H₂S and O₂ react according to the equation below. Predict the equilibrium pressure of SO₂ by constructing an ICE table, writing the equilibrium constant expression expressed in terms of partial pressure, and solving for the equilibrium partial pressure of SO₂. Complete Parts 1-3 before submitting your answer. Initial (atm) Change (atm) Equilibrium (atm) NEXT > A reaction flask was filled 2.00 atm of H₂S and 5.00 atm of O₂ at 200 K and allowed to react. Fill in the ICE table with the appropriate value for each involved species to determine the pressure of all reactants and products. -2x 5.00 + 3x 0 2H,S(g) -3x 2 H₂S(g) + 3 O₂(g) = 2 H₂O(g) + 2 SO₂(g) 5.00-x 2.00 2.00 + x 5.00 - 2x + 5.00 2 30,(g) 2.00 + 2x 5.00 - 3x +X 2.00-x at +2x 2.00 - 2x 2H₂O(g) +3x 2.00 - 3x RESET 5.00 + x 250 (9)

H₂S and O₂ react according to the equation below. Predict the equilibrium pressure of SO₂ by constructing an ICE table, writing the equilibrium constant expression expressed in terms of partial pressure, and solving for the equilibrium partial pressure of SO₂. Complete Parts 1-3 before submitting your answer. Initial (atm) Change (atm) Equilibrium (atm) NEXT > A reaction flask was filled 2.00 atm of H₂S and 5.00 atm of O₂ at 200 K and allowed to react. Fill in the ICE table with the appropriate value for each involved species to determine the pressure of all reactants and products. -2x 5.00 + 3x 0 2H,S(g) -3x 2 H₂S(g) + 3 O₂(g) = 2 H₂O(g) + 2 SO₂(g) 5.00-x 2.00 2.00 + x 5.00 - 2x + 5.00 2 30,(g) 2.00 + 2x 5.00 - 3x +X 2.00-x at +2x 2.00 - 2x 2H₂O(g) +3x 2.00 - 3x RESET 5.00 + x 250 (9)

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 29 of 30 Consider the reaction of N2O 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 NO(g) +3 O₂(g) 4 NO2(g) 1 2 NEXT > A 1.00 L reaction vessel was filled with 0.0560 mol O2 and 0.200 mol N2O and allowed to react at 298 K. At equilibrium, there were 0.0200 mol of NO2 present. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products.. 2N₂O(g) + 302(g) == 4NO2(g) Initial (M) 0.200 -0.0100 0.190 Change (M) 0.0560 -0.0150 0.0410 Equilibrium (M) 0 0.0200 0.0200 RESET 0 0.0560 0.200 -1.00 -0.0560 0.0200 -0.0200 0.0100 -0.0100 -0.0050 0.0050 0.0150 -0.0150 0.210 0.190
Subject: chemistry
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