Describe the effect on the concentration of the bold substance by the following change: decrease the volume
The equilibrium is: 2HF(g) <--> F2(g) + H2; change in H=536KJ
F2(g) is bolded.
Shouldn't F2(g) increase when voume is decreased? Why is there no change?
Thanks in advance.
you actually left out something very important:
2HF(g) <--> F2(g) + H2(g)
Hydrogen is a gas.
Notice that you have two volumes on the left, two volumes on the right at equilibrium. So reducing volume on both sides will have no effect on equilibrium.
So I have to count the number of gaseous molecules first? Thanks!
To understand the effect on the concentration of F2(g) when the volume decreases in the given equilibrium reaction, we need to consider the Le Chatelier's principle. According to this principle, when a change is applied to a system at equilibrium, the system tries to minimize the effect of that change and restore equilibrium.
In this case, when the volume is decreased, the system will try to reduce the number of gas molecules to minimize the effect. Since F2(g) is the only gas molecule on the product side, the system will try to decrease its concentration. However, there is no change in the concentration of F2(g) when the volume is decreased because it is already in its maximum concentration according to the stoichiometry of the balanced equation.
In the given equilibrium reaction, 2 moles of HF(g) produce 1 mole of F2(g). Therefore, F2(g) is already at its maximum concentration, and decreasing the volume has no additional effect on its concentration. Hence, there is no change in the concentration of F2(g) when the volume is decreased.
It's important to note that the change in volume will not directly affect the concentration of F2(g) in this particular equilibrium. However, it may affect other factors, such as the partial pressures of the gases involved, which can have an indirect influence on the equilibrium position.