How will the equilibrium: Heat energy + CH4 + 2H2S = CS2 + 4H2 be affected by the following?

a) A decrease in temperature?
b) The addition of H2
c) The removal of some CH4
d) An increase in the volume of the container
e) The addiotion of a catalyst.

i know that [CH4] goes up, [H2S] goes up, [CS2]goes down and [H2] goes down.

and also, e) is no change am i correct?

I assume everything is a gas.

You have 5 questions and one answer? Your answer is correct for part a, part b and part c. part e is correct. For part d the reaction shifts to the right so CH4 and H2S go down; H2 and CS2 to up.

Let's break down each scenario and see how it affects the equilibrium:

a) A decrease in temperature:
According to Le Chatelier's principle, a decrease in temperature favors the exothermic reaction. As a result, the reaction will shift in the direction that produces more heat. In this case, heat is produced on the left side of the equation, so the reaction will shift to the left. Consequently, the concentrations of CH4 and H2S will increase, while the concentrations of CS2 and H2 will decrease.

b) The addition of H2:
By adding H2, you are increasing the concentration of one of the reactants. According to Le Chatelier's principle, this will cause the reaction to shift in the direction that consumes the added substance. In this case, adding H2 will drive the reaction to the right, resulting in an increase in the concentrations of CS2 and H2, while the concentrations of CH4 and H2S will decrease.

c) The removal of some CH4:
Removing CH4 from the system will decrease the concentration of this reactant. According to Le Chatelier's principle, the reaction will shift in the direction that replenishes the missing substance. In this case, the reaction will shift to the right, leading to an increase in the concentrations of CS2 and H2, while the concentrations of CH4 and H2S will decrease.

d) An increase in the volume of the container:
Increasing the volume of the container causes a decrease in pressure. According to Le Chatelier's principle, the reaction will shift in the direction that produces more molecules of gas (to compensate for the decrease in pressure). In this case, the reaction will shift to the right since there are more molecules of gas on the right side of the equation. As a result, the concentrations of CS2 and H2 will increase, while the concentrations of CH4 and H2S will decrease.

e) The addition of a catalyst:
Adding a catalyst does not affect the equilibrium position of the reaction. It only speeds up the rate at which the reaction reaches equilibrium. Therefore, the concentrations of all species remain the same.

So, your understanding is correct for the effects of temperature, addition of H2, removal of CH4, and increase in volume. Additionally, you are also correct that the addition of a catalyst will not cause any changes in the concentrations of the species involved in the reaction.

Let's analyze the effects of each factor on the given equilibrium equation:

a) A decrease in temperature:
According to Le Chatelier's principle, when the temperature decreases, the equilibrium will shift in the direction that produces heat. In this case, the forward reaction is exothermic, meaning it releases heat. To counteract the decrease in temperature, the equilibrium will shift towards the forward direction, leading to an increase in the formation of CH4 and H2S, while reducing the formation of CS2 and H2.

b) The addition of H2:
The addition of H2 will cause the equilibrium to shift in the direction that consumes H2. Since the forward reaction requires H2, the equilibrium will shift towards the product side, resulting in a decrease in H2 concentration. As a result, the concentrations of CH4 and H2S will decrease, while the concentration of CS2 will increase.

c) The removal of some CH4:
Removing CH4 will disrupt the equilibrium balance. In response, the equilibrium will shift towards the direction that replenishes CH4, which is the forward direction. Consequently, the concentration of CH4 will increase, while the concentrations of H2S and CS2 will decrease.

d) An increase in the volume of the container:
If the volume is increased, the equilibrium will shift towards the side with more moles of gas to restore the balance. In this case, the forward reaction has fewer moles of gas compared to the reverse reaction. Therefore, the equilibrium will shift in the reverse direction, resulting in an increase in the concentrations of CS2 and H2, while reducing the concentrations of CH4 and H2S.

e) The addition of a catalyst:
The addition of a catalyst does not directly affect the equilibrium concentrations. It provides an alternative reaction pathway with lower activation energy, enabling the reaction to proceed at a faster rate. As a result, the equilibrium will be reached more quickly, but the final concentrations of the reactants and products will remain the same.

So, in summary:
a) The concentrations of CH4 and H2S will increase, while the concentrations of CS2 and H2 will decrease.
b) The concentrations of CH4 and H2S will decrease, while the concentration of CS2 will increase.
c) The concentration of CH4 will increase, while the concentrations of H2S and CS2 will decrease.
d) The concentrations of CS2 and H2 will increase, while the concentrations of CH4 and H2S will decrease.
e) No change in equilibrium concentrations, but the reaction rate will be increased.