25- 2 H2S(g) → 2 H2(g) + S2(g) When heated, hydrogen sulfide gas decomposes according to the equation above. A 3.40 g sample of H2S(g) is introduced into an evacuated rigid 1.25 L container. The sealed container is heated to 483 K, and 3.72x10-2 mol of S2(g) is present at equilibrium. (a) Write the expression for the equilibrium constant, Ke, for the decomposition reaction represented above. (b) Calculate the equilibrium concentration, in mol·L-l, of the following gases in the container at 483 K. (i) H2(g) (ii) H2S(g) (c) Calculate the value of the equilibrium constant, Ke, for the decomposition reaction at 483 K.

25- 2 H2S(g) → 2 H2(g) + S2(g) When heated, hydrogen sulfide gas decomposes according to the equation above. A 3.40 g sample of H2S(g) is introduced into an evacuated rigid 1.25 L container. The sealed container is heated to 483 K, and 3.72x10-2 mol of S2(g) is present at equilibrium. (a) Write the expression for the equilibrium constant, Ke, for the decomposition reaction represented above. (b) Calculate the equilibrium concentration, in mol·L-l, of the following gases in the container at 483 K. (i) H2(g) (ii) H2S(g) (c) Calculate the value of the equilibrium constant, Ke, for the decomposition reaction at 483 K.

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

Related questions

Q: The equilibrium system 2SO:(g)+ O2(g) = 2S03(g) is an exothermic reaction. Which change will result…

A: Lechatelier's principle :- It states that , when a system at equilibrium is subjected to a change in…

Q: Consider the following reaction that takes place in a closed 2.0L container: N2(g) + 202(g) 2 NO2(g)…

A: The objective of the question is to calculate the equilibrium concentrations of nitrogen and oxygen.

Q: Consider the reaction for the decomposition of hydrogen disulfide (H2S). 2 H2S (g) → 2 H2 (g ) +…

Q: What is the equilibrium concentration of IBr? Express your answer in moles per liter to three…

Q: A chem gineer is studying the following reaction: 2 NO(g) + 2H₂(g) → N₂(g) + 2H₂O(g) At the…

A: Answer:When , reaction mixture is at equilibrium.When , reaction mixture is not at equilibrium and…

Q: • In an analysis of inter halogen reactivity, 0.500 mol ICI (iodine chloride) was placed in a 5.00 L…

Q: At a certain temperature, the equilibrium constant, Kc, for the reaction is 4.00. An equilibrium…

A: Given information: Kc = 4.00 V = 1.00 L 4.60 moles of NH3(g) 3.00 moles of Cl2(g) 5.90 moles of…

Q: For the reaction sO2g) + NO2)= SO3(g) + NOg), the equilibrium constant Ke is 18.0 at 1200°C. At…

A: Given that: equilibrium constant, Kc = 18.0 volume = 10.0 L moles of SO2 = 1.0 moles of NO2 = 2.0…

Q: 20. Which of the following statements most correctly describe(s) any chemical equilibrium? (A) All…

A: We need to tell which among these options is correct at equilibrium. (A) All reactions cease (B) The…

Q: Consider the following reaction at equilibrium, What will happen if the volume decreased at constant…

A: Le Chatelier's principle: When a change is applied to a system at equilibrium, the equilibrium will…

Q: Consider the following reaction: 2CH(g) C₂H₂(g) + 3H₂(g) The reaction of CH4 is carried out at some…

A: We will first construct the ICE table. It helps us to find the equilibrium concentration of the…

Q: A mixture of nitrogen and chlorine gases was kept at a certain temperature in a 5.0 L reaction…

A: Number of moles of N2 at equilibrium = 0.0070 molNumber of moles of Cl2 at equilibrium = 0.0022…

Q: Consider the following equilibrium: 2NOCl(g) 2NO(g) + Cl2(g) with K = 1.6 × 10–5. In an experiment,…

A: Consider the following equilibrium:2NOCl(g) 2NO(g) + Cl2(g) with K = 1.6 × 10–5. In an experiment,…

Q: Consider the formation of chloromethane CH4 (g) + Cl2 (g) ------ CH3Cl(g) + HCl (g) If Kc= 4.5 x…

Q: Consider the reaction and associated equilibrium constant: aA(g) bB (g), K = 2.2 Find the…

Q: Titanium(IV) chloride decomposes to form titanium and chlorine, like this: TICL,(1)→ Ti(s)+2 Cl,(9)…

A: Given: At equilibrium, Mass of TiCl4 =2.59 g Mass of Ti =2.97 g Mass of Cl2 =1.45 g Volume of…

Q: The teeth are protected by a hard enamel layer, which is composed of a mineral called hydroxyaptite,…

A: Answer: This question is based on Le-chatalier's principle according to which on changing any…

Q: 18. À mixture of Û.i0Û moi of H2 and 0.132 moi of CO is piaced in a reaction container and allowed…

A: Given equilibrium is 2H2(g) + CO(g) ⇌ CH3OH(g) Initial moles of H2 = 0.100 mol Initial moles of…

Q: A 0.10 mole of A and 0.10 mole of B are put in 1.00L vessel. Calculate the equilibrium concentration…

A: The given reaction is A (g) + B (g) ↔ 2C (g) A(g) + B(g) ↔ 2C(g)0.10…

Q: The reaction quotient for a system is 3.9 x 103. If the equilibrium constant for the system is 2x…

A: Given : reaction quotient = 3.9 X 103 And equilibrium constant = 2 X 10-4

Q: rogen, compound amount Fe,03 4.85 g H2 2.01 g Fe 3.53 g 1.33 g Calculate the value of the…

Q: Consider the following equilibrium reaction: 2 NO (g) + Cl2 (g) 2 NOCI (g) After the system had come…

