. Increasing ${\text{H}}_{2}$ concentration

2. Increasing ${\text{Cl}}_{2}$ concentration

3. Raising temperature of reaction

#### Explanation:

We're asked to find three changes in the conditions that would results in a production of more of the product, $\text{HCl} \left(g\right)$. We can use Le Châtelier's equilibrium principle to help us.

1

One way to shift equilibrium to the right is by adding more ${\text{H}}_{2}$ to result in a higher concentration of ${\text{H}}_{2}$.

At the same temperature, the equilibrium constant is always the same for a particular reaction. Thus, the equilibrium must shift toward the right to counterbalance the increased reactant concentration. (At this point, the reaction quotient $Q < {K}_{c}$, so equilibrium shifts to the right.)

2

For the same reasons as in the above section, increasing the concentration of ${\text{Cl}}_{2}$ also shifts equilibrium toward the right.

3

We know that this reaction is endothermic (heat energy added to system throughout reaction).

Therefore, increasing the temperature at which the reaction proceeds produces more product.

Why? Treating heat as a reactant here (because it's added to form product), increasing it will result in an increase in the concentration of the other side (similar to how the first two examples counterbalanced the increased reaction concentrations).