Predict the effect of each of the following on the indicated equilibrium system in terms of which reaction will be favored (forward, reverse, or neither)
H2(g)+Cl2(g)<=>2HCl(g) +184 kJ
A)addition of Cl2
B)removal of HCl
C)increased pressure
D)decreased temperature
E)removal of H2
F)decreased pressure
G)addition of a catalyst
H)increased temperature
I)decreased system volume
I really don't get these at all. Please help! Thanks so much!
The forward reaction gives off heat. Would the abilty to give off heat be enhanced if it were cooled?
The forward reaction produces as many volumes of gas as it had in the beginning. Will that reaction be favored if pressure is changed?
If the reactants are removed, would not the reverse reaction tend to increase them?
I will be happy to critique your thinking.
I'd be happy to help you understand the effects of each of the factors on the equilibrium system!
A) Addition of Cl2:
When Cl2 is added to the system, according to Le Chatelier's principle, the system will try to counteract the increase in Cl2 concentration by shifting the equilibrium towards the side with fewer Cl2 molecules. Therefore, the system will be shifted to favor the reverse reaction.
B) Removal of HCl:
If HCl is removed from the system, the equilibrium will shift towards the side with fewer HCl molecules to compensate for the loss. In this case, the system will favor the forward reaction to restore the balance.
C) Increased pressure:
Increasing the pressure affects the system based on the number of moles of gas involved in the reaction. In this case, since the forward reaction produces two moles of gas (2HCl), increasing the pressure will favor the side with fewer moles of gas. Therefore, the equilibrium will shift towards the forward reaction to decrease the pressure.
D) Decreased temperature:
Lowering the temperature will favor the exothermic reaction since the forward reaction gives off heat. The system will shift in the direction that absorbs heat, which is the forward reaction. Therefore, the equilibrium will shift towards the forward reaction.
E) Removal of H2:
Removing H2 from the system will cause the equilibrium to shift towards the side with fewer H2 molecules to maintain balance. In this case, it will favor the reverse reaction to replenish the lost H2.
F) Decreased pressure:
Decreasing the pressure will favor the side with more moles of gas. Since the forward reaction produces two moles of gas (2HCl), decreasing the pressure will shift the equilibrium towards the forward reaction.
G) Addition of a catalyst:
The addition of a catalyst does not affect the equilibrium position. It only speeds up the rate at which equilibrium is achieved but does not shift the equilibrium towards either the forward or reverse reaction.
H) Increased temperature:
Increasing the temperature will favor the endothermic reaction to absorb heat. Since the forward reaction is exothermic, the system will shift towards the reverse reaction to absorb the excess heat.
I) Decreased system volume:
Decreasing the system volume will increase the pressure. As discussed earlier, increasing the pressure favors the side with fewer moles of gas. Therefore, the equilibrium will shift towards the side with fewer moles of gas, which in this case is the forward reaction.
It's great that you are questioning and trying to understand the reasoning behind each answer. Please let me know if there's anything else I can help you with!