Q2 The equilibrium constant, K, for the following reaction is 1.29x102 at 600 K.COCI₂(g) CO(g) + Cl₂(g)An equilibrium mixture of the three gases in a 1.00 L flask at 600 K contains 0.264 M COCI₂, 5.83x102 MCO and 5.83x102 M Cl₂. What will be the concentrations of the three gases once equilibrium has beenreestablished, if 4.50x102 mol of Cl₂(g) is added to the flask?[CoCl₂]=[CO][Cl₂]The equilibrium constant, K, for the following reaction is 10.5 at 350 K.2CH₂Cl₂(9)CH4(9) + CCL4 (9)MMMAn equilibrium mixture of the three gases in a 1.00 L flask at 350 K contains 5.55x102 M CH₂Cl₂, 0.180M CH4 and 0.180 M CCI4. What will be the concentrations of the three gases once equilibrium has beenreestablished, if 0.125 mol of CH4(g) is added to the flask?[CH₂Cl₂] =[CH4][CCI4]MMM

Dear student , since you have posted multiple questions we are allowed to solve only first question…

The equilibrium constant, K, for the following reaction is 1.29x102 at 600 K. COCI₂(g)=CO(g) + Cl₂(g) An equilibrium mixture of the three gases in a 1.00 L flask at 600 K contains 0.264 M COCl₂, 5.83x102 M CO and 5.83x102 M Cl₂. What will be the concentrations of the three gases once equilibrium has been reestablished, if 4.50x102 mol of Cl₂(g) is added to the flask? [COCI₂] = [Co] = [Cl₂] = M M M e equilibrium constant, K, for the following reaction is 10.5 at 350 K. 2CH₂Cl₂(9) CH4(9) + CCl4(9)

The equilibrium constant, K, for the following reaction is 1.29x102 at 600 K. COCI₂(g)=CO(g) + Cl₂(g) An equilibrium mixture of the three gases in a 1.00 L flask at 600 K contains 0.264 M COCl₂, 5.83x102 M CO and 5.83x102 M Cl₂. What will be the concentrations of the three gases once equilibrium has been reestablished, if 4.50x102 mol of Cl₂(g) is added to the flask? [COCI₂] = [Co] = [Cl₂] = M M M e equilibrium constant, K, for the following reaction is 10.5 at 350 K. 2CH₂Cl₂(9) CH4(9) + CCl4(9)

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 60QRT

See similar textbooks

Similar questions

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?
The equilibrium constant Kc, for the reaction 2 NOCI(g) 2 NO(g) + Cl2(g) is 3.9 103 at 300 C. A mixture contains the gases at the following concentrations: [NOCl] = 5.0 103 mol/L, [NO] = 2.5 103 mol/L, and [Cl2] = 2.0 103 mol/L. Is the reaction at equilibrium at 300 C? If not, in which direction does the reaction proceed to come to equilibrium?
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?
Consider 0.200 mol phosphorus pentachloride sealed in a 2.0-L container at 620 K. The equilibrium constant, Kc, is 0.60 for PCl5(g) PCl3(g) + Cl2(g) Calculate the concentrations of all species after equilibrium has been reached.
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
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.
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?
Consider the equilibrium N2(g)+O2(g)2NO(g) At 2300 K the equilibrium constant Kc = 1.7 103. If 0.15 mol NO(g) is placed into an empty, sealed 10.0-L flask and heated to 2300 K, calculate the equilibrium concentrations of all three substances at this temperature.
The diagram represents an equilibrium mixture for the reaction N2(g) + O2(g) ⇌ 2 NO(g) Estimate the equilibrium constant.
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 room temperature, the equilibrium constant Kc for the reaction 2 NO(g) ⇌ N2(g) + O2(g) is 1.4 × 1030. Is this reaction product-favored or reactant-favored? Explain your answer. In the atmosphere at room temperature the concentration of N2 is 0.33 mol/L, and the concentration of O2 is about 25% of that value. Calculate the equilibrium concentration of NO in the atmosphere produced by the reaction of N2 and O2. How does this affect your answer to Question 11?