Respuesta :
The equilibrium constant Kc, for the reaction 2 NO₂(g) ⇌ N2(g) + 2O₂(g) is 4.77 × 10¹³.
What is Kc?
The equilibrium constant, Kc, is the ratio of the equilibrium concentrations of products over the equilibrium concentrations of reactants each raised to the power of their stoichiometric coefficients.
We are to determine the equilibrium constant, Kc for the reaction
2 NO₂(g) ⇌ N2(g) + 2O₂(g)
The equilibrium constant, Kc for this reaction is given by
2 NO2(g) ⇌ N2(g) + 2 O2(g)
(1) 1/2 N2(g) + 1/2 O2(g) ⇌ NO(g) Kc = 4.8 × 10 −10
(2) 2 NO2(g) ⇌ 2NO(g) + O2(g) Kc = 1.1 × 10−5
To create the first reaction from the two provided reactions, multiply one of them by two, switch the reactants and products, and then sum the results.
(1): 1/2 N2(g) + 1/2 O2(g) ⇌ NO(g) / x2
N2(g) + O2(g) ⇌ 2 NO(g) / switch reactants with products (equivalent to multiply by -1)
2 NO(g) ⇌ N2(g) + O2(g)
(2): 2 NO2(g) ⇌ 2NO(g) + O2(g)
Adding them you get:
2 NO(g) + 2 NO2(g) ⇌ 2NO(g) + O2(g) + O2(g)
After eliminating NO in both sides:
2 NO2(g) ⇌ 2NO(g) + O2(g)
Once the reaction has created, everything you multiplied by the reactions must now be done in the constant rather than the exponent. If you combine reactions, you multiply the constants by one another, which results in:
Kc = (4.8 × 10 −10)^(2*(-1)) * 1.1 × 10−5 = 4.8x10^13
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