The reaction system CS2(g) + 4H2(g) CH4(g) + 2H2S(g)
is at equilibrium. Which of the following statements describes the behavior of the system if the partial pressure of hydrogen is doubled?
a. As equilibrium is reestablished, the partial pressure of methane, CH4, decreases.
b. As equilibrium is reestablished, the partial pressure of carbon disulfide increases.
c. As equilibrium is reestablished, all the partial pressures will decrease.
d. As equilibrium is reestablished, the partial pressure of hydrogen sulfide decreases.
e. As equilibrium is reestablished, the partial pressure of hydrogen decreases.

e. As equilibrium is reestablished, the partial pressure of hydrogen decreases.

Explanation:

Hello,

In this case, for the given chemical reaction:

Considering the Le Chatelier's principle which states that adding more reactant shifts the reaction towards the products, condition that is related with the doubling of the hydrogen partial pressure, we can notice that e. As equilibrium is reestablished, the partial pressure of hydrogen decreases since the addition of hydrogen will be used to form more methane and hydrogen sulfide, for that reason, its amount is decreased to reattain equilibrium.

Regards.

it is stable as it is in group 0 which have full outer shells of electrons