Answer:
Kc=13.61
Explanation:
A chemical equilibrium is the situation in which the ratio between the amounts of reagents and products in a chemical reaction remains constant over time.
The equilibrium constant (Kc) is useful for the study of chemical equilibrium, being a constant that indicates whether the reaction is favored to the formation of products or to the formation of reactants.
Being:
aA + bB ⇔ cC + dD
where a, b, c, d are the stoichiometric coefficients of the reaction and A, B, C, D are the symbols or formulas of the different substances involved
Then:
[tex]Kc=\frac{[C]^{c} *[D]^{d} }{[A]^{a} *[B]^{b} }[/tex]
where [] is the Molar concentration of each of the substances in equilibrium.
In this case, you know: 2 SO₂(g) +O₂(g)⇌2 SO₃(g)
So: [tex]Kc=\frac{[SO_{3} ]^{2} }{[SO_{2}] ^{2} *[O_{2} ]}[/tex]
Being: [SO2]=0.48 M, [O2]=0.40 M, and [SO3]=1.12 M
[tex]Kc=\frac{[1.12]^{2} }{[0.48] ^{2} *[0.40 ]}[/tex]
Kc=13.61
Answer:
The equilibrium constant for this reactions is 13.61
Explanation:
Step 1: Data given
Concentrations at the equilibrium are:
[SO2]=0.48 M
[O2]=0.40 M
[SO3]=1.12 M.
Step 2: The balanced equation
2SO2(g) +O2(g) ⇌ 2SO3(g)
Step 3: Calculate Kc
Kc = [SO3]²/[O2]*[SO2]²
Kc = (1.12²) / (0.40 * 0.48²)
Kc = 13.61
The equilibrium constant for this reactions is 13.61
