kasse said:Homework Statement
Find the eq. constant for the reaction
CH3COOH (aq) + NO2- (aq) = CH3COO- (aq) + HNO2 (aq)
kasse said:I managed to find the correct solution by multiplying Ka1 and the 1/Ka2. Is 1/Ka2 the same av Kb?
kasse said:I managed to find the correct solution by multiplying Ka1 and the 1/Ka2. Is 1/Ka2 the same av Kb?
The equilibrium constant (Kc) is calculated by dividing the concentration of products by the concentration of reactants, with each concentration raised to the power of its coefficient in the balanced chemical equation. This can also be written as Kc = [C]c[D]d / [A]a[B]b.
If a reaction is at equilibrium, the concentrations of the reactants and products will remain constant over time. This means that the forward and reverse reactions are occurring at the same rate, and the concentrations of all substances involved are not changing.
The equilibrium constant is determined by the temperature of the reaction and the specific reactants and products involved. Therefore, it can change if any of these factors are altered. However, at a given temperature, the equilibrium constant remains constant.
The reaction quotient (Q) is calculated in the same way as the equilibrium constant, but with current concentrations instead of equilibrium concentrations. If Q is less than Kc, the reaction will proceed forward to reach equilibrium. If Q is greater than Kc, the reaction will proceed in the reverse direction. When Q is equal to Kc, the reaction is at equilibrium.
According to Le Chatelier's principle, if the concentration or pressure of a substance is increased, the reaction will shift in the direction that reduces the concentration or pressure. This will result in a change in the equilibrium constant. However, if the temperature remains constant, the equilibrium constant will remain constant as well.