Sulfuryl chloride, SO₂ Cl2, is a compound with very irritating vapors; itis used as a reagent in the synthesis of organic compounds. Whenheated to a sufficiently high temperature, it decomposes to SO2 andCl₂.SO₂ Cl₂ (g) → SO₂ (g) + Cl₂ (g)Kc=0.045 at 375°C Now, do the same calculation, but here, starting with 7.00 g of SO2 Cl2(which gave an initial concentration of [SO₂Cl₂] = 0.0519 mol/L) and aCl2 pressure of 1.00 atm in the 1.00-L flask. What is the concentrationof SO2 C12 in the system when equilibrium is achieved?Concentration =mol/L

Answer: Initially in the system two gases SO2Cl2 and Cl2 are present and we have to find out the…

Now, do the same calculation, but here, starting with 7.00 g of SO2 Cl2 (which gave an initial concentration of [SO₂Cl₂] = 0.0519 mol/L) and a Cl2 pressure of 1.00 atm in the 1.00-L flask. What is the concentration of SO₂ Cl2 in the system when equilibrium is achieved? Concentration = mol/L

Now, do the same calculation, but here, starting with 7.00 g of SO2 Cl2 (which gave an initial concentration of [SO₂Cl₂] = 0.0519 mol/L) and a Cl2 pressure of 1.00 atm in the 1.00-L flask. What is the concentration of SO₂ Cl2 in the system when equilibrium is achieved? Concentration = mol/L

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter15: Additional Aqueous Equilibria

Section: Chapter Questions

Problem 84QRT

See similar textbooks

Related questions

Q: Suppose a 250. mL flask is filled with 1.4 mol of I₂ and 0.10 mol of HI. The following reaction…

A: The volume of the flask = 250 mL = 0.250 L (1 L = 1000 mL) Number of moles of I2 = 1.4 mol Number of…

Q: 2 SO2(g) + O2(g) ---> 2 SO3(g). You place 1.00 mol/L each of SO2 and O2 in a flask and…

A: Given :- 2 SO2(g) + O2(g) ---> 2 SO3(g) initial concentration of SO2 = 1.00 mol/L or 1.00…

Q: Suppose a 500. mL flask is filled with 0.60 mol of Cl, and 1.0 mol of HCI. The following reaction…

A: We will first find out the concentration of a given species. We know -After that we will construct…

Q: The equilibrium constant, Keq, for the reaction: 2 NOCl(g) -> 2NO(g) + Cl2(g) is 2.4 x 10-7 (no…

A: At a given temperature and pressure, equilibrium constant (Keq) for each chemical reaction that…

Q: Suppose a 250, ml flask is filled with 0.40 mol of H₂ and 1.1 mol of HI. The following reaction…

A: Molarity can be calculated by dividing number of moles by volume. Here, volume of the flask = 250 mL…

Q: Suppose a 250. mL flask is filled with 0.60 mol of H₂ and 0.30 mol of HI. The following reaction…

Q: At a certain temperature, the reaction 2HF(g) H2(g) + F2(3) has K. = 1.2 x 1013. Does this reaction…

Q: equilibrium constant

A: Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: Suppose a 250.mL flask is filled with 1.0mol of Cl2 and 1.5mol of HCl. The following reaction…

A: Molarity can be calculated by dividing number of moles by volume. Here, volume of the flask = 250…

Q: Tiny samples of aqueous solutions are sketched below, as if under a microscope so powerful that…

A: Answer: When value of reaction quotient is equal to the value of equilibrium constant then system is…

Q: At a certain temperature, the reaction 2HF(g) H₂(g) + F₂(g) has Kc = 1.2 × 10-13. Yes, it proceeds…

Q: Suppose a 500. mL flask is filled with 0.90 mol of NO and 1.9 mol of NO2. The following reaction…

A: The concentration of NO at equilibrium is 2.59 MExplanation:

