Iron(III) oxide and hydrogen react to form iron and water, like this:Fe,0;(s)+3 H,(g)→2FE(s)+3H,O(9)At a certain temperature, a chemist finds that a 5.1 L reaction vessel containing a mixture of iron(III) oxide, hydrogen, iron, and water at equilibrium has thefollowing composition:compound amountdbFe,O34.36 gH,4.35 gFe3.23 gH,02.73 gCalculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits.ExplanationCheck2022 McGraw H LLC. A Rights Reserved Terms of Use Pvacy Center AccessibilDEP Type here to searchJUP.AltalexaENADLED

Kc is the ratio of product of concentration of products raised to their stoichiometric coefficient…

Iron(III) oxide and hydrogen react to form iron and water, like this: Fe,0,(s)+3 H,(9)-2Fe(s)+3 H,O(9) At a certain temperature, a chemist finds that a 5.1 L reaction vessel containing a mixture of iron(II) oxide, hydrogen, iron, and water at equilibrium has the following composition: compound amount Fe,O3 4.36 g H, 4.35 g Fe 3.23 g H,0 2.73g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits.

Iron(III) oxide and hydrogen react to form iron and water, like this: Fe,0,(s)+3 H,(9)-2Fe(s)+3 H,O(9) At a certain temperature, a chemist finds that a 5.1 L reaction vessel containing a mixture of iron(II) oxide, hydrogen, iron, and water at equilibrium has the following composition: compound amount Fe,O3 4.36 g H, 4.35 g Fe 3.23 g H,0 2.73g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits.

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.103PAE: 12.103 Methanol, CH3OH, can be produced by the reaction of CO with H2, with the liberation of heat....

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A 4.72-g sample of methanol (CH3OH) was placed in an otherwise empty 1.00-L flask and heated to 250.C to vaporize the methanol. Over time, the methanol vapor decomposed by the following reaction: CH3OH(g)CO(g)+2H2(g) After the system has reached equilibrium, a tiny hole is drilled in the side of the flask allowing gaseous compounds to effuse out of the flask. Measurements of the effusing gas show that it contains 33.0 times as much H2(g) as CH3OH(g). Calculate K for this reaction at 250.C.
Show that the complete chemical equation, the total ionic equation, and the net ionic equation for the reaction represented by the equation KI(aq)+I2(aq)KI3(aq) give the same expression for the reaction quotient. KI3 is composed of the ions K+ and I3-.
A gaseous material XY(g) dissociates to some extent to produce X(g) and Y(g): XY(g)X(g)+Y(g) A 2.00-g sample of XY (molar mass = 165 g/mol) is placed in a container with a movable piston at 25C. The pressure is held constant at 0.967 atm. As XY begins to dissociate, the piston moves until 35.0 mole percent of the original XY has dissociated and then remains at a constant position. Assuming ideal behavior, calculate the density of the gas in the container after the piston has stopped moving, and determine the value of K for this reaction of 25C.
12.103 Methanol, CH3OH, can be produced by the reaction of CO with H2, with the liberation of heat. All species in the reaction are gaseous. What effect will each of the following have on the equilibrium concentration of CO? (a) Pressure is increased, (b) volume of the reaction container is decreased, (c) heat is added, (d) the concentration of CO is increased, (e) some methanol is removed from the container, and (f) H2 is added.
Suppose a reaction has the equilibrium constant K = 1.3 108. What does the magnitude of this constant tell you about the relative concentrations of products and reactants that will be present once equilibrium is reached? Is this reaction likely to be a good source of the products?
5.2. What is the difference between a static equilibrium and a dynamic equilibrium? Give examples difference from the examples in the text. What is similar for the two types of equilibria?
. What does it mean to say that a state of chemical or physical equilibrium is dynamic?
12.101 An engineer working on a design to extract petroleum from a deep thermal reservoir wishes to capture toxic hydrogen sulfide gases present by reaction with aqueous iron(II) nitrate to form solid iron(II) sulfide. (a) Write the chemical equation for this process, assuming that it reaches equilibrium. (b) What is the equilibrium constant expression for this system? (c) How can the process be manipulated so that it does not reach equilibrium, allowing the continuous removal of hydrogen sulfide?
In a 3.0-L vessel, the following equilibrium partial pressures are measured: N2, 190 torr; H2, 317 torr; NH3, 1.00103 torr. N2(g)+3H2(g)2NH3(g) (a) How will the partial pressures of H2, N2, and NH3 change if H2 is removed from the system? Will they increase, decrease, or remain the same? (b) Hydrogen is removed from the vessel until the partial pressure of nitrogen, at equilibrium, is 250 torr. Calculate the partial pressures of the other substances under the new conditions.
For the system SO3(g)SO2(g)+12 O2(g)at 1000 K, K=0.45. Sulfur trioxide, originally at 1.00 atm pressure, partially dissociates to SO2 and O2 at 1000 K. What is its partial pressure 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