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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Enter your answer in the provided box. The equilibrium constant K, for the equation 2H,(g) + CO(g) =CH;OH(g) is 23 at a certain temperature. If there are 1.81 x 102 moles of H, and 2.31 x 10-3 moles of CH3OH at equilibrium in a 6.75-L flask, what is the concentration of CO? M
Le Chatelier’s Principle. Directions: Predict the directions that happen in the system to achieve equilibrium after having disturbances or changes occur in it. Explain your answer. S8(g) + 12O2(g) ó 8 SO3(g) + 808 kcals What will happen when …… Sulfur trioxide is added? Heat is added? Pressure of oxygen gas is increased?
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 =
12) If 1.34 moles each of Br2 and Cl2 are introduced into an 11.0 liter flask and allowed to come to equilibrium, what should the equilibrium concentrations of Br2, Cl2, and BrCl be? 2 BrCl (g) « Br2 (g) + Cl2 (g)Kc = 0.143
Consider the following equilibrium for which H = -114.44: 4 HCl(g) + O2(g) 2 Cl2(g) + 2 H2O(g) How will each of the following changes affect an equilibrium mixture of the 4 gases in this reaction?(a) O2(g)) is added to the system. The equilibrium will not shift The equilibrium will shift toward product but Keq will not change The equilibrium will shift toward reactant but Keq will not change The equilibrium will shift toward product but Keq will will increase The equilibrium will shift toward reactant but Keq will decrease(b) The reaction mixture is cooled. (c) The volume of the reaction vessel is reduced by 50%.
Determine whether each phrase is true or false 1. For gaseous equilibrium shown, 3A +B → C + 2D, some C is removed from the system. The quantity of D will rise.
using the equilibrium constant expression 2H2(g)+S2(g)---->2H2S(g). Calculate the equilibrium constant if: [H2]=2.1*10-1 M [S2]=1.1*10-6 M [H2S]=7.3*10-1 M
Predict the equilibrium concentration of CO: 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. Co(g) + H:O(g) = CO:(g) + H:(g) 1 2 3 4 NEXT > In a 2.0 L container at 700 K, 0.13 mol CO, 0.56 mol H:O, 1.62 mol CO:, and 0.43 mol H: 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 5 RESET [0.13] [0.56] [1.62] [0.43] [0.065] [0.28] [0.81] [0.22] [0.26] [0.13] [1.62] [0.065) [0.28] 0.10 96 3.1 9.8 ||
For the following equilibrium, Kc = 56 at a given temperature. At equilibrium, [CH4] = 0.2 and [Cl2] = 0.4. What are the equilibrium concentrations of CH3Cl and HCl if they are equal?
Consider the following equilibrium: N₂O4(g) = 2NO2(g) A 1.00 L container is initially filled with 0.200 mol N₂O4At equilibrium, 0.160 mol NO₂are present. What is the equilibrium concentration of N₂O4? 0.120 mol/L 0. 040 mol/L O.0.160 mol/L 0.080 mol/L 0.100 mol/L
Predict the equilibrium concentration of NH in the reaction described below (for which Kc = 1.210 at the reaction temperature) by constructing an ICE table, writing the equilibrium constant expression, and solving for the equilibrium concentration. Complete Parts 1-3 before submitting your answer. = NHSH(s) NH¸(g) + H₂S(g) Using the data from your ICE Table (Part 1), construct the expression for the equilibrium constant, Kc. Each reaction participant must be represented by one tile. Do not combine terms. KC = II = 1.2 × 10-4 RESET [x] [2x] [2x]² [1.2 × 104+x] [1.2 × 104-x] [1.2 × 104 + 2x] [1.2 × 104 -2x] [1.2 × 10+ + x]² [1.2 × 10+ - x]² [1.2 × 10+ + 2x]² [1.2 × 104 -2x]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) 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. [0] [0.050] 0.030 [1.0] [0.201² 1 9.0 x 10-4 Qc = [0]² [0.15]² 1.1 x 104 2 [1.01² [0.40]² [0.20] [0.30]² 3 [0.15] [0.050]² [0.40] 0 ✓ RESET [0.30] 33