write the equilibrum constant expression for Kp of the following:
a.) O2-->--<2O3(g)
b.)SiH4(g) + 2O2(g)-->--<SiO(s) + 2H2O(g)
c.)MgO(s) + SO2(g) + O2(g)-->--<MgSO4(s)
d.)2PbS(s) + 3O2(g)-->--< 2PbO(s) + 2SO2(g)
This is a fundamental concept that you need to know how to do yourself. If you will explain what you don't understand I ca help you through it. Basically it's partial pressure of products over partial pressure reactants with coefficients becoming exponents. Solids are not included in Kc OR Kp. Pure liquids aren't either.
To write the equilibrium constant expression for Kp, you need to determine the stoichiometric coefficients of the reactants and products and raise them to the power of their coefficients in the balanced chemical equation. Here's how you can do that for each given reaction:
a.) O2 --> 2O3(g)
The balanced equation shows that the stoichiometric coefficient of O2 is 1 and that of O3 is 2. Therefore, the equilibrium constant expression for this reaction is:
Kp = [O3]^2 / [O2]
b.) SiH4(g) + 2O2(g) --> SiO(s) + 2H2O(g)
The balanced equation reveals that the stoichiometric coefficients of SiH4 and SiO are 1, and those of O2 and H2O are 2. Hence, the equilibrium constant expression becomes:
Kp = [SiO] / [SiH4] * [H2O]^2 / [O2]^2
c.) MgO(s) + SO2(g) + O2(g) --> MgSO4(s)
In this equation, the stoichiometric coefficients of MgO, SO2, and MgSO4 are 1, 1, and 1, respectively. As there is no gas involved, the Kp expression is not required.
d.) 2PbS(s) + 3O2(g) --> 2PbO(s) + 2SO2(g)
For this reaction, the stoichiometric coefficients of PbS, O2, PbO, and SO2 are 2, 3, 2, and 2, respectively. Since only gases participate in the reaction, we can write the equilibrium constant expression using the partial pressures of the gases:
Kp = (P(PbO)^2 * P(SO2)^2) / (P(PbS)^2 * P(O2)^3)
Make sure to balance the equation correctly before writing the equilibrium constant expression to ensure accurate results.