Q: 25- 2 H2S(g) →2 H2(g) + S2(g) When heated, hydrogen sulfide gas decomposes according to the equation…

Q: The reaction below was allowed to react at 375 degrees Celcius until it formed an equilibrium. At…

A: In this question we want to determine the value of Kc Equilibrium constant. You can see details…

Q: Q3. At 298 K, F3SSF(g) decomposes partially to SF2(g). At equilibrium, the partial pressure of…

A: Given that, Equilibrium partial pressure of SF2=1.1×10-4 atm Partial pressure of F3SSF = 0.0484 atm…

Q: Consider the following equilibrium reaction: 2NO (g) + Cl2 (g) 2 NOCl (g) K=12 At…

Question

100%

25- 2 H2S(g) → 2 H2(g) + S2(g)
When heated, hydrogen sulfide gas decomposes according to the equation above. A 3.40 g
sample of H2S(g) is introduced into an evacuated rigid 1.25 L container. The sealed container
is heated to 483 K, and 3.72x10-2 mol of S2(g) is present at equilibrium.
(a) Write the expression for the equilibrium constant, Ke, for the decomposition reaction
represented above.
(b) Calculate the equilibrium concentration, in mol·L-1, of the following gases in the container
at 483 K.
(i) H2(g)
(i) Н2S(g)
(c) Calculate the value of the equilibrium constant, Ko, for the decomposition reaction at 483
K.
(d) Calculate the partial pressure of S2(3) in the container at equilibrium at 483 K.
(e) For the reaction H2(g) + S2(2) –→ H2S(g) at 483 K, calculate the value of the equilibrium
constant, K.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

A sample of HI was placed in a container and the following reaction was allowed to come equilibrium. H₂(g) + 1₂(g) = 2 HI(g) The equilibrium concentrations were found to be [HI] = 3.88 M and [H₂] = [1₂] = 0.556. Calculate the equilibrium const Kc, for the reaction. Note Kc is often called K.
Iron and water react to form iron(III) oxide and hydrogen, like this: 2 Fe(s)+3 H,0(g)→ Fe,O3(s)+3 H,(g) At a certain temperature, a chemist finds that a 9.2 L reaction vessel containing a mixture of iron, water, iron(III) oxide, and hydrogen at equilibrium has the following composition: compound amount ol. Fe 4.85 g Ar H,O 1.44 g Fe,O3 2.98 g H2 2.51 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K_ = 0 Ox10 Explanation Check © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility
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
A student ran the following reaction in the laboratory at 303 K:2NO(g) + Br2(g) 2NOBr(g)When she introduced NO(g) and Br2(g) into a 1.00 L evacuated container, so that the initial partial pressure of NO was 1.15 atm and the initial partial pressure of Br2 was 0.408 atm, she found that the equilibrium partial pressure of Br2 was 0.138 atm.Calculate the equilibrium constant, Kp, she obtained for this reaction. Kp =
The equilibrium reaction of 2 moles of SO2e) plus 1 mole of O2e) produces 1 mole of SO3@)- What is the equilibrium constant expression for this reaction. 2(g)
Consider the equilibrium between SbCl5, SbCl3 and Cl₂. SbCl5(g) SbCl3(g) + Cl₂(g) K = 2.46x10-² at 530 K The reaction is allowed to reach equilibrium in a 7.30-L flask. At equilibrium, [SbCl5] = 0.430 M, [SbCl3] = 0.103 M and [Cl₂] = 0.103 M. (a) The equilibrium mixture is transferred to a 14.6-L flask. In which direction will the reaction proceed to reach equilibrium? (b) Calculate the new equilibrium concentrations that result when the equilibrium mixture is transferred to a 14.6-L flask. [SbCl5] = [SbCl3] = [Cl₂] |||| ΣΣΣ
O KINETICS AND EQUILIBRIUM Using the general properties of equilibrium constants At a certain temperature, the equilibrium constant K for the following reaction is 380.: NO,(8) + CO(3) = NO(g) + CO,(3) Use this information to complete the following table. Suppose a 16. L reaction vessel is filled with 1.4 mol of NO, and 1.4 mol of CO. What can you say about the composition of the mixture in the vessel at equilibrium? There will be very little No, and CO. O There will be very little NO and CO,. O Neither of the above is true. What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. K = ] NO(9)+CO,(9) NO,(9)+CO(g) What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. K = ] %3D 3 NO,(9)+3CO(g) 3 NO(g)+3CO,(9) 1L Explanation Check III
Consider the following equilibrium process at 686 degrees celsius. CO2 (g) + H2 (g) ---> CO (g) + H2O (g) The equilibrium concentrations of the reaction species are [CO]= 0.0510 M, [H2]= 0.0410 M, [CO2]= 0.0840 M, and [H2O]= 0.0390 M. a) alculate Kc for the reaction at 686 degrees celcius. Round your answer to 3 significant figures. b) If we add CO2 to increase its concentration to 0.420 M, what will the concentration of all the gases be when equilibrium is reestablished? [CO2]= M. Round your answer to 3 significant figures. c) [H2] = M. Round your answer to 2 significant figures. d) [CO]= M. Round your answer to 2 significant figures. e) [H2O]= M. Round your answer to 2 significatnt figures
Explain the effect of each of the following stresses on the position of the following equilibrium: 3 NO(g) 2 N¿O(g) + NO2(g) The reaction as written is exothermic. (a) N¿O(g) is added to the equilibrium mixture without change of volume or temperature. (b) The volume of the equilibrium mixture is reduced at constant temperature. (c) The equilibrium mixture is cooled. (d) Gaseous argon (which does not react) is added to the equilibrium mixture while both the total gas pressure and the temperature are kept constant. (e) Gaseous argon is added to the equilibrium mixture without changing the volume.