Write the equilibrium constant expression, K, for each of the following reactions. Where appropriate, designate the K as Ksp.
2H2(g) + O2(g)<-->2H2O(g)
2Hg(l) + Cl2(g) <-->Hg2Cl2(s)
See above.
To write the equilibrium constant expression, we need to first understand what the equilibrium constant represents.
The equilibrium constant (K) is a measure of the position of the equilibrium for a given chemical reaction. It gives us information about the relative concentrations of reactants and products at equilibrium.
For a general reaction:
aA + bB <--> cC + dD
The equilibrium constant expression can be written as:
K = ([C]^c * [D]^d) / ([A]^a * [B]^b)
Now, let's write the equilibrium constant expressions for the given reactions:
1. For the reaction: 2H2(g) + O2(g) <--> 2H2O(g)
The equation shows a gaseous reaction, so we can use the equilibrium constant expression for gases.
The equilibrium constant expression is:
K = ([H2O]^2) / ([H2]^2 * [O2])
2. For the reaction: 2Hg(l) + Cl2(g) <--> Hg2Cl2(s)
This reaction involves a liquid and a solid, so we treat the concentrations of solids and liquids as constants.
The equilibrium constant expression is:
K = [Hg2Cl2] / ([Hg]^2 * [Cl2])
In this case, we designate K as Ksp to indicate that it is the solubility product constant, which is specific to reactions involving the dissolution of a solid.
It's important to note that the equilibrium constant expressions may change depending on the reaction conditions, such as temperature and pressure.