At a certain temperature, the K, for the decomposition of H,S is 0.840. H,S(g) =H,(g) + S(g) Initially, only H,S is present at a pressure of 0.117 atm in a closed container. What is the total pressure in the container at equilibrium?

At a certain temperature, the K, for the decomposition of H,S is 0.840. H,S(g) =H,(g) + S(g) Initially, only H,S is present at a pressure of 0.117 atm in a closed container. What is the total pressure in the container at equilibrium?

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter12: Gaseous Chemical Equilibrium

Section: Chapter Questions

Problem 81QAP: For the system SO3(g)SO2(g)+12 O2(g)at 1000 K, K=0.45. Sulfur trioxide, originally at 1.00 atm...

See similar textbooks

Related questions

Q: Consider the following reaction: COCI,(g) CO(g) + Cl,(g) If 1.79×10 moles of COCI,(g), 0.470 moles…

A: Equilibrium constant of any reaction can be obtained by dividing the multiplication of…

Q: For the exothermic reaction PCl3(g)+Cl2(g)⇌PCl5(g) Kp= 0.200 at a certain temperature. A flask is…

Q: The equilibrium constant Kp for the following reaction is found to be 4.31 X 10 N2g) + 3H2(g)…

A: Given Kp = 4.31×10-⁴ Initial pressure of Nitrogen = 0.932 atm Initial pressure of hydrogen =…

Q: A sample of N204(g) is placed in an empty cylinder at a certain temperature. It is allowed to…

Q: Nitric oxide, NO, is formed in automobile exhaust by the reaction of N, and 0, in air. N: (g) + 0:…

Q: The equilibrium constant K, for the reaction H2(g) + Br,(g) - 2HBr(g) is 2.18 x 10 at 730°C.…

Q: Nitrogen dioxide decomposes according to the reaction 2 NO2(g) ⇌ 2 NO(g) + O2(g) where Kp =…

A: Nitrogen dioxide decomposes into nitrogen oxide and oxygen, the balanced chemical equation is given…

Q: For the reaction 2 A (g) + B (g) = C(g) + D(s) AH = - 33.0 kJ 1. Initially in a 5.0 L flask at 75°C,…

A: 1. Since, solids do not exert any pressure, so D will not have any pressure. Thus, ICE table for the…

Q: 2HI(g) H2(g) + 12(g) Kp = 0.0184 %3D A reaction vessel is filled with HI to a pressure of O.0240…

Q: Hydrogen iodide can decompose into hydrogen and iodine gases. 2 HI(g) --> H2(g) + I2(g)…

Q: Consider the following equilibrium:N2O4(g)⇌ 2 NO2(g)You may assume that ΔH° and ΔS° do not varywith…

A: The vaporization of liquid N2O4 is,

Q: r. N2(g) + 3H2(g) ⇌ 2NH3(g) (a) How will the partial pressures of H2, N2, and NH3 change if H2 is…

Q: At a certain temperature, the K for the decompositon of H2S is 0.891. H,S(g) = H2(g) + S(g)…

A: All things are provide in hand written solution.

Q: . Iodine, 12, is a blue-black solid, but it easily vaporizes to give a violet vapor. At high…

A: chemical reaction is I2 →2I occurs at high temperature

Q: nsider the following reaction: 2SO2(g) + O2(g) ⇌ 2 SO3(g) KP = 0.14 at 625°C If a reaction vessel…

A: For any reversible reaction at any moment, reaction quotient (Q) helps us to find the direction of…

Q: I need these conditions with a pressure of NOCl tend to rise or fall. Calculate the minimum pressure…

A: Part 1:The pressure of NOCl will fall because the initial pressure of NO, one of the products is…

Q: 1. Methane, CH. reacts with hydrogen sulfide, H2S to yield hydrogen gas, Hz and carbon disulfide,…

Q: At 900.0 K, the equilibrium constant, Kp, for the following reaction is 0.527. 2S0212) + O2lg)…

Q: The equilibrium constant K, for the oxidation of sulfur dioxide into sulfur trioxide is 5.6 x 104 at…

Q: At 2000 K the partial pressures of an equilibrium mixture of H2S, H2, and S are 0.0353,0.0371, and…

A: The balanced reaction is given as H2S(g) <====> H2(g) + S(g) According to law of chemical…

Q: At a certain temperature, the K, for the decomposition of H,S is 0.819 atm. H, S(g) = H, (g) + S(g)…

A: Our equation, of course, is H2S → H2 + S Using an ICE box (or chart): I…

Q: At a certain temperature, the K, for the decomposition of H,S is 0.734 atm. H,S(g) = H,(g) + S(g)…

A: The equilibrium reaction given is, => H2S (g) --------> H2 (g) + S (g)…

Q: A sample of ammonium chloride was heated in a closed container.NH4 Cl(s) ⇌ NH3(g) + HCl(g)At…

