Reversible equilibrium:
what would the effect be by adding hydrogen gas to:
3Fe(s)+4H20(i)<==>Fe3O4(s)+4H2(g)
and...
effect of adding chlorine gas to:
P4(s)+6Cl2(g)<===>4PCl3(i)
ah equilibrium, how annoying thou art...
since adding to either side of an equilibrium equation causes a dramatic increase to the opposite side, adding more H2 [a product] would increase the other side of the reaction, leaving you with more reactant.
the same principle applies to adding chlorine [a reactant] and would give you more product
Dude Cody, your right it is annoying!
have you had to solve the problems where you add something that reacts with both reactant and product but at a different rate? i printed off a second copy just to watch it burn when i was done.
To understand the effect of adding hydrogen gas to the reaction 3Fe(s) + 4H2O(i) ⇌ Fe3O4(s) + 4H2(g) and adding chlorine gas to the reaction P4(s) + 6Cl2(g) ⇌ 4PCl3(i), we need to consider Le Chatelier's principle. This principle states that when a system in equilibrium is subjected to a stress (such as changing the concentrations, pressure, or temperature), it will shift in a way that partially counteracts the stress.
1. Effect of Adding Hydrogen Gas:
When hydrogen gas is added to the reaction 3Fe(s) + 4H2O(i) ⇌ Fe3O4(s) + 4H2(g), the concentration of hydrogen gas increases. According to Le Chatelier's principle, the system will shift in a way that reduces this increase.
Since the forward reaction consumes hydrogen gas, the system will shift to the right to consume some of the added hydrogen gas. This means that the equilibrium will shift towards the formation of more Fe3O4(s) and H2O(i), resulting in a decrease in the concentration of H2(g). As a result, the concentration of Fe3O4(s) and H2O(i) will increase.
2. Effect of Adding Chlorine Gas:
When chlorine gas is added to the reaction P4(s) + 6Cl2(g) ⇌ 4PCl3(g), the concentration of chlorine gas increases. Again, Le Chatelier's principle predicts that the system will shift to counteract this increase.
In this case, the forward reaction (formation of PCl3) consumes chlorine gas. Thus, the system will shift to the left to consume some of the added chlorine gas. The equilibrium will shift towards the formation of more P4(s), resulting in a decrease in the concentration of PCl3. Hence, the concentration of P4(s) will increase.
It is important to note that while the added hydrogen gas or chlorine gas will cause a temporary shift in the equilibrium position, the equilibrium will eventually be reestablished to maintain a balance between the reactants and products.