Q: 4. In some equilibria, the value of K increases as temperature increases. In other equilibria, the…

A: Given reaction is : Ca(OH)2 (s) <---------> Ca2+ (aq) + 2OH- (aq)

Q: Write the expression for their equilibrium constant. a) SO 2 (g) + O 2 (g) SO 3 (g) b) NaHCO3 (s) ->…

Q: At a certain temperature, the reaction 2HF(g) H2(g) + F2(g) has Kc = 1.2 × 10-13. Does this…

Q: A gaseous mixture contains 0.26 mol CO, 0.14 mol H2, and 0.021 mol H2O, plus an unknown amount of…

A: A numerical problem based on equilibrium concept, which is to be accomplished.

Q: Suppose a 500 ml. flask is filled with 1.4 mol of 12 and 1.3 mol of HI. The following reaction…

Q: eaction proceed far towards completion when equilibrium is reached? l HF was placed in a 1.00 L…

A: As we know, if Kc is vert very small ,then reaction is reactant dominated over reactant. And if Kc…

Q: Consider the reaction: PCl3(g) + Cl2(g) → PCl5(g). If [PCl3] = 0.78 M, [Cl2] = 0.44 M, and [PCl5] =…

A: GIVEN: To solve: Value of K=? Calculation:

Q: At a certain temperature, the reaction 2HF(g) H2(g) + F2(g) has Kc = 1.2 × 10-13. Does this reaction…

Q: Suppose a 500. mL flask is filled with 1.8 mol of H₂ and 1.5 mol of HI. The following reaction…

Q: Det a partial equilibrium. Sulfur dioxide and oxygen react to form sulfur trioxide during one of the…

Q: 13. At a constant temperature, a solution of acetic acid has the concentrations at equilibrium…

Q: At a certain temperature, the equilibrium constant, Ke, is 6.12 × 10-3 for the reaction Cl,(g) =…

A: The given reaction is : Cl2(g) ⇌ 2Cl(g) Kc for the reaction = 6.12 x 10-3 Mass of Cl2 = 2.69 g…

Q: Consider the following reaction: CO (g) + 2 H2 (g) = CH3OH (g) A reaction mixture in a 5.15 L flask…

A: Given: CO (g) + 2 H2 (g) <=> CH3OH (g) Mass of CO = 27.1 g Mass of H2 = 2.32 g Mass of CH3OH…

Q: At a certain temperature, 0.4211 mol of N₂ and 1.601 mol of H₂ are placed in a 5.00 L container.…

A: Answer:For any reaction, value of equilibrium constant KC is equal to the ratio of molar…

Q: Le Chatelier’s Principle. Directions: Predict the directions that happen in the system to achieve…

A: Answer: According to Le-chatalier's principle, on changing any parameter of the chemical reaction…

Q: 4 PH3(g) 6 H,(g) + P4(g) the equilibrium concentrations were found to be [PH,] = 0.250 M, [H,] =…

Q: If 1.34 moles each of Br2 and Cl2 are introduced into an 11.0 liter flask and allowed to come to…

A: Consider the given information is as follows; Initial moles of Br2 = 1.34 mol Moles of of Cl2 = 1.34…

Q: Consider the following reaction: 2NOBr(g) 2NO(g) + Br₂ (9) for this question. If 0.340 moles of…

Q: Suppose a 500. mL flask is filled with 1.5 mol of Cl2 and 0.60 mol of HCI. The following reaction…

Q: Consider the following equilibrium: BaSO4(s) Ba2+(aq) + SO4 2-(aq) ; change in heat is >0 Which…

A: The question is based on the concept of Le-chatlier principle. It States that when a system at…

Q: What is the correct K expression for the following reaction? N₂ (g) + 3 H₂ (g) = 2 NH₂ (g) O Kc 1 O…

Q: Consider the following reaction at a high temperature. Br₂(g) 2Br(g) When 1.30 moles of Br2 are put…

