What is the correct equilibrium constant for the following reaction?
2NO(g) + 2H2(g) ⇔ N2(g) + 2H2O
a) Keq = ([H2]^2 [NO]^2) / ([N2][H2O]^2)
b) Keq = ([N2][H2O]) / ([H2][NO])
c) Keq = ([N2]^2[H2O]) / (2[H2]^2 [NO])
d) Keq = ([N2][H2O]^2) / ([H2]^2 [NO]^2)
e) Keq = ([H2][NO^2) / ([N2][H2O]^2)
The correct equilibrium constant for the following reaction is:
b) Keq = ([N2][H2O]) / ([H2][NO])
ARE YOU SURE?
I apologize for the confusion. You are correct, I made an error in my response.
The correct equilibrium constant for the reaction
2NO(g) + 2H2(g) ⇔ N2(g) + 2H2O(g)
is:
d) Keq = ([N2][H2O]^2) / ([H2]^2 [NO]^2)
Thank you for pointing out the mistake.
what is the correct answer?
The correct answer is:
d) Keq = ([N2][H2O]^2) / ([H2]^2 [NO]^2)
To determine the correct equilibrium constant for the given reaction, we can use the law of mass action, which states that the equilibrium constant (Keq) is the ratio of the concentrations of the products raised to their stoichiometric coefficients divided by the concentrations of the reactants raised to their stoichiometric coefficients.
Looking at the balanced reaction:
2NO(g) + 2H2(g) ⇔ N2(g) + 2H2O
The stoichiometric coefficients in the reaction are:
Reactants: NO(g) and H2(g)
Products: N2(g) and H2O
Now we can write the equilibrium constant expression using the concentrations (denoted by square brackets) of the species involved:
Keq = ([N2][H2O]^2) / ([H2]^2 [NO]^2)
Comparing this expression with the options given, we find that the correct equilibrium constant expression is represented by:
d) Keq = ([N2][H2O]^2) / ([H2]^2 [NO]^2)