please answer completely from a-e General Chemistry 22 Ag + Cl = 2AgClKbe.[CL]2 FeBr 2 FeBr, )+ Br 2ig)K = [Br,]3(s)%3Dbe.Activity 5.1Write the equilibrium constant expression of the following reversible reactions.a. N+ 3Cl 2NCIb. 2NO+2C0 N,+ 2C02)2(g)(g)с. CaFCa+ 2F,2(s)d. BaCO,+2H,O Ba" + H,CO)+ 2H,0e. PCI, PCI+ Cl o(aq)3(aq)5 (@)Significance of Equilibrium ConstantAs stated earlier, a large value of K (K>1) corresponds mostly to products(favors forward reaction), and a small value of K (K<1) indicates mostly the reactantsholpingportance of eqilibrium consta

Since you are asked for multiple sub-parts, we are entitled to solve first three questions.

2(g) 24 : Activity 5.1 Write the equilibrium constant expression of the following reversible reactions. a. N + 3Cl = 2NCI b. 2NO+2CO N, 2(g) 2(0) + 2CO) 2(g) 2(g) c. CaF, Ca) 2(s) + 2F, (b) d. BaCO+2H,O Ba" + H,CO)+ 2H,0 e. PCI, PCIo) (aq) (aq) 3(aq) + Cl, (a) 2 (@)

2(g) 24 : Activity 5.1 Write the equilibrium constant expression of the following reversible reactions. a. N + 3Cl = 2NCI b. 2NO+2CO N, 2(g) 2(0) + 2CO) 2(g) 2(g) c. CaF, Ca) 2(s) + 2F, (b) d. BaCO+2H,O Ba" + H,CO)+ 2H,0 e. PCI, PCIo) (aq) (aq) 3(aq) + Cl, (a) 2 (@)

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 12.22PAE

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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?
Consider the same reaction as in Question 11. In one experiment 1.0 mole of H2O(g) and 1.0 mole of CO(g) are put into a flask and heated to 350C. In a second experiment 1.0 mole of H2(g) and 1.0 mole of CO2(g) are put into another flask with the same volume as the first. This mixture is also heated to 350C. After equilibrium is reached, will there be any difference in the composition of the mixtures in the two flasks?
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?
Many sugars undergo a process called mutarotation, in which the sugar molecules interconvert between two isomeric forms, finally reaching an equilibrium between them. This is true for the simple sugar glucose, C6H12O6, which exists in solution in isomeric forms called alpha-glucose and beta-glucose. If a solution of glucose at a certain temperature is analyzed, and it is found that the concentration of alpha-glucose is twice the concentration of beta-glucose, what is the value of K for the interconversion reaction?
A common type of reaction we will study is that having a very small K value (K 1). Solving for equilibrium concentrations in an equilibrium problem usually requires many mathematical operations to be perfomed. However, the math involved when solving equilibrium problems for reactions having small K values (K 1) is simplified. What assumption is made when solving the equilibrium concentrations for reactions with small K values? Whenever assumptions are made, they must be checked for validity. In general, the 5% rule is used to check the validity of assuming x (or 2 x, 3x, and so on) is very small compared to some number. When x (or 2 x. 3x. and so on) is less than 5% of the number the assumption was made against, then the assumption is said to be valid. If the 5% rule fails, what do you do to solve for the equilibrium concentrations?
Among the solubility rules previously discussed is the statement: All chlorides are soluble except Hg2Cl2, AgCI, PbCl2, and CuCl. (a) Write the expression for the equilibrium constant for the reaction represented by the equation AgCI(s)Ag+CI(aq). Is Kc1,1, or 1? Explain your answer. (b) Write the expression for the equilibrium constant for the reaction represented by the equation Pb2+(aq)+2CI(aq)PbCI2(s). Is Kc1,1, or 1? Explain your answer.
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?
Hydrogen and carbon dioxide react at a high temperature to give water and carbon monoxide. H2(g) + CO2(g) H2O(g) + CO(g) (a) Laboratory measurements at 986 C show that there are 0.11 mol each of CO and H2O vapor and 0.087 mol each of H2 and CO2 at equilibrium in a 50.0-L container. Calculate the equilibrium constant for the reaction at 986 C. (b) Suppose 0.010 mol each of H2 and CO2 are placed in a 200.0-L container. When equilibrium is achieved at 986 C, what amounts of CO(g) and H2O(g), in moles, would be present? [Use the value of Kc from part (a).]
Iodine dissolves in water, but its solubility in a nonpolar solvent such as CCl4 is greater. Extracting iodine (I2) from water with the nonpolar solvent CCl4. I2 is more soluble in CCl4 and, after shaking a mixture of water and CCl4, the I2 has accumulated in the more dense CCl4 layer. The equilibrium constant is 85.0 for the process I2(aq) I2(CCl4) You place 0.0340 g of I2 in 100.0 mL of water. After shaking it with 10.0 mL of CCl4, how much I2 remains in the water layer?
12.42 The following reaction is in equilibrium in lake water: HCO,_(aq) + H+(aq)«=*H,CO,(aq) Predict the change in the reaction quotient, Q, for each disturbance below and use that prediction to explain how the equilibrium is shifted by the stress. NaHCOj is added to the lake. H,CO}is added. NaOH is added.
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?
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?