given
PCl5(g)+heat <-> PCl3(g)+Cl2(g)
a. addition of cl2
answer : would shift to the left
b. increase in pressure:
answer: ?
c. removal of heat
answer: ?
d. Removal of PCl3 as it forms
answer: ?
please help! thanks!
All of the texts give really GREAT (and quite esoteric) descriptions of Le Chatelier's Principle. I find that putting it down to earth helps. In plain words, Le Chatelier's Principle says that when we do something to a system at equilibrium it will react in such a ways so as to UNDO what we did. So to take your first one, which you've answered correctly, if we add Cl2 it will try to undo that. How can it undo adding Cl2. It can use up the Cl2. How can it do that. It can react to the left; doing that uses up the added Cl2.
b. Increasing pressure makes it shift to the side with the fewer mols. That is the left side so it will shift to the left (1 mol gas on the left and 2 mols gas on the right)
Now you try the others.
I'll be glad to check you work..
To determine the effect of changes in pressure, temperature, and concentration on the given chemical reaction, we need to apply Le Chatelier's principle. This principle states that if a change is made to a system at equilibrium, the system will adjust itself to minimize the effect of that change.
b. Increase in pressure:
When the pressure is increased, according to Le Chatelier's principle, the equilibrium will shift in the direction that produces fewer gas molecules. In this case, the forward reaction produces two moles of gas (PCl3 and Cl2), while the reverse reaction produces only one mole of gas (PCl5). Therefore, increasing the pressure will shift the equilibrium to the left, favoring the formation of PCl5 (g).
c. Removal of heat:
If heat is removed from the system, the equilibrium will shift in the direction that produces more heat. The forward reaction is exothermic, meaning it releases heat, while the reverse reaction is endothermic (absorbs heat). Thus, removing heat from the system will cause the equilibrium to shift to the right, favoring the forward reaction and the production of PCl3 (g) and Cl2 (g).
d. Removal of PCl3 as it forms:
If PCl3 is removed from the system, the equilibrium will shift in the direction that replenishes the lost compound. According to Le Chatelier's principle, the system will shift to the right to produce more PCl3 to compensate for the removal. As a result, the equilibrium will shift to the right, favoring the formation of PCl3 (g) and Cl2 (g).
Remember that these answers are based on applying Le Chatelier's principle to the given chemical reaction.
b. Increase in pressure:
When the pressure is increased, according to Le Chatelier's principle, the equilibrium will shift in the direction that minimizes the number of gaseous molecules. In this case, the reaction produces one mole of gas (PCl5(g)) on the left side, and two moles of gas (PCl3(g) + Cl2(g)) on the right side. Therefore, increasing the pressure would shift the equilibrium to the right, to decrease the total gas moles.
c. Removal of heat:
Removing heat disrupts the balance of energy within the reaction. According to Le Chatelier's principle, the equilibrium will shift in the direction that opposes the change. Since heat is a reactant in the forward reaction, removal of heat will shift the equilibrium to the right, favoring the exothermic forward reaction.
d. Removal of PCl3 as it forms:
Removing PCl3 as it forms will disrupt the equilibrium. According to Le Chatelier's principle, the equilibrium will shift in the direction that replenishes the reacted substance. As PCl3 is removed, the equilibrium will shift to the right, favoring the formation of more PCl3 to compensate for the lost amount.