Q: Det a partial equilibrium. Sulfur dioxide and oxygen react to form sulfur trioxide during one of the…

Q: Nitrogen dioxide decomposes according to the reaction 2 NO2(g) ⇌ 2 NO(g) + O2(g) where Kp = 4.48…

Q: Consider the following reaction: PCI{(g) PC13(g)+ Cl2(g) If 1.00×10-3 moles of PCI5, 0.302 moles of…

A: Equilibrium constants mainly get measured in concentration terms as well as pressure terms. The…

Q: At a certain temperature, the K, for the decomposition of H,S is 0.800. H, S(g) = H,(g) + S(g)…

A: The given equilibrium is H2S(g) ⇌ H2(g) + S(g) Equilibrium constant , Kp = 0.800 Initial pressure of…

Q: Use the References to access important values if needed for this question. Consider the following…

Q: Consider the following reaction: COCI2(g)CO(g) + Cl2(g) If 1.39x102 moles of COCL. 0.302 moles of…

Q: A sample of ammonium chloride was heated in a closed container. NH4Cl(s)⇌NH3(g)+HCl(g) At…

A: A strong acid is an acid that dissociates to make protons available for reaction. Acid mainly…

Q: For the following reaction H₂(g) + I₂(g) ⇌ 2HI(g) ∆H° = -10.64 kJ/mol and ∆S° = 21.48 J/mol･K. A…

A: This can be solved using the equations of ∆G°. The steps are given as,

Q: Be sure to answer all parts. The equilibrium constant (K) for the formation of nitrosyl chloride, an…

A: Given-> 2NO(g) + Cl2(g) ---> 2NOCl(g) Kc= 5×106 Mole of NO = 9.30 × 10-2 Mole of Cl2 = 1.60 ×…

Q: The equilibrium constant KP for the decomposition of phosphorus pentachloride tophosphorus…

A: The equation can be written as: PPCl5 = 0.973 atm PPCl3= 0.548 atm Kp = 1.05

Q: The reaction PCl3 + Cl2 <=>PCl5 has Kp =0.0870 at 300 °C. A flask is charged with 0.50 atm…

A: Assuming that y atm of PCl5 is reacting in backward direction Hence the pressure of PCl3 and Cl2…

Q: At 800 K, hydrogen iodide can decompose into hydrogen and iodine gases. 2HI (g) ---> <----- I2 (g)…

A: Equilibrium constant,K = 0.0169 Pressure of HI = 0.213 atm Temperature = 800 K At Equilibrium,…

Q: At 500 K, the Kp of the reaction PCl5 (g) = PCl3 (g) + Cl2 (g) is 0.497. In a chamber at 500 K, we…

A: Kp is the constant of equilibrium determined from the partial pressures of the equation of reaction.…

Q: A mixture of 7.19 mol N, and 25.93 g NO is heated in a closed vessel to 2000 °C. After heating, the…

Q: Nitric oxide, NO, is formed in an automobile exhaust by the reaction of N2 and O2 in the air. N2 (g)…

A: Given,Volume = 2L,Concentration =1\2 = 0.5.ICE table:Initial concentrationCC0At…

Q: At 500 K, the Kp of the reaction PCI5 (g) = PCI3 (g) + Cl2 (g) is 0.497. In a chamber at 500 K, we…

A: Recall the given reaction PCl5g→PCl3 g+ Cl2gWrite expression of reaction…

Q: For the following reaction, Kₚ=6.5X10⁴ at 308 K 2NO(g)+Cl₂(g)⇌2NOCl(g) At equilibrium, P(NO)=0.35…

A: Kp is the equilibrium constant calculated from the partial pressures of a reaction equation. It is…

Q: In a 3.0-L vessel, the following equilibrium partial pressures are measured: N2, 190 torr; H2, 317…

A: According to Le Chatlier's principle, when the chemical system in equilibrium is disturbed by…

Q: Hydrogen iodide gas is formed from its elements with a value for Kp = 25.5 at a certain temperature:…

A: Calculate partial pressure of HI at equilibrium....

Q: Sulfur oxychloride, SO2 Cl2, decomposes to sulfur dioxide and chlorine gases. SO, Cl (g)SO2(9)+ Cl2…

A: From the expression of equilibrium constant we can determine K using partial pressure values.

Q: lfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid…

Q: A student ran the following reaction in the laboratory at 591 K: COCl2(g) CO(g) + Cl2(g) When…

Q: Consider the following reaction: COCl2(g) CO(g) + Cl2(g) If 7.22×10-3 moles of COCl2, 0.276 moles…

A: The equilibrium reaction is: COCl2(g) → CO(g) + Cl2(g) ∆n = 2-1 = 1 Given that: 7.22×10-3 moles of…

Q: Liquid N2O3 is dark blue at low temperatures, but the color fades and becomes greenish at higher…

Question

100%

At a certain temperature, the K, for the decomposition of H,S is 0.840.
H,S(g) =H,(g) + S(g)
Initially, only H,S is present at a pressure of 0.117 atm in a closed container. What is the total pressure in the container
at equilibrium?

