Predict the equilibrium concentration of O₂ in the reaction described below by constructing an equilibrium expression for Qc, constructing an ICE table, writing an equilibrium expression for Kc, and solving for the equilibrium concentration. Complete Parts 1-4 before submitting your answer. N₂(g) + O₂(g) = 2 NO(g) 3 In a 1.0 L container at high temperature, 0.20 mol N₂ and 0.15 mol O₂ are allowed to react. Set up the expression for Qc. Each reaction participant must be represented by one tile. Do not combine terms. Once the expression is constructed, solve for Qc to determine the direction of the reaction. 1 2 4 Predict the equilibrium concentration of O₂ in the reaction described below by constructing an equilibrium expression for Qc, constructing an ICE table, writing an equilibrium expression for Kc, and solving for the equilibrium concentration. Complete Parts 1-4 before submitting your answer. N₂(g) + O₂(g) = 2 NO(g) 1 3 Based on the initial concentrations and your value of Qc (Part 1), fill in the ICE table with the appropriate value for each involved species to determine the partial pressures of all reactants and products. Where applicable, use the x variables to represent any unknown change in concentration. N₂(g) + O₂(g) = 2 NO(g) 2 4
Predict the equilibrium concentration of O₂ in the reaction described below by constructing an equilibrium expression for Qc, constructing an ICE table, writing an equilibrium expression for Kc, and solving for the equilibrium concentration. Complete Parts 1-4 before submitting your answer. N₂(g) + O₂(g) = 2 NO(g) 3 In a 1.0 L container at high temperature, 0.20 mol N₂ and 0.15 mol O₂ are allowed to react. Set up the expression for Qc. Each reaction participant must be represented by one tile. Do not combine terms. Once the expression is constructed, solve for Qc to determine the direction of the reaction. 1 2 4 Predict the equilibrium concentration of O₂ in the reaction described below by constructing an equilibrium expression for Qc, constructing an ICE table, writing an equilibrium expression for Kc, and solving for the equilibrium concentration. Complete Parts 1-4 before submitting your answer. N₂(g) + O₂(g) = 2 NO(g) 1 3 Based on the initial concentrations and your value of Qc (Part 1), fill in the ICE table with the appropriate value for each involved species to determine the partial pressures of all reactants and products. Where applicable, use the x variables to represent any unknown change in concentration. N₂(g) + O₂(g) = 2 NO(g) 2 4
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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this is a 4 part problem.
![Question 35 of 40
Predict the equilibrium concentration of O₂
in the reaction described below by
constructing an equilibrium expression for
Qc, constructing an ICE table, writing an
equilibrium expression for Kc, and solving
for the equilibrium concentration. Complete
Parts 1-4 before submitting your answer.
N₂(g) + O₂(g) = 2 NO(g)
Kc =
1
3
The value of Kc is 4.10 x 10-4 at a high
temperature. Based on your ICE table (Part
2), set up the equilibrium expression for Kc
in order to determine concentrations of all
species. Each reaction participant must be
represented by one tile. Do not combine
terms.
2
Submit
[x]
[2x]
[0.20 + x]
[0.20 -x]
[0.15 + x]
[0.15 -x]
[0.20 + x]²
[0.20 -x]²
Tap here or pull up for additional resources
[x]²
[0.20 + 2x]
[0.15 + 2x]
[0.20 + 2x]²
4
= 4.10 x 10-4
>
RESET
[2x]²
[0.20 - 2x]
[0.15 - 2x]
[0.20 - 2x]²
Question 35 of 40
Predict the equilibrium concentration of O₂
in the reaction described below by
constructing an equilibrium expression for
Qc, constructing an ICE table, writing an
equilibrium expression for Kc, and solving
for the equilibrium concentration. Complete
Parts 1-4 before submitting your answer.
N₂(g) + O₂(g) 2 NO(g)
=
3
1
0
0.20
2
Based on the information from your ICE
Table (Part 2) and the Kc expression (Part
3), solve for the the equilibrium
concentration of O₂.
[0₂]eq =
0.0017
0.0034
M
6.1 x 10-6
0.15
Submit
4
Tap here or pull up for additional resources
RESET
0.0035
0.0069](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc7cfbf0b-4345-4268-a259-634bcd51c9b5%2F54b3c31d-7408-47b3-93e0-df9a08d31da1%2Fccl2j6r_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Question 35 of 40
Predict the equilibrium concentration of O₂
in the reaction described below by
constructing an equilibrium expression for
Qc, constructing an ICE table, writing an
equilibrium expression for Kc, and solving
for the equilibrium concentration. Complete
Parts 1-4 before submitting your answer.
N₂(g) + O₂(g) = 2 NO(g)
Kc =
1
3
The value of Kc is 4.10 x 10-4 at a high
temperature. Based on your ICE table (Part
2), set up the equilibrium expression for Kc
in order to determine concentrations of all
species. Each reaction participant must be
represented by one tile. Do not combine
terms.
