Iron(III) oxide and hydrogen react to form iron and water, like this:Fe,O3(s)+3 H,(g)-2 Fe(s)+3 H,0(9)At a certain temperature, a chemist finds that a 2.7 L reaction vessel containing a mixture of iron(III) oxide, hydrogen, iron,and water at equilibrium has the following composition:compound amountFe,O33.66 gH24.09 gFe4.46 gH2O1.82 gCalculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits.ExplanationCheckO 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privacy I Accessibility29MacBook AirD00吕口F3F10D00 F4F5F7F8F223&45789ERTY| K LLL

Equilibrium constant is the ratio of the concentration of products to the concentration of reactants…

Iron(III) oxide and hydrogen react to form iron and water, like this: Fe,O3(s)+3 H,(g)-2 Fe(s)+3 H,0(9) At a certain temperature, a chemist finds that a 2.7 L reaction vessel containing a mixture of iron(III) oxide, hydrogen, iron, and water at equilibrium has the following composition: compound amount Fe,O3 3.66 g H2 4.09 g Fe 4.46 g H20 1.82 g 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,O3(s)+3 H,(g)-2 Fe(s)+3 H,0(9) At a certain temperature, a chemist finds that a 2.7 L reaction vessel containing a mixture of iron(III) oxide, hydrogen, iron, and water at equilibrium has the following composition: compound amount Fe,O3 3.66 g H2 4.09 g Fe 4.46 g H20 1.82 g 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....

See similar textbooks

Similar questions

The hydrocarbon naphthalene was frequently used in mothballs until recently, when it was discovered that human inhalation of naphthalene vapors can lead to hemolytic anemia. Naphthalene is 93.71% carbon by mass, and a 0.256-mole sample of naphthalene has a mass of 32.8 g. What is the molecular formula of naphthalene? This compound works as a pesticide in mothballs by. sublimation of the .solid so that it fumigates enclosed spaces with its vapors according to the equation Naphthalene(s)naphthalene(g)K=4.29106(at298K) If 3.00 g solid naphthalene is placed into an enclosed space with a volume of 5.00 L at 25C, what percentage of the naphthalene will have sublimed once equilibrium bas been established?
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.
At a certain temperature, K=0.29 for the decomposition of two moles of iodine trichloride, ICl3(s), to chlorine and iodine gases. The partial pressure of chlorine gas at equilibrium is three times that of iodine gas. What are the partial pressures of iodine and chlorine at equilibrium?
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?
The figures below represent the following reaction at equilibrium at different temperatures. A2(g)+3B2(g)2AB3(g)where squares represent atom A and circles represent atom B. Is the reaction exothermic?
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.
. 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?
Nitrogen, hydrogen, and ammonia are in equilibrium in a 1000-L reactor at 550 K. The concentration of N2 is 0.00485 M, H2 is 0.022 M, and NH3 is 0.0016 M. The volume of the container is halved, to 500 L. (a) Calculate the equilibrium constant. (b) Define y as the change in the concentration of nitrogen in the 500-L container. Is y positive or negative? (c) Write the iCe table and express the equilibrium constant in a polynomial in terms of y.
Mustard gas, used in chemical warfare in World War I, has been found to be an effective agent in the chemotherapy of Hodgkin's disease. It can be produced according to the following reaction: SCl2(g)+2C2H4(g)S(CH2CH2Cl)2(g)An evacuated 5.0-1- flask at 20.0C is filled with 0.258 mol SCl2 and 0.592 mol C2H4. After equilibrium is established, 0.0349 mol mustard gas is present. (a) What is the partial pressure of each gas at equilibrium? (b) What is K at 20.0C?
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.
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?