Hydrogen is the lightest of elements with atomic number one. When hydrogen gas reacts with bromine gas, they form hydrogen bromide gas, i.e., H₂(g) + Br₂(g) → 2HBr(g) At equilibrium, concentration values of the compounds are: Compound Equilibrium Concentration [H₂(g)] [Br₂(g)] [HBr(g)] 0.024 mol/L 0.024 mol/L 0.05 mol/L The value of equilibrium constant Keq, for the above reaction, is 2.6 3.1 4.3 5.2 8.7

Hydrogen is the lightest of elements with atomic number one. When hydrogen gas reacts with bromine gas, they form hydrogen bromide gas, i.e., H₂(g) + Br₂(g) → 2HBr(g) At equilibrium, concentration values of the compounds are: Compound Equilibrium Concentration [H₂(g)] [Br₂(g)] [HBr(g)] 0.024 mol/L 0.024 mol/L 0.05 mol/L The value of equilibrium constant Keq, for the above reaction, is 2.6 3.1 4.3 5.2 8.7

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 26E: At high temperatures, elemental nitrogen and oxygen react with each other to form nitrogen monoxide:...

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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?
The following equilibrium was studied by analyzing the equilibrium mixture for the amount of H2S produced. Sb2S3(s)+3H2(g)2Sb(s)+3H2S(g) A vessel whose volume was 2.50 L was filled with 0.0100 mol of antimony(III) sulfide, Sb2S3, and 0.0100 mol H2. After the mixture came to equilibrium in the closed vessel at 440C, the gaseous mixture was removed, and the hydrogen sulfide was dissolved in water. Sufficient lead(II) ion was added to react completely with the H2S to precipitate lead(II) sulfide, PbS. If 1.029 g PbS was obtained, what is the value of Kc at 440C?
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?
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?
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?
The following reaction is earned out at 500 K in a container equipped with a movable piston. A(g)+B(g)C(g);Kc=10(at500K) After the reaction has reached equilibrium, the container has the composition depicted here. Suppose the container volume is doubled. a How does the equilibrium composition shift? b How does the concentration of each of the reactants and the product change? (That is, does the concentration increase, decrease, or stay the same?)
The equilibrium constant, Kc, for the reaction N2O4(g) 2 NO2(g) at 25 C is 5.9 103. Suppose 15.6 g of N2O4 placed in a 5.000-L flask at 25 C. Calculate the following; (a) the amount of NO2 (mol) present at equilibrium; (b) the percentage of the original N2O4 that is dissociated.
The equilibrium constant for the dissociation of iodine molecules to iodine atoms I2(g) 2 I(g) is 3.76 103 at 1000 K. Suppose 0.105 mol of I2 is placed in a 12.3-L flask at 1000 K. What are the concentrations of I2 and I when the system comes to equilibrium?
A sample of gaseous nitrosyl bromide (NOBr) was placed in a container tiued with a frictionless, massless piston, where it decomposed at 25C according to the following equation: 2NOBr(g)2NO(g)+Br2(g) The initial density of the system was recorded as 4.495 g/L. After equilibrium was reached, the density was noted to be 4.086 g/L. a. Determine the value of the equilibrium constant K for the reaction. b. If Ar(g) is added to the system at equilibrium at constant temperature, what will happen to the equilibrium position? What happens to the value of K? Explain each answer
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?
. For the reaction CaCO3(s)CaO(s)+CO2(g)the equilibrium constant K has the form K=[CO2]. Using a handbook to find density information about CaCO3(s) and CaO(s), show that the concentrations of the two solids (the number of moles contained in 1 L of volume) are constant.
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.