Would either of the following reactions go almost completely to product at equilibrium?
a)2NO + 2H2 at equil N2 + 2H2O
Kc = 6.5 x 10 113
b)COCl at equil CO + Cl
Kc = 3.6 x 10 -16
How do you figure this out?
If that is Kc = 6.5 x 10^113, yes, that K is so large it favors the products. The second one is so small it will not produce much in the way of products.
To determine if a reaction goes almost completely to product at equilibrium, you can analyze the value of the equilibrium constant (Kc). Kc is a measure of the ratio of product concentrations to reactant concentrations at equilibrium. The larger the value of Kc, the more product is formed at equilibrium.
a) The reaction 2NO + 2H2 ⇌ N2 + 2H2O has an equilibrium constant Kc of 6.5 x 10^113. This extremely high value indicates that the concentration of products is much greater than the concentration of reactants at equilibrium. Therefore, this reaction goes almost completely to product at equilibrium.
b) The reaction COCl ⇌ CO + Cl has an equilibrium constant Kc of 3.6 x 10^-16. This very small value indicates that the concentration of reactants is much greater than the concentration of products at equilibrium. Therefore, this reaction does not go almost completely to product at equilibrium.
In summary, for reaction a) the equilibrium strongly favors the formation of products, while for reaction b) the equilibrium strongly favors the formation of reactants.
To determine whether a reaction will go almost completely to product at equilibrium, we need to compare the magnitude of the equilibrium constant (Kc) to determine if it is significantly greater than 1.
In reaction a): 2NO + 2H2 ↔ N2 + 2H2O, the equilibrium constant (Kc) is given as 6.5 x 10^113. Since this value is extremely large, it suggests that the reaction strongly favors the formation of products N2 and H2O. Therefore, it can be concluded that reaction a) goes almost completely to product at equilibrium.
In reaction b): COCl ↔ CO + Cl, the equilibrium constant (Kc) is given as 3.6 x 10^-16. Since this value is extremely small, it suggests that the reaction strongly favors the formation of reactant COCl. Therefore, it can be concluded that reaction b) does not go almost completely to product at equilibrium.
In summary, to figure out if a reaction goes almost completely to product at equilibrium, compare the magnitude of the equilibrium constant (Kc). If Kc is significantly larger than 1, the reaction goes almost completely to product. If Kc is significantly smaller than 1, the reaction does not go almost completely to product.