Methanol liquid burns readily in air. One way to represent this equilibrium is: co2(2) + 2 H,0(g)CH;OH(1) + 3/2 0;(g) We could also write this reaction three other ways, listed below. The equilibrium constants for all of the reactions are related. Write the equilibrium constant for each new reaction in terms of K, the equilibrium constant for the reaction above. 1) 2 CH3OH(1) + 3 02(g) =2 CO2(g) + 4 H2O(g) K1 = 2) 2 CO2(g) + 4 H,0(g) =2 CH3OH(1) + 3 O2(g) K2 = 3) CH3OH(1) + 3/2 0;(g) =CO2(g) + 2 H2O(g) K3 = Drag and drop your selection from the following list to complete the answer: K? 1/K (1/K)?

Methanol liquid burns readily in air. One way to represent this equilibrium is: co2(2) + 2 H,0(g)CH;OH(1) + 3/2 0;(g) We could also write this reaction three other ways, listed below. The equilibrium constants for all of the reactions are related. Write the equilibrium constant for each new reaction in terms of K, the equilibrium constant for the reaction above. 1) 2 CH3OH(1) + 3 02(g) =2 CO2(g) + 4 H2O(g) K1 = 2) 2 CO2(g) + 4 H,0(g) =2 CH3OH(1) + 3 O2(g) K2 = 3) CH3OH(1) + 3/2 0;(g) =CO2(g) + 2 H2O(g) K3 = Drag and drop your selection from the following list to complete the answer: K? 1/K (1/K)?

Living By Chemistry: First Edition Textbook

1st Edition

ISBN:9781559539418

Author:Angelica Stacy

Publisher:Angelica Stacy

ChapterU6: Showtime: Reversible Reactions And Chemical Equilibrium

SectionU6.4: How Favorable: Equilibrium Constank K

Problem 5E

See similar textbooks

Similar questions

What is the law of mass action? Is it true that the value of K depends on the amounts of reactants and products mixed together initially? Explain. Is it true that reactions with large equilibrium constant values are very fast? Explain. There is only one value of the equilibrium constant for a particular system at a particular temperature, but there is an infinite number of equilibrium positions. Explain.
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?
. Explain what it means that a reaction has reached a state of chemical equilibrium. Explain why equilibrium is a dynamic state: Does a reaction really “stop” when the system reaches a state of equilibrium? Explain why, once a chemical system has reached equilibrium, the concentrations of all reactants remain constant with time. Why does this constancy of concentration not contradict our picture of equilibrium as being dynamic? What happens to the rates of the forward and reverse reactions as a system proceeds to equilibrium from a starting point where only reactants are present?
Explain that equilibrium is dynamic, and that at equilibrium the forward and backward reaction rates are equal.
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