Steam reforming of methane (CH4) produces "synthesis gas," a mixture of carbon monoxide gas and hydrogen gas, which is the starting point for many important industrial chemical syntheses. An industrial chemist studying this reaction fills a 500. mL flask with 3.2 atm of methane gas and 4.3 atm of water vapor, and when the mixture has come to equilibrium measures the partial pressure of hydrogen gas to be 0.96 atm. Calculate the pressure equilibrium constant for the steam reforming of methane at the final temperature of the mixture. Round your answer to 2 significant digits. = K-0 x10

Steam reforming of methane (CH4) produces "synthesis gas," a mixture of carbon monoxide gas and hydrogen gas, which is the starting point for many important industrial chemical syntheses. An industrial chemist studying this reaction fills a 500. mL flask with 3.2 atm of methane gas and 4.3 atm of water vapor, and when the mixture has come to equilibrium measures the partial pressure of hydrogen gas to be 0.96 atm. Calculate the pressure equilibrium constant for the steam reforming of methane at the final temperature of the mixture. Round your answer to 2 significant digits. = K-0 x10

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 61QRT

See similar textbooks

Similar questions

Write an equation for an equilibrium system that would lead to the following expressions (ac) for K. (a) K=(Pco)2 (PH2)5(PC2H6)(PH2O)2 (b) K=(PNH3)4 (PO2)5(PNO)4 (PH2O)6 (c) K=[ ClO3 ]2 [ Mn2+ ]2(Pcl2)[ MNO4 ]2 [ H+ ]4 ; liquid water is a product
. What does it mean to say that a state of chemical or physical equilibrium is dynamic?
Write a chemical equation for an equilibrium system that would lead to the following expressions (ad) for K. (a) K=(PH2S)2 (PO2)3(PSO2)2 (PH2O)2 (b) K=(PF2)1/2 (PI2)1/2PIF (c) K=[ Cl ]2(Pcl2)[ Br ]2 (d) K=(PNO)2 (PH2O)4 [ Cu2+ ]3[ NO3 ]2 [ H+ ]8
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?
Describe a nonchemical system that is in equilibrium, and explain how the principles of equilibrium apply to the system.
Because calcium carbonate is a sink for CO32- in a lake, the student in Exercise 12.39 decides to go a step further and examine the equilibrium between carbonate ion and CaCOj. The reaction is Ca2+(aq) + COj2_(aq) ** CaCO,(s) The equilibrium constant for this reaction is 2.1 X 10*. If the initial calcium ion concentration is 0.02 AI and the carbonate concentration is 0.03 AI, what are the equilibrium concentrations of the ions? A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H2COj(aq) H+(aq) + HCO}‘(aq) K = 4.4 X 10"7 She starts with 0.1000 AI carbonic acid. What are the concentrations of all species at equilibrium?