An equilibrium mixture contains 0.5 mol of each of A and B and 3.5 mol of C in one-liter container at a certain temperature. (a) How many moles of C must be added to the con- tainer to increase the new equilibrium mole number of A to 0.75? (b) If 1 mol of each of A, B and C is added to the first equilibrium mixture, what will be the new equi- librium concentration of each species at the same emperature?

An equilibrium mixture contains 0.5 mol of each of A and B and 3.5 mol of C in one-liter container at a certain temperature. (a) How many moles of C must be added to the con- tainer to increase the new equilibrium mole number of A to 0.75? (b) If 1 mol of each of A, B and C is added to the first equilibrium mixture, what will be the new equi- librium concentration of each species at the same emperature?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

The reaction CO(g) + H,O(g) 2 C02(g) + H2(g) has AH = -9.8 kcal/mol (-41 kJ/mol). Does the amount of H2 in an equilibrium mixture increase or decrease when the temperature is decreased? %3D The reactio
At a certain temperature, the equilibrium constant K for the following reaction is 0.0069: Br,(g) + OC1,(g) = BROCI(g) + BrC1(g) Use this information to complete the following table. Suppose a 48. L reaction vessel is filled with 1.8 mol of Br, and O There will be very little Br, and OCl,. 1.8 mol of OCl,. What can you say about the composition of the mixture in the vessel at equilibrium? O There vwill be very little BroCl and BrCI. O Neither of the above is true. What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K =I BROC1(g)+BIC1(9) Br,(9)+OC1,(9) What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K =I 2 Br,(g)+20C1,(9) 2 BIOC1(9)+2BrC1(9) 1. Check 02021 McGrmw-Hill Education All Rights Reseved Ters of Uhe Explanation
What can be said about the magnitude of the equilibrium constant in a reaction whose equilibrium lies far to the right? To the left?
A.) At a certain temperature, 0.720 mol SO3 is placed in a 3.00 L container. 2SO3(g)↽−−⇀2SO2(g)+O2(g) At equilibrium, 0.150 mol O2 is present. Calculate ?c. Answer is not 0.0765 B.) Phosphorus pentachloride decomposes according to the chemical equation PCl5(g)↽−−⇀PCl3(g)+Cl2(g)?c=1.80 at 250 ∘C A 0.1974 mol sample of PCl5(g) is injected into an empty 2.65 L reaction vessel held at 250 ∘C. Calculate the concentrations of PCl5(g) and PCl3(g) at equilibrium.
Hydrofluoric acid and water react to form fluoride anion and hydronium cation, like this: + HF(aq)+H,O(1)→F (aq)+H;O"(aq) At a certain temperature, a chemist finds that a 2.7 L reaction vessel containing an aqueous solution of hydrofluoric acid, water, fluoride anion, and hydronium cation at equilibrium has the following composition: compound amount HF 2.21 g H,0 857. g F 0.169 g H;O 0.141 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K = 0
1.)Hydrogen sulfide, a colorless gas with a foul odor, dissociates on heating: 2H2S(g) 2H2(g)+ S2(g) When 0.100 mol H2S was put into a 10.0-L vessel and heated to 1132°C, it gave an equilibrium mixture containing 0.0285 mol H2. What is the value of Kc at this temperature? 2.) In the contact process, sulfuric acid is manufactured by first oxidizing SO, to SO3, which is then reacted with water. The reaction of SO2 with 02 is 2SO2(g) + O2(g) 2S03(g) A 2.000-L flask was filled with 0.0400 mol SO2 and 0.0200 mol O2. At equilibrium at 900 K, the flask contained 0.0296 mol SO3. How many moles of each substance were in the flask at equilibrium? Whatis the value of Kc at this temperature?
Consider the equilibrium between COCl2, CO and Cl2.COCl2(g) CO(g) + Cl2(g) K = 0.142 at 920 KThe reaction is allowed to reach equilibrium in a 8.00-L flask. At equilibrium, [COCl2] = 0.309 M, [CO] = 0.209 M and [Cl2] = 0.209 M. (a) The equilibrium mixture is transferred to a 16.0-L flask. In which direction will the reaction proceed to reach equilibrium? (b) Calculate the new equilibrium concentrations that result when the equilibrium mixture is transferred to a 16.0-L flask. [COCl2] M = [CO] M = [Cl2] M = If your equilibrium values are correct, when you substitute them into the equilibrium expression you should reproduce the value of K given. please do this part last two times I asked they didn't and gave me the wrong answer
At a certain temperature, 0.900 mol SO, is placed in a 5.00 L container. 2 SO₂(g) 2 SO₂(g) + O₂(g) At equilibrium, 0.170 mol O₂ is present. Calculate Ke.
Consider the equilibrium between SO₂Cl₂, SO₂ and Cl₂. SO₂Cl₂(g) SO₂(g) + Cl₂(g) K 0.193 at 390 K The reaction is allowed to reach equilibrium in a 5.80-L flask. At equilibrium, [SO₂Cl₂] = 0.290 M, [SO₂] = 0.237 M and [Cl₂] = 0.237 M. (a) The equilibrium mixture is transferred to a 11.6-L flask. In which direction will the reaction proceed to reach equilibrium? (b) Calculate the new equilibrium concentrations that result when the equilibrium mixture is transferred to a 11.6-L flask. [SO₂Cl₂] = [SO₂] [Cl₂] = M
Hydrofluoric acid and water react to form fluoride anion and hydronium cation, like this: + HF(aq)+H,O(1)→→F (aq)+H;O"(aq) At a certain temperature, a chemist finds that a 9.1 L reaction vessel containing an aqueous solution of hydrofluoric acid, water, fluoride anion, and hydronium cation at equilibrium has the following composition: compound amount HF 1.65 g H,O 745. g F 0.150 g H;O* 0.136 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K = x10 ?
Nitrogen monoxide, NO, reacts with bromine, Br2, to give nitosyl bromide, NOBr. 2NO (g) +Br2(g) --> <-- 2NOBr (g) A sample of 0.425 mole NO with 0.626 mole Br2 in a 1.25 L reaction vessel gives an equilibrium mixture containing 0.113 mol NOBr. What is the composition of the equilibrium mixture in term of Molarity?
Q3. At 298 K, F3SSF(g) decomposes partially to SF2(g). At equilibrium, the partial pressure of SF2(g) is 1.1X10-4 atm and the partial pressure of F3SSF is 0.0484 atm. (a) Write a balanced equilibrium equation to represent this reaction. (b) Compute the equilibrium constant corresponding to the equation you wrote. (c) Some SF2 (at a partial pressure of 2.3X10-4 atm) is placed in a closed container at 298 K with some F3SSF (at a partial pressure of 0.0484 atm). Enough argon is added to raise the total pressure to 1.000 atm. Calculate the initial reaction quotient for the decomposition of F3SSF to SF2.