2
Submit
[x]
[2x]
[0.20 + x]
[0.20 -x]
[0.15 + x]
[0.15 -x]
[0.20 + x]²
[0.20 -x]²
Tap here or pull up for additional resources
[x]²
[0.20 + 2x]
[0.15 + 2x]
[0.20 + 2x]²
4
= 4.10 x 10-4
>
RESET
[2x]²
[0.20 - 2x]
[0.15 - 2x]
[0.20 - 2x]²
Question 35 of 40
Predict the equilibrium concentration of O₂
in the reaction described below by
constructing an equilibrium expression for
Qc, constructing an ICE table, writing an
equilibrium expression for Kc, and solving
for the equilibrium concentration. Complete
Parts 1-4 before submitting your answer.
N₂(g) + O₂(g) 2 NO(g)
=
3
1
0
0.20
2
Based on the information from your ICE
Table (Part 2) and the Kc expression (Part
3), solve for the the equilibrium
concentration of O₂.
[0₂]eq =
0.0017
0.0034
M
6.1 x 10-6
0.15
Submit
4
Tap here or pull up for additional resources
RESET
0.0035
0.0069
![Question 35 of 40
Predict the equilibrium concentration of O₂
in the reaction described below by
constructing an equilibrium expression for
Qc, constructing an ICE table, writing an
equilibrium expression for Kc, and solving
for the equilibrium concentration. Complete
Parts 1-4 before submitting your answer.
N₂(g) + O₂(g) = 2 NO(g)
Qc =
1
3
In a 1.0 L container at high temperature,
0.20 mol N₂ and 0.15 mol O₂ are allowed to
react. Set up the expression for Qc. Each
reaction participant must be represented
by one tile. Do not combine terms.
Once the expression is constructed, solve
for Qc to determine the direction of the
reaction.
2
[1.0]
[0.15]
[0.20]²
[0]
[0]²
[0.20]
[0.40]
[0.050]
[0.15]²
Tap here or pull up for additional resources
Submit
4
>
RESET
[1.0]²
[0.30]
[0.40]²
Predict the equilibrium concentration of O₂
in the reaction described below by
constructing an equilibrium expression for
Qc, constructing an ICE table, writing an
equilibrium expression for Kc, and solving
for the equilibrium concentration. Complete
Parts 1-4 before submitting your answer.
N₂(g) + O₂(g) 2 NO(g)
=
Initial (M)
1
3
Based on the initial concentrations and your
value of Qc (Part 1), fill in the ICE table with
the appropriate value for each involved
species to determine the partial pressures
of all reactants and products. Where
applicable, use the x variables to represent
any unknown change in concentration.
N₂(g) + O₂(g) = 2 NO(g)
Change (M)
Question 35 of 40
Equilibrium (M)
+x
0
2
-X
0.20
+2x
Submit
020+x
020
020 +2
Tap here or pull up for additional resources
4
RESET
0.15
-2x
020-2x](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc7cfbf0b-4345-4268-a259-634bcd51c9b5%2F54b3c31d-7408-47b3-93e0-df9a08d31da1%2Fis3xjvb_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Question 35 of 40
Predict the equilibrium concentration of O₂
in the reaction described below by
constructing an equilibrium expression for
Qc, constructing an ICE table, writing an
equilibrium expression for Kc, and solving
for the equilibrium concentration. Complete
Parts 1-4 before submitting your answer.
N₂(g) + O₂(g) = 2 NO(g)
Qc =
1
3
In a 1.0 L container at high temperature,
0.20 mol N₂ and 0.15 mol O₂ are allowed to
react. Set up the expression for Qc. Each
reaction participant must be represented
by one tile. Do not combine terms.
Once the expression is constructed, solve
for Qc to determine the direction of the
reaction.
2
[1.0]
[0.15]
[0.20]²
[0]
[0]²
[0.20]
[0.40]
[0.050]
[0.15]²
Tap here or pull up for additional resources
Submit
4
>
RESET
[1.0]²
[0.30]
[0.40]²
Predict the equilibrium concentration of O₂
in the reaction described below by
constructing an equilibrium expression for
Qc, constructing an ICE table, writing an
equilibrium expression for Kc, and solving
for the equilibrium concentration. Complete
Parts 1-4 before submitting your answer.
N₂(g) + O₂(g) 2 NO(g)
=
Initial (M)
1
3
Based on the initial concentrations and your
value of Qc (Part 1), fill in the ICE table with
the appropriate value for each involved
species to determine the partial pressures
of all reactants and products. Where
applicable, use the x variables to represent
any unknown change in concentration.
N₂(g) + O₂(g) = 2 NO(g)
Change (M)
Question 35 of 40
Equilibrium (M)
+x
0
2
-X
0.20
+2x
Submit
020+x
020
020 +2
Tap here or pull up for additional resources
4
RESET
0.15
-2x
020-2x
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