Predict the equilibrium concentration of O2 in the reaction described below (forwhich Kc = 4.10 x 10 at a high temperature) by constructing an equilibriumexpression for Qc, constructing an ICE table, writing an equilibrium expressionfor Kc, and solving for the equilibrium concentration. Complete Parts 1-4 beforesubmitting your answer.N2(g) + O2(g) 2 NO(g)<PREV3NEXT>Based on the initial concentrations and your value of Qc (Part 1), fill in the ICE table with theappropriate value for each involved species to determine the partial pressures of all reactants andproducts. Where applicable, use the x variables to represent any unknown change inconcentration.Initial (M)Change (M)Equilibrium (M)N₂(g)O2(g)142 NO(g)RESET00.200.15+x-x+2x-2x0.20 + x0.20-x0.20 + 2x0.20-2x0.15 + x0.15-x0.15+2x0.15-2x22AA80F2F3$54#3E888F4F5%905^6MacBook Air---<<DIIF7F8&87RTYUF9* ∞(890-CJF103DFGHJKLCVBNMVיוP{V Predict the equilibrium concentration of O2 in the reaction described below (forwhich Kc = 4.10 x 10 at a high temperature) by constructing an equilibriumexpression for Qc, constructing an ICE table, writing an equilibrium expressionfor Kc, and solving for the equilibrium concentration. Complete Parts 1-4 beforesubmitting your answer.N2(g) + O2(g) 2 NO(g)234NEXT >In a 1.0 L container at high temperature, 0.20 mol N2 and 0.15 mol O2 are allowed to react. Setup the expression for Qc. Each reaction participant must be represented by one tile. Do notcombine 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]²0330.0309.0 × 10-41.1 x 104F280F3MAR22

The given reaction is:N2(g) + O2(g) 2NO(g)Kc = Volume of container = 1.0 LMoles of N2 = 0.20…

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 =

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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Question

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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A
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Step 1: Given data

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Step 2: Calculating the molarity of N2 and O2

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Step 3: Calculating the Qc for the reaction

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Step 4: Constructing the ICE table and writing the equilibrium constant expression

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4 PH3(g) 6 H,(g) + P4(g) the equilibrium concentrations were found to be [PH,] = 0.250 M, [H,] = 0.570 M, and [P] = 0.750 M. %3D What is the equilibrium constant for this reaction? Ke =
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