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
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
1 Answer
Explanation:
-
Write a chemical equation that is balanced
#H_2O + CO -> CO_2 + H_2#
Turns out it is already balanced. -
#K_"eq" = ([CO_2]^1[H_2]^1)/([H_2O]^1[CO]^1)#
Each one of these will have a exponent of
If the balanced chemical equation had a
#0.66 = (["0.134 M"]["3.33 M"])/(["0.750 M"][xcolor(white)(.)"M"])#
#x = "0.90 M"#
