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 =

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%.

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 ||

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

During an experiment, O.257 mol of H2 and 0.257 mol of I2 were placed into a 1.28 liter vessel where the reaction H2(g) + 12(g) 2 2HI(g) came to equilibrium. For this reaction, Kc = 49.5 at the temperature of the experiment. What were the equilibrium concentrations of H2, 12, and HI? [H2] = M %3D [12] = M [HI] = i M

MOving to anotrie question will save this response. Question 7 A state of dynamic equilibrium, Ag2CO3(s) +→ 2Ag*(aq) + CO32(aqg), exists in solutida. Which direction will the equilibrium shift if Ca(NO3)2(aq) is added to the system? O To the left. O To the right. O It will not shift left or right. A Moving to another question will save this response. MacBook Pro 80 888 FS F6 F7 FA esc F2 %23 2$ 8. 2 3 4. Q K A D 5

Consider the following equilibrium. N2(s) + O2(g) 2 NO(g) At 2300 K, the equilibrium constant K - 1.7 x 10. Suppose that 0.015 mol NO(g), 0.16 mol N, (9), and 0.16 mol O, (9) are placed into a 10.0 L flask and heated to 2300 K. (a) Is the system at equilibrium? If the system is not at equilibrium, in which direction must the reaction proceed to reach equilibrium? The system is at equilibrium. OThe system is not at equilibrium. The reaction must proceed to the left. The system is not at equilibrium. The reaction must proceed to the right (b) Calculate the equilibrium concentrations of all three substances. (Enter unrounded answers.) [02 - [NO M