Let's begin by considering the equilibrium position: Let's consider the formation of ammonia from nitrogen and hydrogen gases in a rigid container. a) Write the balanced chemical equation for this reaction. b) At some temperature the initial reaction mixture contains 4.00M each of hydrogen gas and nitrogen gas and no ammonia gas and in 60 seconds, at equilibrium, the mixture contains 2.50M ammonia gas (plus some hydrogen and nitrogen). Calculate the molarities of nitrogen gas and hydrogen gas at equilibrium.
Let's begin by considering the equilibrium position: Let's consider the formation of ammonia from nitrogen and hydrogen gases in a rigid container. a) Write the balanced chemical equation for this reaction. b) At some temperature the initial reaction mixture contains 4.00M each of hydrogen gas and nitrogen gas and no ammonia gas and in 60 seconds, at equilibrium, the mixture contains 2.50M ammonia gas (plus some hydrogen and nitrogen). Calculate the molarities of nitrogen gas and hydrogen gas at equilibrium.
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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How can we solve these questions on equilibrium?
![General Chemistry II
Part II. Equilibrium
An equilibrium reaction is the reaction that can proceed in BOTH the forwards and backwards
directions at the same time. Chemical equilibrium is the point in a chemical reaction when the
relative concentrations of reactants and products in the mixture stop changing.
Let's consider the following generic equilibrium reaction: Az(g) + 2B(g) 2AB(g). Now
imagine that we add some A2(g) and some B(g) to a container and seal it. As soon as we do that
the reaction will start to proceed in the forwards direction: Az and B will react with one another
to form AB and the concentrations of A2 and B will begin to decrease while the concentration of
AB will begin to increase. However, as soon as some AB forms the reverse reaction will also
begin to occur, but, at this point, at a much slower rate than the forwards reaction. As the process
continues the forward reaction will keep slowing down and the backward reaction will keep
speeding up. The relative concentrations of A2, B, and AB will keep changing until the rate of the
backward reaction becomes equal to the rate of the forward reaction. At this point
concentrations of all reactants and products will stop changing and we say that the process has
reached the equilibrium. This equilibrium is called dynamic. So if the system is at equilibrium, at
any moment, the number of AB molecules that form from of Az and B is equal to the number of
the AB molecules that break to produce of Az and B.
Given any chemical reaction, you should be able to visualize these changes and plot them on a
concentration vs time graph.
Equilibrium constant, K, gives us information about how far in the forwards direction a reaction
will proceed until it reaches equilibrium. K can be calculated using the ratio of the concentrations
of species present at equilibrium, raised to the power of the stoichiometric coefficients. For our
equilibrium reaction, A2(g) + 2B(g) 2AB(g), the equilibrium constant, K = [AB]²/([A₂][B]²).
The numerical value of K is a constant for a given reaction at a fixed temperature, i.e. if we
change the concentrations of chemicals in the initial reaction mixture, when the system arrives
to equilibrium the concentrations [AB]', [A2]', and [B]' may be different from [AB], [A2], and [B],
but the equilibrium constant value will not change (K'=K if T=T).
Let's begin by considering the equilibrium position:
Let's consider the formation of ammonia from nitrogen and hydrogen gases in a rigid container.
a) Write the balanced chemical equation for this reaction.
b) At some temperature the initial reaction mixture contains 4.00M each of hydrogen gas and
nitrogen gas and no ammonia gas and in 60 seconds, at equilibrium, the mixture contains
2.50M ammonia gas (plus some hydrogen and nitrogen). Calculate the molarities of
nitrogen gas and hydrogen gas at equilibrium.
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Transcribed Image Text:General Chemistry II
Part II. Equilibrium
An equilibrium reaction is the reaction that can proceed in BOTH the forwards and backwards
directions at the same time. Chemical equilibrium is the point in a chemical reaction when the
relative concentrations of reactants and products in the mixture stop changing.
Let's consider the following generic equilibrium reaction: Az(g) + 2B(g) 2AB(g). Now
imagine that we add some A2(g) and some B(g) to a container and seal it. As soon as we do that
the reaction will start to proceed in the forwards direction: Az and B will react with one another
to form AB and the concentrations of A2 and B will begin to decrease while the concentration of
AB will begin to increase. However, as soon as some AB forms the reverse reaction will also
begin to occur, but, at this point, at a much slower rate than the forwards reaction. As the process
continues the forward reaction will keep slowing down and the backward reaction will keep
speeding up. The relative concentrations of A2, B, and AB will keep changing until the rate of the
backward reaction becomes equal to the rate of the forward reaction. At this point
concentrations of all reactants and products will stop changing and we say that the process has
reached the equilibrium. This equilibrium is called dynamic. So if the system is at equilibrium, at
any moment, the number of AB molecules that form from of Az and B is equal to the number of
the AB molecules that break to produce of Az and B.
Given any chemical reaction, you should be able to visualize these changes and plot them on a
concentration vs time graph.
Equilibrium constant, K, gives us information about how far in the forwards direction a reaction
will proceed until it reaches equilibrium. K can be calculated using the ratio of the concentrations
of species present at equilibrium, raised to the power of the stoichiometric coefficients. For our
equilibrium reaction, A2(g) + 2B(g) 2AB(g), the equilibrium constant, K = [AB]²/([A₂][B]²).
The numerical value of K is a constant for a given reaction at a fixed temperature, i.e. if we
change the concentrations of chemicals in the initial reaction mixture, when the system arrives
to equilibrium the concentrations [AB]', [A2]', and [B]' may be different from [AB], [A2], and [B],
but the equilibrium constant value will not change (K'=K if T=T).
Let's begin by considering the equilibrium position:
Let's consider the formation of ammonia from nitrogen and hydrogen gases in a rigid container.
a) Write the balanced chemical equation for this reaction.
b) At some temperature the initial reaction mixture contains 4.00M each of hydrogen gas and
nitrogen gas and no ammonia gas and in 60 seconds, at equilibrium, the mixture contains
2.50M ammonia gas (plus some hydrogen and nitrogen). Calculate the molarities of
nitrogen gas and hydrogen gas at equilibrium.
5
Transcribed Image Text:General Chemistry II
c) Now use the axes below to draw a graph that shows the change in concentration vs time for
each of the 3 species in this reaction if you start with 4.00M each of hydrogen gas and
nitrogen gas only and at equilibrium you have 2.50M ammonia gas.
Before you draw the graph make sure that EVERYONE in your group is comfortable with
predicting the changes that are going to occur. Which concentrations increase and which
concentrations decrease? Take a moment to discuss these questions in your group and when
you are sure you all agree draw your graph in the space provided. Remember to show one
line for EACH species present in the mixture.
d) Now calculate the value of the equilibrium constant for the process
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