Predict the equilibrium concentration of O2 in the reaction described below (for which Kc = 4.10 x 10 at a high temperature) 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) 2 3 NEXT > 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. Qc =
Predict the equilibrium concentration of O2 in the reaction described below (for which Kc = 4.10 x 10 at a high temperature) 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) 2 3 NEXT > 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. Qc =
Introduction to General, Organic and Biochemistry
11th Edition
ISBN:9781285869759
Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Chapter7: Reaction Rates And Chemical Equilibrium
Section: Chapter Questions
Problem 7.64P: 7-64 As we shall see in Chapter 20, there are two forms of glucose, designated alpha and betawhich...
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Transcribed Image Text:Predict the equilibrium concentration of O2 in the reaction described below (for
which Kc = 4.10 x 10 at a high temperature) 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)
<
PREV
3
NEXT
>
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.
Initial (M)
Change (M)
Equilibrium (M)
N₂(g)
O2(g)
14
2 NO(g)
RESET
0
0.20
0.15
+x
-x
+2x
-2x
0.20 + x
0.20-x
0.20 + 2x
0.20-2x
0.15 + x
0.15-x
0.15+2x
0.15-2x
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![Predict the equilibrium concentration of O2 in the reaction described below (for
which Kc = 4.10 x 10 at a high temperature) 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)
2
3
4
NEXT >
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.
Qc =
=
RESET
[0]
[1.0]
[0]²
[1.02
[0.20]
[0.15]
[0.40]
[0.30]
[0.050]
[0.20]²
[0.15]²
[0.40]²
[0.30]²
[0.050]²
0
33
0.030
9.0 × 10-4
1.1 x 104
F2
80
F3
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22
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Transcribed Image Text:Predict the equilibrium concentration of O2 in the reaction described below (for
which Kc = 4.10 x 10 at a high temperature) 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)
2
3
4
NEXT >
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.
Qc =
=
RESET
[0]
[1.0]
[0]²
[1.02
[0.20]
[0.15]
[0.40]
[0.30]
[0.050]
[0.20]²
[0.15]²
[0.40]²
[0.30]²
[0.050]²
0
33
0.030
9.0 × 10-4
1.1 x 104
F2
80
F3
MAR
22
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Expert Solution
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Step 1: Given data
VIEWStep 2: Calculating the molarity of N2 and O2
VIEWStep 3: Calculating the Qc for the reaction
VIEWStep 4: Constructing the ICE table and writing the equilibrium constant expression
VIEWStep 5: Calculating the value of x
VIEWStep 6: Calculating the concentration at equilibrium
VIEWSolution
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