Predict the equilibrium concentration of H₂O in the reaction described below (for which Kc = 1.79 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. 2 H₂S(g) + SO₂(g) = 3 S(s) + 2 H₂O(g) Initial (M) Change (M) Equilibrium (M) -3.x 0.025 + 2x The reaction mixture initially contains 0.050 M H₂S and 0.050 M SO₂. Fill in the ICE table with the appropriate value for each involved species to determine the concentrations of all reactants and products. 0 1 2 H₂S(g) + 0.050 + x 0.025 + 3x 0.050 0.050 + 2x 0.025 - x +X 2 SO₂(g) 0.050 + 3x 0.025 - 2x +2x 0.050- x 0.025 -3x = 3 3 S(s) +3x 0.050 - 2x -X + 0.050-3x NEXT > 2 H₂O(g) RESET -2x 0.025 + x

Predict the equilibrium concentration of H₂O in the reaction described below (for which Kc = 1.79 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. 2 H₂S(g) + SO₂(g) = 3 S(s) + 2 H₂O(g) Initial (M) Change (M) Equilibrium (M) -3.x 0.025 + 2x The reaction mixture initially contains 0.050 M H₂S and 0.050 M SO₂. Fill in the ICE table with the appropriate value for each involved species to determine the concentrations of all reactants and products. 0 1 2 H₂S(g) + 0.050 + x 0.025 + 3x 0.050 0.050 + 2x 0.025 - x +X 2 SO₂(g) 0.050 + 3x 0.025 - 2x +2x 0.050- x 0.025 -3x = 3 3 S(s) +3x 0.050 - 2x -X + 0.050-3x NEXT > 2 H₂O(g) RESET -2x 0.025 + x

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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For the equilibrium Br₂(g) + Cl₂ (g) = 2BrCl(g) at 400 K, K₂= 7.0. Part A If 0.54 mol of Br₂ and 1.23 mol of Cl₂ are introduced into a 3.0-L container at 400 K, what will be the equilibrium concentration of Br₂? Express your answer to two significant figures and include the appropriate units. Value Submit Part B HÅ Submit Value ▾ Part C If 0.54 mol of Br₂ and 1.23 mol of Cl₂ are introduced into a 3.0-L container at 400 K, what will be the equilibrium concentration of Cl₂? Express your answer to two significant figures and include the appropriate units. μA Submit 1 Request Answer Value C Units μÃ Units Request Answer If 0.54 mol of Br₂ and 1.23 mol of Cl₂ are introduced into a 3.0-L container at 400 K, what will be the equilibrium concentration of BrCl? Express your answer to two significant figures and include the appropriate units. =)? Units Request Answer ? B) ?
Initial (M) Change (M) Equilibrium (M) -0.00875 0.0209 Consider the reaction of SO2 and O₂ described by the chemical reaction below. Determine the equilibrium constant for this reaction by constructing an ICE table, writing the equilibrium constant expression, and solving it. Complete Parts 1-2 before submitting your answer. 2 SO2(g) + O₂(g) = 2 SO3(g) NEXT > A 2.00 L reaction vessel was filled 0.0432 mol SO₂ and 0.0296 mol O₂2 at 900 K and allowed to react. At equilibrium, the concentration of SO3 was found to be 0.0175 M. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. 0 0.00875 re or pull up for additional resources 2.00 1 2SO2(g) 0.0216 2.00 0.0432 0.0148 + 0.0296 2 0.0041 O₂(g) 0.0175 0.0129 11 -0.0175 0.0061 2SO3(g) RESET 0.0350 0.0257
Predict the equilibrium concentration of H₂O in the reaction described below (for which Kc = 1.79 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. 2 H₂S(g) + SO₂(g) 3 S(s) + 2 H₂O(g) Initial (M) Change (M) Equilibrium (M) -3.x 0.025 + 2x The reaction mixture initially contains 0.050 M H₂S and 0.050 M SO₂. Fill in the ICE table with the appropriate value for each involved species to determine the concentrations of all reactants and products. 0 1 2 H₂S(g) + 0.050 + x 0.025 + 3x 0.050 0.050 + 2x 0.025 - x +X 2 SO₂(g) 0.050 + 3x 0.025 - 2x +2x 0.050- x 0.025 -3x 3 3 S(s) +3.x 0.050 - 2x -X + 0.050-3x NEXT > 2 H₂O(g) RESET -2x 0.025 + x
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Enter your answer in the provided box. Use the equilibrium constant expression, and equilibrium constant to det concentration of H₂S if: [H₂S]² [S₂][H₂]² Keq=1.1 x 107 [H₂] = 1.0 × 10-3 M [S₂] = 5.0 × 10 5 M [H₂S] = 0.55 X Keq = 2 H₂(g) + S₂(g) → 2 H₂S(g)
A mixture of 0.10 mole NO, 0.050 mole H₂, and 0.10 mole H₂O is placed in a 2.0 L vessel. The following equilibrium is established: + 2 H₂ (g) = N2(g) + 2 H₂O (g) 2 NO At equilibrium [NO] = 0.030 M. The initial concentration of N₂ was not mentioned so you must assume [N₂] = 0. Calculate the equilibrium concentrations (in M) of: More Information X H₂ (g) XN₂ (g) X H₂O (g) Question Answer Your answer -.020 is Your answer .035 is in Your answer .170 is i Tol: 0.0001 Tol: 0.001 Tol: 0.001
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Suppose a 250. mL flask is filled with 1.0 mol of CO, 0.60 mol of NO and 1.3 mol of CO2. The following reaction becomes possible: NO,(g) + CO (g) = NO(g)+CO,(g) The equilibrium constant K for this reaction is 3.67 at the temperature of the flask. Calculate the equilibrium molarity of NO,. Round your answer to two decimal places. ? Check Explanation
Consider the equilibrium system described by the chemical reaction below. For this reaction, Kc = 2.4 x 103 at a particular temperature. If the equilibrium concentrations of H,0 and H, are 0.11 M and 0.019 M, respectively, determine the concentration of O, at equilibrium.. 2 2 H,O(g) = 2 H,(g) + 0,(g) 2 NEXT > If [x] represents the equilibrium concentration of O, set up the equilibrium expression for Kc to solve for the concentration. Do not combine or simplify terms.. 2' K. = = 2.4 x 103 5 RESET [О.11] [0.019] 2[0.11] 2[0.019] [0.11]? [0.019]? [x] [x]? [2x] [2x]?
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