69. Carbon reacts with water vapor at elevated temperatures. C(s) + H₂O(g) = CO(g) + H₂(g) Kc 0.2 at 1000°C Assuming a reaction mixture initially contains only reactants, what is the concentration of CO in an equilibrium mixture with [H₂O] = 0.500 M at 1000 °C? You can solve this with just algebra, or use an ICE table to make it clearer. Actually, the ICE table seems to make it more confusing. Please write the equilibrium expression and create your equation from that. Enter your answer with one sig fig. [CO] =

69. Carbon reacts with water vapor at elevated temperatures. C(s) + H₂O(g) = CO(g) + H₂(g) Kc 0.2 at 1000°C Assuming a reaction mixture initially contains only reactants, what is the concentration of CO in an equilibrium mixture with [H₂O] = 0.500 M at 1000 °C? You can solve this with just algebra, or use an ICE table to make it clearer. Actually, the ICE table seems to make it more confusing. Please write the equilibrium expression and create your equation from that. Enter your answer with one sig fig. [CO] =

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 12.35PAE: In the reaction in Exercise 12.33, another trial was carried out. The reaction began with an initial...

See similar textbooks

Similar questions

. 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?
The experiment in Exercise 12.33 was redesigned so that the reaction started with 0.15 mol each of N2 and O2 being injected into a 1.0-L container at 2500 K. The equilibrium constant at 2500 K is 3.6 X 10“’. What was the composition of the reaction mixture after equilibrium was attained? The following reaction establishes equilibrium at 2000 K: N2(g) + O2(g) *2 2 NO K = 4.1 X IO-4 If the reaction began with 0.100 mol L-1 of N2 and 0.100 mol L-’ ofO2, what were the equilibrium concentrations of all species?
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.
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?
Which reaction mechanism assumptions are unimportant in describing simple ionic reactions between cations and anions? Why?
Suppose 0.086 mol of Br2 is placed in a 1.26-L flask and heated to 1756 K, a temperature at which the halogen dissociates to atoms. Br2(g) 2 Br(g) If Br2 is 3.7% dissociated at this temperature, calculate Kc.
In the reaction in Exercise 12.33, another trial was carried out. The reaction began with an initial concentration of N2 equal to the initial concentration of NO. Each had a concentration of 0.100 mol L-1. WTat were the equilibrium concentrations of all species? The following reaction establishes equilibrium at 2000 K: N2(g) + O2(g) ^2 NO K = 4.1 X 10~4 If the reaction began with 0.100 mol L-1 of N2 and 0.100 mol L'1 ofO2, what were the equilibrium concentrations of all species?
At 2300 K the equilibrium constant for the formation of NO(g) is 1.7 103. N2(g) + O2(g) 2 NO(g) (a) Analysis shows that the concentrations of N2 and O2 are both 0.25 M, and that of NO is 0.0042 M under certain conditions. Is the system at equilibrium? (b) If the system is not at equilibrium, in which direction does the reaction proceed? (c) When the system is at equilibrium, what are the equilibrium concentrations?
. How does the collision model account for the fact that a react ion proceeds faster when the concentrations of the reactants are increased?
. Mercury(I) chloride, Hg2Cl2, was formerly administered orally as a purgative. Although we usually think of mercury compounds as highly toxic, the K of mercury(I) chloride is small enough (1.31018)that the amount of mercury that dissolves and enters the bloodstream is tiny. Calculate the concentration of mercury(I) ion present in a saturated solution of Hg2Cl2.
. The equilibrium constant for the reaction 2NOCl(g)2NO(g)+Cl2(g)has the value 9.2106at a particular temperature. The system is analyzed at equilibrium, and it is found that the concentrations of NOCl(g) and NO(g) are 0.44 M and 1.5103M. respectively. What is the concentration of Cl2(g) in the equilibrium system under these conditions?
Is a system at equilibrium if the rate constants of the forward and reverse reactions are equal?