Learning Goal: Understand the form and meaning of the equilibrium constant expression. Chemical reactions are usually not one-way trips from reactant to product. In fact, most chemical reactions are reversible to at least some extent. In other words, products formed by the forward reaction may react with each other to regenerate the reactants. When reactants are mixed, they will begin to react at a forward reaction rate particular to that chemical reaction. As reactants are depleted and products are formed, however, the rate of the forward reaction begins to slow, and the rate of the reverse reaction begins to increase. Eventually, the forward and reverse reaction rates will be identical. The products of the reaction are being formed at the same rate as they are being converted back to reactant, and there is no overall change in the concentrations of the reactants or the products. At this point, chemical reactions are said to be at equilibrium. Keep in mind that this is not the same as saying that the reaction has "stopped." Equilibrium is dynamic, meaning that it is a balance of continuous forward and reverse reactions. To indicate this dynamic nature of equilibrium, chemical equations of reactions with measurable reverse reaction rate are written using a double headed arrow: aA+bB=cC+dD For ideal gases and ideal solutions, the extent to which a particular chemical reaction proceeds to products is given by the equilibrium equation: K [C][D] [A][B] where K is the eqiulibrium constant and the right-hand side of the equation is known as the equilibrium constant expression. Part A. What is the proper form of the equilibrium constant expression for the equation; N2(g) + O2(g) 2NO(g) ▸ View Available Hint(s) OK [NO] [N2][02] OK = [NO] [N2][02] OK = [N2][02] [NO]2 OK = 2[NO] N2][02] Submit
Learning Goal: Understand the form and meaning of the equilibrium constant expression. Chemical reactions are usually not one-way trips from reactant to product. In fact, most chemical reactions are reversible to at least some extent. In other words, products formed by the forward reaction may react with each other to regenerate the reactants. When reactants are mixed, they will begin to react at a forward reaction rate particular to that chemical reaction. As reactants are depleted and products are formed, however, the rate of the forward reaction begins to slow, and the rate of the reverse reaction begins to increase. Eventually, the forward and reverse reaction rates will be identical. The products of the reaction are being formed at the same rate as they are being converted back to reactant, and there is no overall change in the concentrations of the reactants or the products. At this point, chemical reactions are said to be at equilibrium. Keep in mind that this is not the same as saying that the reaction has "stopped." Equilibrium is dynamic, meaning that it is a balance of continuous forward and reverse reactions. To indicate this dynamic nature of equilibrium, chemical equations of reactions with measurable reverse reaction rate are written using a double headed arrow: aA+bB=cC+dD For ideal gases and ideal solutions, the extent to which a particular chemical reaction proceeds to products is given by the equilibrium equation: K [C][D] [A][B] where K is the eqiulibrium constant and the right-hand side of the equation is known as the equilibrium constant expression. Part A. What is the proper form of the equilibrium constant expression for the equation; N2(g) + O2(g) 2NO(g) ▸ View Available Hint(s) OK [NO] [N2][02] OK = [NO] [N2][02] OK = [N2][02] [NO]2 OK = 2[NO] N2][02] Submit
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![Learning Goal:
Understand the form and meaning of the equilibrium constant expression.
Chemical reactions are usually not one-way trips from reactant to product. In fact, most chemical reactions are reversible to at least some extent. In other words, products formed by the forward reaction may react with each
other to regenerate the reactants. When reactants are mixed, they will begin to react at a forward reaction rate particular to that chemical reaction. As reactants are depleted and products are formed, however, the rate of the
forward reaction begins to slow, and the rate of the reverse reaction begins to increase. Eventually, the forward and reverse reaction rates will be identical. The products of the reaction are being formed at the same rate as
they are being converted back to reactant, and there is no overall change in the concentrations of the reactants or the products. At this point, chemical reactions are said to be at equilibrium.
Keep in mind that this is not the same as saying that the reaction has "stopped." Equilibrium is dynamic, meaning that it is a balance of continuous forward and reverse reactions. To indicate this dynamic nature of equilibrium,
chemical equations of reactions with measurable reverse reaction rate are written using a double headed arrow:
aA+bB=cC+dD
For ideal gases and ideal solutions, the extent to which a particular chemical reaction proceeds to products is given by the equilibrium equation:
K
[C][D]
[A][B]
where K is the eqiulibrium constant and the right-hand side of the equation is known as the equilibrium constant expression.
Part A.
What is the proper form of the equilibrium constant expression for the equation;
N2(g) + O2(g) 2NO(g)
▸ View Available Hint(s)
OK
[NO]
[N2][02]
OK =
[NO]
[N2][02]
OK =
[N2][02]
[NO]2
OK =
2[NO]
N2][02]
Submit](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F18339013-6253-441b-924b-1414d5a6f8bc%2Fc6140aef-f4fd-48bd-b3a8-6034840bf101%2F7e4wza_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Learning Goal:
Understand the form and meaning of the equilibrium constant expression.
Chemical reactions are usually not one-way trips from reactant to product. In fact, most chemical reactions are reversible to at least some extent. In other words, products formed by the forward reaction may react with each
other to regenerate the reactants. When reactants are mixed, they will begin to react at a forward reaction rate particular to that chemical reaction. As reactants are depleted and products are formed, however, the rate of the
forward reaction begins to slow, and the rate of the reverse reaction begins to increase. Eventually, the forward and reverse reaction rates will be identical. The products of the reaction are being formed at the same rate as
they are being converted back to reactant, and there is no overall change in the concentrations of the reactants or the products. At this point, chemical reactions are said to be at equilibrium.
Keep in mind that this is not the same as saying that the reaction has "stopped." Equilibrium is dynamic, meaning that it is a balance of continuous forward and reverse reactions. To indicate this dynamic nature of equilibrium,
chemical equations of reactions with measurable reverse reaction rate are written using a double headed arrow:
aA+bB=cC+dD
For ideal gases and ideal solutions, the extent to which a particular chemical reaction proceeds to products is given by the equilibrium equation:
K
[C][D]
[A][B]
where K is the eqiulibrium constant and the right-hand side of the equation is known as the equilibrium constant expression.
Part A.
What is the proper form of the equilibrium constant expression for the equation;
N2(g) + O2(g) 2NO(g)
▸ View Available Hint(s)
OK
[NO]
[N2][02]
OK =
[NO]
[N2][02]
OK =
[N2][02]
[NO]2
OK =
2[NO]
N2][02]
Submit
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