Chemical Equilibrium Lab Report
1. Briefly explain the following:
a. Chemical equilibrium- Chemical equilibrium is the state of a reaction when the concentrations of the reactants and products are no longer changing and remain constant. The forward reaction proceeds at the same rate as the reverse reactions making them equal. This type of equilibrium is also named dynamic equilibrium or a dynamic process.
When a reaction has reached its chemical equilibrium, the constant K value will remain constant unless the temperature changes. If conditions change the concentration in the experiment of any species in the equilibrium reaction, all other species concentrations must also change in order for K to remain constant.
b. Equilibrium constant- When a chemical reaction has reached equilibrium a reaction quotient is given a value symbolized in an equation by the letter K. Normally this value is a ratio expressing the relationship between the concentration of the products to the concentration of the reactants at equilibrium. The two different types of equilibrium reactions are heterogeneous and homogeneous. The reaction will move to the left if the K value is less than one and if the value of K is greater than one the reaction will move to the right.
c. …show more content…
LeChatelier’s principle- This principle is also known as called Chatelier's principle or "The Equilibrium Law” named after Henry Louis Le Châtelier. This principle states that if the equilibrium state of a system is disturbed by an external stress, a shift in the system will take place to counteract the effect of that disturbance to maintain equilibrium. This disruption can be caused by a change in concentration of the reactants or products, a temperature change, or pressure change.
2. List four factors that can affect the position of equilibrium. Of these four factors, which is the only one that can alter the value of the equilibrium constant?
1. Changes in pressure
2. Changes in
a. Chemical equilibrium- Chemical equilibrium is the state of a reaction when the concentrations of the reactants and products are no longer changing and remain constant. The forward reaction proceeds at the same rate as the reverse reactions making them equal. This type of equilibrium is also named dynamic equilibrium or a dynamic process.
When a reaction has reached its chemical equilibrium, the constant K value will remain constant unless the temperature changes. If conditions change the concentration in the experiment of any species in the equilibrium reaction, all other species concentrations must also change in order for K to remain constant.
b. Equilibrium constant- When a chemical reaction has reached equilibrium a reaction quotient is given a value symbolized in an equation by the letter K. Normally this value is a ratio expressing the relationship between the concentration of the products to the concentration of the reactants at equilibrium. The two different types of equilibrium reactions are heterogeneous and homogeneous. The reaction will move to the left if the K value is less than one and if the value of K is greater than one the reaction will move to the right.
c. …show more content…
LeChatelier’s principle- This principle is also known as called Chatelier's principle or "The Equilibrium Law” named after Henry Louis Le Châtelier. This principle states that if the equilibrium state of a system is disturbed by an external stress, a shift in the system will take place to counteract the effect of that disturbance to maintain equilibrium. This disruption can be caused by a change in concentration of the reactants or products, a temperature change, or pressure change.
2. List four factors that can affect the position of equilibrium. Of these four factors, which is the only one that can alter the value of the equilibrium constant?
1. Changes in pressure
2. Changes in