Answer:
Keq = 0.133
The reactants are favored at equilibrium.
Explanation:
The initial concentration of N₂O₄ is 0.125 mol/1.00 L = 0.125 M
We can relate the initial concentrations with the concentrations at equilibrium using an ICE chart.
N₂O₄ ⇄ 2 NO₂
I 0.125 0
C -x +2x
E 0.125-x 2x
The concentration of N₂O₄ at equilibrium is 0.0750 M. Then,
0.0750 = 0.125 - x
x = 0.050
The concentration of NO₂ at equilibrium is:
2 x = 2 (0.050) = 0.100 M
The concentration equilibrium constant (Keq) is:
Keq = [NO₂]² / [N₂O₄]
Keq = 0.100² / 0.0750
Keq = 0.133
Since Keq < 1, the reactants are favored at equilibrium.
Answer:
The Keq value for the reaction is 0.13
The reactants are favored in the reaction.
Explanation:
The equilibrium expression: N[tex]^{2}[/tex]O4(g) ⇌ 2 [NO[tex]^{2}[/tex]](g)
Keq = squared of [NO[tex]^{2}[/tex]] divided by [N[tex]^{2}[/tex]O4]
Keq = squared of [0.10] divided by [0.075]
Keq = 0.13
Equilibrium constant (Keq) indicates what will be favoured at equilibrium, as it is a ratio that quantifies the position of a chemical equilibrium at a given temperature. It measures the extent to which reactants are converted to products.
If equilibrium constant is less than 1, the mixture contains mostly reactants. Which indicates more reactants are present at equilibrium. If equilibrium constant is equal to 1, then, the amount of products is roughly equal to the amount of reactants at equilibrium. If equilibrium constant is much greater than 1, more products are present at equilibrium.
In the question treated above, the reactants are N[tex]^{2}[/tex]O4(g). While, the products are: 2 [NO[tex]^{2}[/tex]](g).
