Predict the equilibrium concentration of CO, in the reaction described below byconstructing an equilibrium expression for Qc, constructing an ICE table, writingan equilibrium expression for Kc, and solving for the equilibrium concentration.Complete Parts 1-4 before submitting your answer.CO(g) + H₂O(g) = CO₂(g) + H₂(g)PREVThe value of Kc is 5.1 at a temperature of 700 K. Based on your ICE table (Part 2), set up theequilibrium expression for Kc in order to determine concentrations of all species. Each reactionparticipant must be represented by one tile. Do not combine terms.[x][0.065 + x][0.28 + x]²[2x][0.065 -x][0.81 -x]²Kc[x]²=[0.28 + x][0.22 -x]²[2x]²[0.81 -x]3[0.13 -x][0.22 -x]5.1[0.56 + x][0.56 + x]²4[1.62 + x]NEXT[0.065 + x]²>RESET[0.43 -x][0.065 -x]²

Answer: Value of equilibrium constant KC is always equal to the ratio of molar concentration of…

Predict the equilibrium concentration of CO, in the reaction described below by constructing an equilibrium expression for ac, 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) + H₂O(g) = CO₂(g) + H₂(g) < PREV 1 2 3 The value of Kc is 5.1 at a temperature of 700 K. 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. Kc = = 5.1 4 NEXT >

Predict the equilibrium concentration of CO, in the reaction described below by constructing an equilibrium expression for ac, 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) + H₂O(g) = CO₂(g) + H₂(g) < PREV 1 2 3 The value of Kc is 5.1 at a temperature of 700 K. 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. Kc = = 5.1 4 NEXT >

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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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 ||
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
True/False. Explain your answer in one sentence or less. In an equilibrium process, the concentrations of products and of reactants are equal. The value of the equilibrium constant for a given reaction depends on the initial concentrations of reactants. Large value for equilibrium constant K means the reaction will be less complete at the equilibrium point. The concentration of a pure solid is left out of an equilibrium constant expression but a pure liquid is included.
Consider the equilibrium system described by the chemical reaction below. Determine the concentration of O, at equilibrium by writing the equilibrium constant expression and solving it. Complete Parts 1-2 before submitting your answer. = 2 H₂O(g) 2 H2(g) + O̟₂(g) 1 2 NEXT At this temperature, the Kc = 2.4 × 103 and the equilibrium concentrations of H2O and H2 are 0.11 M and 0.019 M, respectively. If [x] represents the equilibrium concentration of O2, set up the equilibrium expression for Kc to solve for the concentration. Each reaction participant must be represented by one tile. Do not combine terms. Кс = 2' = 2.4 × 103 > RESET [0.11] [0.019] 2[0.11] 2[0.019] [0.11]² [0.019]² [x] [x]² [2x] [2x]²
K = 1.3 \times 10-10 for the reaction HC6H50(aq) = H+(aq) + C6H50-(aq). In which direction is the equilibrium favored? Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a Forward b Reverse c Appreciable quantities of all species are present at equilibrium d No direction is favored e There is not enough information to determine the direction
true or false
ST5B.2 - The reaction A2(g) + B2(g) --> 2AB(g) has an equilibrium constant Kc = 1.22. What is the equilibrium concentration [in mol/L] of B2(g) if the reaction is run at a constant volume of one liter with initial reactant amounts of 0.96 mol A2lg) and 2.50 mol B2(g) with no product present? You can solve this algebraically or graphically - but be sure to zoom in enough if you use a graph so that you get enough precision in your answer. Don't just solve for "x" - make sure you get the equilibrium concentration of B2(g). Type your answer...
Write the equilibrium-constant expression for the reaction shown in terms of [SO2], [CO2], [CS2], and [O2]. 2SO2(g)+CO2(g)↽−−⇀CS2(g)+3O2(g) ?c, which is sometimes symbolized as ? or ?eq, denotes that the equilibrium constant is expressed using molar concentrations. For this question, ?c means the same thing as ? and ?eq.