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Why the reaction mixture doesn't have 50 percents reactants and 50 percents products at equilibrium position?
Chemical equilibrium occurs when the rate of the forward reaction is equal to the rate of the reverse reaction. Take this example:
2NO2(g) ↔
N2O4(g)
At this point of the reaction the rate of N2O4 produced from NO2 is the same as the rate of NO2 produced from N2O4. The key aspect to keep in mind is that the amounts (of moles) of products and reactants at equilibrium is not always 50%/50%. It is usually not.
Finding the amounts of products and reactants present during a reaction can be found using Q. Q is known as the reaction quotient. Q can be found like so:
Q=[products]
/[reactants]
reaction quotient =
concentrations of products (M) / concentrations of reactants
Q is used to find this ratio at a certain point in time during a reaction (not at
equlilibrium)
Most likely, you will be given Keq
, the equilibrium constant, for a reaction. The value tells you the concentrations of products/reactants at equilibrium. Comparing Q and Keq
will tell you whether a reaction is at equilibrium.
Not to get off topic, the answer is that equilibrium does not mean that the reaction mixture has 50% reactants and 50% products. Equilibrium means that the rate of the forward reaction equals the rate of the reverse reaction.
What else can I help you with?
What is used to describe the conditions of a reaction to equilibrium?
An equilibrium constant
What factors influence the position of equilibrium in a chemical reaction?
The position of equilibrium in a chemical reaction is influenced by factors such as temperature, pressure, concentration of reactants and products, and the presence of catalysts. These factors can shift the equilibrium towards the formation of more products or more reactants, depending on the conditions of the reaction.
Which occurs faster at equilibrium the formation of products from reactants or reactants from the product?
At equilibrium, the formation of products from reactants will be faster.
What happens when a base is added to water and the position of equilibrium lies to the left?
When a base is added to water and the equilibrium position shifts to the left, it means that the reaction is favoring the formation of the reactants rather than the products. This indicates that the base is not fully dissociating in water and the concentration of the reactants is higher than the products.
Are the amounts of reactants and products equal when equilibrium is reached?
At equilibrium, the rates of the forward and reverse reactions are equal, but the amounts of reactants and products may not be equal. The concentrations of reactants and products can vary depending on the specific equilibrium constant for the reaction.
What is the equilibrium constant of a reaction?
It is the ratio of the concentrations of products to the concentrations of reactants.
What is used to describe the conditions of a reaction to equilibrium?
An equilibrium constant
What factors influence the position of equilibrium in a chemical reaction?
The position of equilibrium in a chemical reaction is influenced by factors such as temperature, pressure, concentration of reactants and products, and the presence of catalysts. These factors can shift the equilibrium towards the formation of more products or more reactants, depending on the conditions of the reaction.
Which occurs faster at equilibrium the formation of products from reactants or reactants from the product?
At equilibrium, the formation of products from reactants will be faster.
What ways can equilibrium be shifted?
Equilibrium can be shifted by changing the concentration of reactants or products, adjusting the temperature, altering the pressure (for gases), or adding a catalyst. By changing these factors, the equilibrium position can be shifted towards either the products or the reactants to favor the desired reaction.
Why the reaction mixture does not have 50 percent reactants and 50 percent products at equilibrium position?
At equilibrium, the reaction mixture does not have 50 percent reactants and 50 percent products because the reaction has reached a dynamic state where the rates of the forward and reverse reactions are equal. This means that both reactants and products are continuously being formed and consumed at the same rate, leading to a constant concentration of reactants and products. The specific ratio of reactants to products at equilibrium is determined by the equilibrium constant for the reaction, which is unique to each reaction and depends on factors such as temperature and pressure.
Why are there more products than reactants after establishing equilibirium?
When a reaction reaches equilibrium, it means the rates of the forward and reverse reactions are equal. If there are more products present than reactants at equilibrium, it suggests that the equilibrium position favors the formation of products over reactants. This could be due to factors such as temperature, pressure, concentration, or the nature of the reaction itself.
What can effect equilibrium shifts?
Changes in concentration, pressure, or temperature can all affect the equilibrium position of a reaction. Adding or removing reactants or products, changing the volume of the container, or altering the temperature can lead to shifts in equilibrium to favor the formation of products or reactants. Additionally, catalysts do not affect the position of equilibrium but can speed up the attainment of equilibrium.
What will happen to the concentration of reactants after an equilibrium reaction shifts to the left?
Increasing the concentration of reactants will shift the equilibrium towards the products. The equilibrium will always shift to reduce the change you caused. If you add more products, it shifts toward reactants. This is known as the Le Chatelier Principle.See the Web Links to the left of this answer for more about this.
When equilibrium shifts to the reactants in response to stress how is the equilibrium position changed?
When the concentration increases, the equilibrium shifts away from the substance. Equilibrium is based on the molarity of the reactants. Increasing concentration increases the amount of that reactant in the solution.
What happens when a base is added to water and the position of equilibrium lies to the left?
When a base is added to water and the equilibrium position shifts to the left, it means that the reaction is favoring the formation of the reactants rather than the products. This indicates that the base is not fully dissociating in water and the concentration of the reactants is higher than the products.
What describes the two phases is dynamic equilibrium?
reactants are turning into products. products are turning into reactants.
