H₂S and O₂ react according to the equation below. Predict the equilibriumpressure of SO, by constructing an ICE table, writing the equilibrium constantexpression expressed in terms of partial pressure, and solving for the equilibriumpartial pressure of SO₂. Complete Parts 1-3 before submitting your answer.2 H₂S(g) + 3 O₂(g) — 2 H₂O(g) + 2 SO₂(g)>A reaction flask was filled 2.00 atm of H₂S and 5.00 atm of O₂ at 200 K and allowed to react. Fillin the ICE table with the appropriate value for each involved species to determine the pressure ofall reactants and products.Initial (atm)Change (atm)Equilibrium (atm)-2x5.00 + 3x0-3x5.00 - x12H₂S(g) +2.002.00 + x5.00 - 2x5.0030₂(g)2.00 + 2x25.00 - 3x+x2.00 -- X2H₂O(g)+2x32.00 - 2x+3x2.00 - 3xNEXT2SO₂(g)RESET5.00 + x

Answered: Image /qna-images/answer/5252325a-aa5e-43fc-ad19-7fce4df098c3.jpg

H₂S and O₂ react according to the equation below. Predict the equilibrium pressure of SO, 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. 2 H₂S(g) + 3 O₂(g) = 2 H₂O(g) + 2 SO₂(g) 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. Initial (atm) Change (atm) Equilibrium (atm) 1 2 2H₂S(g) + 30₂(g) 3 2H₂O(g) + 2SO₂(g)

H₂S and O₂ react according to the equation below. Predict the equilibrium pressure of SO, 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. 2 H₂S(g) + 3 O₂(g) = 2 H₂O(g) + 2 SO₂(g) 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. Initial (atm) Change (atm) Equilibrium (atm) 1 2 2H₂S(g) + 30₂(g) 3 2H₂O(g) + 2SO₂(g)

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...

See similar textbooks

Similar questions

Consider the following system at equilibrium: Fe2 O3 (s) + 3H2 (g) = 2 Fe (s) +3H2O (g) ΔΗ -98.7 kJ | If the volume was increased, what changes would have to occur to reestablish equilibrium? The concentration of H2 would increase. The concentration of H2 would decrease. The concentration of H20 would decrease. The concentration of H20 would increase. No change
(please type answer fast).
If someone takes a breath and the lungs expand from 4.5 L to 5.8 L in volume, and the initial pressure was 758 mm Hg, what is the pressure inside the lungs (in mmHg) before any additional air is pulled in?
None
Chemistry
(please type answer no write by hend)
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
E8hstant from a heterogeneous. Iron(III) oxide and hydrogen react to form iron and water, Ilike this: Fe,0;(s)+3 H,(9)→2 Fe(s)+3H,O(g) At a certain temperature, a chemist finds that a 4.0 L reaction vessel containing a mixture of iron(III) oxide, hydrogen, iron, and water at equilibrium has following composition: compound amount Fe,O3 4.85 g H2 2.01 g Fe 3.53 g H,O 1.33 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K = | Explanation Check 2022 McGraw H LLC A Rights Reservedt Tem of Use acy Conter Accesbity Type here to search 99 C FIO Pr Sc 24 4. & he 7. 8. %3D Y U H K Alt Alt Chl
General Chemistry 4th Edition McQuarrie Rock Gallogly An equilibrium mixture contains 0.500 mol of each of the products (carbon dioxide and hydrogen gas) and 0.200 mol of each of the reactants (carbon monoxide and water vapor) in a 1.00 L container. CO(g) + H₂O(g) = CO₂(g) + H₂(g) How many moles of carbon dioxide would have to be added at constant temperature and volume to increase the amount of carbon monoxide to 0.300 mol once equilibrium has been reestablished? moles of CO₂: University Science Books presented by Macmillan Learning »))) R. mol
Answer all with small explanation or leave for someone else to answer .
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
A student ran the following reaction in the laboratory at 600 K: CO(g) + Cl₂(g) —COCI₂(g) When he introduced CO(g) and Cl₂(g) into a 1.00 L evacuated container, so that the initial partial pressure of CO was 2.09 atm and the initial partial pressure of Cl₂ was 1.22 atm, he found that the equilibrium partial pressure of Cl₂ was 0.405 atm. Calculate the equilibrium constant, Kp, she obtained for this reaction. Кр