Bromine and water react to form hydrogen bromide and oxygen, like this: 2 Br (9) + 2H₂O(g)-4HBr(g) + O₂(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of bromine, water, hydrogen bromide, and oxygen has the following composition compound concentration at equilibrium Br₂ 0.26M 1AM 0.93M 1.9M H₂O HBc 0₂ Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. OP

Bromine and water react to form hydrogen bromide and oxygen, like this: 2 Br (9) + 2H₂O(g)-4HBr(g) + O₂(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of bromine, water, hydrogen bromide, and oxygen has the following composition compound concentration at equilibrium Br₂ 0.26M 1AM 0.93M 1.9M H₂O HBc 0₂ Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. OP

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 38QAP: Nitrogen dioxide can decompose to nitrogen oxide and oxygen. 2NO2(g)2NO(g)+O2(g) K is 0.87 at a...

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Because carbonic acid undergoes a second ionization, the student in Exercise 12.39 is concerned that the hydrogen ion concentration she calculated is not correct. She looks up the equilibrium constant for the reaction HCO,-(aq) «=* H+(aq) + COf'(aq) Upon finding that the equilibrium constant for this reaction is 4.8 X 10“H, she decides that her answer in Exercise 12.39 is correct. Explain her reasoning. A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H,CO,(aq) 5=6 H+(aq) + HCO,'(aq) K = 4.4 X 10'7She starts with 0.1000 A1 carbonic acid. W hat are the concentrations of all species at equilibrium?
. Many sugars undergo a process called mutarotation, in which the sugar molecules interconvert between two isomeric forms, finally reaching an equilibrium between them. This is true for the simple sugar glucose, C6H12O6, which exists in solution in isomeric forms called alpha-glucose and beta-glucose. If a solution of glucose at a certain temperature is analyzed, and it is found that the concentration of alpha-glucose is twice the concentration of beta-glucose, what is the value of K for the inter-conversion reaction?
Consider the following equilibrium constants. Describe how you would expect the equilibrium concentrations of reactants and products to compare with each other larger than, smaller than, etc. for each case. a. K=2.1106 b. K=0.15 c. K=1.2108 d. K=0.00036
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.
. 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.
Methanol, a common laboratory solvent, poses a threat of blindness or death if consumed in sufficient amounts. Once in the body, the substance is oxidized to produce formaldehyde (embalming fluid) and eventually formic acid. Both of these substances are also toxic in varying levels. The equilibrium between methanol and formaldehyde can be described as follows: CH3OH(aq)H2CO(aq)+H2(aq) Assuming the value of K for this reaction is 3.7 1010, what are the equilibrium concentrations of each species if you start with a 1.24 M solution of methanol? What will happen to the concentration of methanol as the formaldehyde is further converted to formic acid?
Equilibrium exists between butane and isobutane when [butane] = 0.020 M and [isobutane] = 0.050 M. An additional 0.0200 mol/L of isobutane is added to the mixture. What are the concentrations of butane and isobutane after equilibrium has again been attained?
What is the difference between homogeneous equilibrium and heterogeneous equilibrium?
Chemical Equilibrium II Magnesium hydroxide. Mg(OH)2, is a white, partially soluble solid that is used in many antacids. The chemical equation for the dissolving of Mg(OH)2(s) in water is Mg(OH)2(s)Mg2+(aq)+2OH(aq) a Describe a simple experimental procedure that you could use to study this solubility equilibrium. In your experiment, how would you determine when the solution process has attained equilibrium? b Write the equilibrium-constant expression for this dissolving of magnesium hydroxide. c Suppose equilibrium has been established in a container of magnesium hydroxide in water, and you decide to add more solid Mg(OH)2. What would you expect to observe? What effect will this addition of Mg(OH)2 have on the concentrations of Mg2+(aq) and OH(aq)? d Say you haw prepared an equilibrium solution of Mg(OH)2 by adding pure solid Mg(OH)2 to water. If you know the concentration of OH(aq), can you determine the concentration of Mg2+(aq)? If not, what information do you need that will allow you to determine the answer? e You slowly add OH from another source (say, NaOH) to an equilibrium mixture of Mg(OH)2 and water. How do you expect the concentration of the Mg2+(aq) to change? What might you be able to observe happening to the Mg(OH)2(s) as you add the OH? f Next you remove some, but not all, of the Mg(OH)2(s) from the mixture. How will this affect the concentrations of the Mg2+(aq) and OH(aq)? g If someone hands you a container of Mg(OH)2(aq) and there is no solid Mg(OH)2 present, is this solution at equilibrium? If it is not at equilibrium, what could you add to or remove from the container that would give an equilibrium system? h Consider an individual OH(aq) ion in an Mg(OH)2 solution at equilibrium. If you could follow this ion over a long period of time, would you expect it always to remain as an OH(aq) ion, or could it change in some way?
For the reaction 2HI(g)H2(g)+I2(g) carried out at some fixed temperature, the equilibrium constant is 2.0. a Which of the following pictures correctly depicts the reaction mixture at equilibrium? b For the pictures that represent nonequilibrium situations, describe which way the reaction will shift to attain 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?
Many sugars undergo a process called mutarotation, in which the sugar molecules interconvert between two isomeric forms, finally reaching an equilibrium between them. This is true for the simple sugar glucose, C6H12O6, which exists in solution in isomeric forms called alpha-glucose and beta-glucose. If a solution of glucose at a certain temperature is analyzed, and it is found that the concentration of alpha-glucose is twice the concentration of beta-glucose, what is the value of K for the interconversion reaction?