Enter your answer in the provided box. Carbonyl chloride (COCI), also called phosgene, was used in World War I as a poisonous gas. The equilibrium concentrations for the reaction between carbon monoxide and molecular chlorine to form carbonyl chloride at a certain temperature are [CO] = 0.0250 M, [Cl] = 0.0770 M, and [COCI,] = 0.180 M. Co(g) + Cl,(g) $COCI,(g) Calculate the equilibrium constant (K).

Enter your answer in the provided box. Carbonyl chloride (COCI), also called phosgene, was used in World War I as a poisonous gas. The equilibrium concentrations for the reaction between carbon monoxide and molecular chlorine to form carbonyl chloride at a certain temperature are [CO] = 0.0250 M, [Cl] = 0.0770 M, and [COCI,] = 0.180 M. Co(g) + Cl,(g) $COCI,(g) Calculate the equilibrium constant (K).

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 10CR: . Explain what it means that a reaction has reached a state of chemical equilibrium. Explain why...

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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?
Explain that equilibrium is dynamic, and that at equilibrium the forward and backward reaction rates are equal.
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?
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.
. 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?
Again the experiment in Exercise 12.33 was redesigned. This time, 0.15 mol each of N, and O2 was injected into a 5.0-L container at 2500 K, at which the equilibrium constant is 3.6 X 10-?. What was the composition of the reaction mixture at equilibrium? l'he 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?
The creation of shells by mollusk species is a fascinating process. By utilizing the Ca2+ in their food and aqueous environment, as well as some complex equilibrium processes, a hard calcium carbonate shell can be produced. One important equilibrium reaction in this complex process is HCO3(aq)H+(aq)+CO32(aq)K=5.61011 If 0.16 mole of HCO3 is placed into 1.00 L of solution, what will be the equilibrium concentration of CO32?
. 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?
. Equilibria involving reactants or products in more than one state are said to be _________ .
. 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.
Calculate the value of the equilibrium constant for the reaction N2(g)+2O2(g)2NO2(g) if the concentrations of the species at equilibrium are [N2] = 0.0013, [O2] = 0.0024, and [NO2] = 0.00065.
In a given experiment, 5.2 moles of pure NOCl was placed in an otherwise empty 2.0-L container. Equilibrium was established by the following reaction: 2NOCl(g)2NO(g)+Cl2(g)K=1.6105 a. Using numerical values for the concentrations in the Initial row and expressions containing the variable x in both the Change and Equilibrium rows, complete the following table summarizing what happens as this reaction reaches equilibrium. Let x = the concentration of Cl2 that is present at equilibrium. b. Calculate the equilibrium concentrations for all species.