Expert Solution

This question has been solved!

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

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step 3

VIEW

Step by step

Solved in 3 steps with 2 images

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

Consider the reaction 2HI(g)H2(g)+I2(g)At 500C a flask initially has all three gases, each at a partial pressure of 0.200 atm. When equilibrium is established, the partial pressure of HI is determined to be 0.48 atm. What is G for the reaction at 500C?
Molecular bromine, Br2, dissociates at elevated temperatures into bromine atoms, Br. Br2(g)2Br(g) A 3.000-L flask initially contains pure molecular bromine. The temperature is then raised to 1600 K. If the total pressure of this equilibrium mixture at this elevated temperature is 1.000 atm, what are the total moles of gas in the container? A spectroscopic analysis of this mixture showed that it contained 1.395 g of Br atoms. What is the partial pressure of Br? What is Kp for the dissociation of molecular bromine to bromine atoms?
. Explain why the development of a vapor pressure above a liquid in a closed container represents an equilibrium. What are the opposing processes? How do we recognize when the system has reached a state of equilibrium?
. Ammonia. a very important industrial chemical. is produced by the direct combination of the following elements under carefully controlled conditions: N2(g)+3H2(g)2NH3(g)Suppose. in an experiment, that the reaction mixture is analyzed after equilibrium is reached, and it is found, at a particular temperature. that [NH3]=0.25M,[H2]=3.4103M, and [N2]=5.3105M. Calculate the value of K at this temperature.
Sulfur oxychloride, SO2Cl2, decomposes to sulfur dioxide and chlorine gases. SO2Cl2(g)SO2(g)+Cl2(g) At a certain temperature, the equilibrium partial pressures of SO2, Cl2, and SO2Cl2 are 1.88 atm, 0.84 atm, and 0.27 atm, respectively. (a) What is K at that temperature? (b) Enough Cl2 condenses to reduce its partial pressure to 0.68 atm. What are the partial pressures of all gases when equilibrium is reestablished?
For the system PCl5(g)PCl3(g)+Cl2(g)K is 26 at 300C. In a 1.0-L flask at 300C, a gaseous mixture consists of all three gases with the following partial pressures: PPCl5=0.026atm,PPCl3=0.65atmPPCl2=0.33atm (a) Is the system at equilibrium? Explain. (b) If the system is not at equilibrium, in which direction will the system move to reach equilibrium?
A student studies the equilibrium I2(g)2I(g)at a high temperature. She finds that the total pressure at equilibrium is 40% greater than it was originally, when only I2 was present. What is K for this reaction at that temperature?
Consider the equilibrium H2(g)+S(s)H2S(g)When this system is at equilibrium at 25C in a 2.00-L container, 0.120 mol of H2, 0.034 mol of H2S, and 0.4000 mol of S are present. When the temperature is increased to 35C, the partial pressure of H2 increases to 1.56 atm. (a) What is K for the reaction at 25C? (b) What is K for the reaction at 35C?
Benzaldehyde, a flavoring agent, is obtained by the dehydrogenation of benzyl alcohol. C6H5CH2OH(g)C6H5CHO(g)+H2(g)K for the reaction at 250C is 0.56. If 1.50 g of benzyl alcohol is placed in a 2.0-L flask and heated to 250C, (a) what is the partial pressure of the benzaldehyde when equilibrium is established? (b) how many grams of benzyl alcohol remain at equilibrium?
A sample of gaseous nitrosyl bromide (NOBr) was placed in a container tiued with a frictionless, massless piston, where it decomposed at 25C according to the following equation: 2NOBr(g)2NO(g)+Br2(g) The initial density of the system was recorded as 4.495 g/L. After equilibrium was reached, the density was noted to be 4.086 g/L. a. Determine the value of the equilibrium constant K for the reaction. b. If Ar(g) is added to the system at equilibrium at constant temperature, what will happen to the equilibrium position? What happens to the value of K? Explain each answer
Nitrogen dioxide can decompose to nitrogen oxide and oxygen. 2NO2(g)2NO(g)+O2(g) K is 0.87 at a certain temperature. A 5.0-L flask at equilibrium is determined to have a total pressure of 1.25 atm and oxygen to have a partial pressure of 0.515 atm. Calculate PNO and PNO2 at equilibrium.
A mixture of 0.0565 mol phosphorus pentachloride, PCl5, and 0.0800 mol helium gas, He, was placed in a 1.000-L flask and heated to 250.0C. The phosphorus pentachloride decomposes at this temperature to give phosphorus trichloride, PCl3, and chlorine gas, Cl2. The helium gas is inert. PCl5(g)PCl3(g)+Cl2(g) What is the partial pressure of helium in this equilibrium mixture at 250.0C? At equilibrium, the total pressure is found to be 6.505 atm. What is Kc for the dissociation of PCl5?