# Exercise 7 | Chemical Equilibrium

For the following reaction, which change would cause the equilibrium to shift to the right?

CH(g) + 2 H2S (g) $⇄$ CS(g) + 4 H(g)     [ΔHrxn = 25.0 kJ]

- increasing [reactant] or decreasing [product]

- increasing volume (right side = side with most moles of gas)

- decreasing pressure (right side = side with most moles of gas)

- increasing the temperature (ΔHrxn > 0)