Question

Question #af614

Answer 1

Here's what I got.

Explanation:

You're dealing with a chemical reaction that involves gases, so you can write two equilibrium constants, one that uses the equilibrium concentrations of the species, `K_c`, and one that uses the equilibrium partial pressures of the species, `K_p`.

In both cases, you're going to be using the ratio that exists between the products and the reactants.

For equilibrium concentrations, you will have

`K_c = (["CO"] * ["H"_2]^3)/(["CH"_4] * ["H"_2"O"])`

Notice that the equilibrium concentration of each species is raised to the power of the stoichiometric coefficient that the species has in the balanced chemical equation, i.e. `1` for `"CO"`, `"CH"_4`, and `"H"_2"O"`, and `3` for `"H"_2`.

For equilibrium partial pressures, you will have

`K_p = (("CO") * ("H"_2)^3)/(("CH"_4) * ("H"_2"O"))`

This time. the partial pressure of each species is raised to the stoichiometric coefficient that the species has in the balanced chemical equation.