Question

Can someone please help me with Equilibrium?

When H2O and CO react at 979°C, the products are CO2 and H2. The equilibrium constant (in terms of equilibrium concentrations of reactants and products) for the reaction below is 0.66 at 979°C.
If the following concentrations are measured after the reaction reaches equilibrium, what is the concentration of CO(g) in the equilibrated mixture? answer will be in M
Component: Measured Equilibrium Concentration
H_2 0 (g) 0.750 M
CO_2 (g) 0.134 M
H_2 (g) 3.33 M

Answer 1

`[CO] = "0.90 M"`

Explanation:

1. Write a chemical equation that is balanced
   `H_2O + CO -> CO_2 + H_2`
   Turns out it is already balanced.

2. `K_"eq" = ([CO_2]^1[H_2]^1)/([H_2O]^1[CO]^1)`

Each one of these will have a exponent of `1`, which derived straight from the balanced chemical equation.

If the balanced chemical equation had a `2` or `3` as a coefficient then that would have to be reflected in the `K_"eq"` equation as an exponent, not a coefficient.

`0.66 = (["0.134 M"]["3.33 M"])/(["0.750 M"][xcolor(white)(.)"M"])`

`x = "0.90 M"`