Question

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.

Answer 1

Answer:

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

Explanation:

Hello,

In this case, for the given chemical reaction:

$CS_2(g) + 4H_2(g)\rightleftharpoons CH_4(g) + 2H_2S(g)$

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.

Answer 2

The statement that explained the behavior of the system should be option e. i.e. re-established of the equilibrium.

What is L-e Ch-at-el-ie-r’s Principle?

In the case when the pressure should be increased in the system so here the equilibrium should be shifted in the direction of the side with the minimum no of moles of gas. Here the total moles in the product side should be 3 while the reactant side it should be 5. So here the shifting of the equilibrium should be on the product side.

Therefore, the option e is correct.

Learn more about pressure here: https://brainly.com/question/24531151