4 22. Hydrogen sulfide is a poisonous gas with a characteristic, offensiveodour. It dissociates at 1400°C, with K. equal to 2.4 x 104.2H,S =2H2e) + Sze!4.0 mol of H2S is placed in a 3.0 L container. What is the equilibriumconcentration of Haig) at 1400°C?tion is

2 H2S (g) ==> 2H2(g) + S2 (g) Kc = 2.4 × 10-4

4 22. Hydrogen sulfide is a poisonous gas with a characteristic, offensve odour. It dissociates at 1400°C, with K. equal to 2.4 x 104. 4.0 mol of H2S is placed in a 3.0 L container. What is the equilibrium concentration of Haie) at 1400°C?

4 22. Hydrogen sulfide is a poisonous gas with a characteristic, offensve odour. It dissociates at 1400°C, with K. equal to 2.4 x 104. 4.0 mol of H2S is placed in a 3.0 L container. What is the equilibrium concentration of Haie) at 1400°C?

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

Thoroughly Explain and Answer
A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: 30, (g) = 20, (g) K, = 4. × 10-6 He fills a reaction vessel at this temperature with 9.0 atm of oxygen gas. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of O3, using only the tools Oyes available to you within ALEKS? O no O atm If you said yes, then enter the equilibrium pressure of O, at right. Round your answer to 1 significant digit.
7. Ammonia can be synthesized according to the equation: 1/2 N₂(g) + 3/2 H₂(g) → NH3(g). The equilibrium constant is 1.69 x 10-4 at 673 K and AHO is -106.5 kJ mol-¹. Calculate the equilibrium constant at 773 K.
A 6.00 mol sample of solid A was placed in a sealed 1.00 L container and allowed to decompose into gaseous B and C. The concentration of B steadily increased until it reached 1.40 M, where it remained constant. A(s)↽−−⇀B(g)+C(g) Then, the container volume was doubled and equilibrium was re‑established. How many moles of A remain? Dont
Consider the reaction, 2AB2(g) = A2(g) + 2B2(g), Kc = 0.263 at 25°C. The reaction begins with an unknown concentration of AB2 in the reaction flask. At equilibrium, the concentration of AB2 is found to be 0.00545 M. a) Complete the ICEE table below, b) Write the equilibrium expression and equation for this reaction (pay close attention to coefficients!), c) Calculate the equilibrium concentration of both products, and d) Calculate the initial concentration of AB2. You should confirm that your equilibrium concentrations will give the correct equilibrium constant when plugged into the expression. ICEE table I C E 2 AB₂(g) A₂(g) + 2 B₂(g)
At a certain temperature, 0.760 mol of SO, is placed in a 4.00 L container. 2 SO, (g) = 2 S0,(g) + 0,(g) At equilibrium, 0.170 mol of O, is present. Calculate K.. Ke = M
6. Hydrogen gas is finding more acceptance as an alternative fuel. It is produced along with carbon dioxide by the reaction of carbon monoxide and gaseous water at 915 K. At this temperature, the equilibrium constant (K.) is 1.56. If this reaction is started in a 4.00 L closed system flask with 0.450 mol of CO, 1.25 mol H2O, 1.15 mol CO2, and 3.50 mol H2, calculate the concentrations of all substances in the flask initially and at equilibrium. Put these values in the ICE table below. (Hint: you will need to use the quadratic formula.) CO Н20 CO2 H2 INITIAL CHANGE EQUILIBRIUM 0.1125 0.3125 0.2875 0.875 -X -X +X +x e these values in the table. d. Calculate the reaction quotient, Q. e. Express the direction of equilibrium shift as an algebraic expression. Complete the change row of the table. f. Substitute the algebraic expressions into the equilibrium expression and solve for the equilibrium concentrations. Place these values in the table.
explain