A: Given, Br2g ⇔ 2Brg Moles of Br2 put in flask = 1.30 moles Volume of flask = 0.710 L Percent…

Q: Kc

Q: Consider this reaction equation: A2B(g)= 2 A(g) + B(g) If you start with 1.2 M A2B, and if at…

A: From given data Initial concentration of A2B = 1.2 M At equilibrium, decomposed 50% means…

Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

Sulfuryl chloride, SO₂ Cl2, is a compound with very irritating vapors; it
is used as a reagent in the synthesis of organic compounds. When
heated to a sufficiently high temperature, it decomposes to SO2 and
Cl₂.
SO₂ Cl₂ (g) → SO₂ (g) + Cl₂ (g)
Kc
=
0.045 at 375°C

Now, do the same calculation, but here, starting with 7.00 g of SO2 Cl2
(which gave an initial concentration of [SO₂Cl₂] = 0.0519 mol/L) and a
Cl2 pressure of 1.00 atm in the 1.00-L flask. What is the concentration
of SO2 C12 in the system when equilibrium is achieved?
Concentration =
mol/L

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Step 5

Step 6

Step by step

Solved in 6 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

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.
Consider the system 4NH3(g)+3O2(g)2N2(g)+6H2O(l)H=1530.4kJ (a) How will the amount of ammonia at equilibrium be affected by 1. removing O2(g)? 2. adding N2(g)? 3. adding water? 4. expanding the container at constant pressure? 5. increasing the temperature? (b) Which of the above factors will increase the value of K? Which will decrease it?
To a beaker with 500 mL of water are added 95 mg of Ba(NO3)2, 95 mg of Ca(NO3)2, and 100.0 mg of Na2CO3. After equilibrium is established, will there be â€¢ no precipitate? â€¢ a precipitate of BaCO3 only? â€¢ a precipitate of CaCO3 only? â€¢ a precipitate of both CaCO3 and BaCO3? Assume that the volume of the solution is still 500.0 mL after the addition of the salts.
In a solution with carbon tetrachloride as the solvent, the compound VCl4. undergoes dimerization: 2VCl4V2Cl8 When 6.6834 g VCl4. is dissolved in 100.0 g carbon tetrachloride, the freezing point is lowered by 5.97C. Calculate the value of the equilibrium constant for the dimerization of VCl4 at this temperature. (The density of the equilibrium mixture is 1.696 g/cm3, and Kf = 29.8C kg/mol for CCl4.)
. Write the balanced chemical equation describing the dissolving of each of the following sparingly soluble salts in water. Write the expression for K for each process. a. AgIO3(s) c. Zn3(PO4)2(s) b. Sn(OH)2(s) d. BaF2(s)
Assume that a sample of hard water contains 50. mg/L of Mg2+ and 150 mg/L of Ca2+, with HCO3 as the accompanying anion. What mass of CaO should be added to 1.0 L of this aqueous solution to precipitate all the Mg2+ and Ca2+ as CaCO3 and MgCO3? What is the total mass of the two solids formed?
Write a chemical equation for an equilibrium system that would lead to the following expressions (ad) for K. (a) K=(PH2S)2 (PO2)3(PSO2)2 (PH2O)2 (b) K=(PF2)1/2 (PI2)1/2PIF (c) K=[ Cl ]2(Pcl2)[ Br ]2 (d) K=(PNO)2 (PH2O)4 [ Cu2+ ]3[ NO3 ]2 [ H+ ]8
The ore cinnabar (HgS) is an important source of mercury. Cinnabar is a red solid whose solubility in water is 5.5 X 10-2 mol L-1. Calculate its \p. What is its solubility' in grams per 100 g of water?
. K for copper(II)hydroxide, Cu(OH)2, has a value 2.21020at 25 °C. Calculate the solubility of copper(II) hydroxide in mol/L and g/L at 25 °C.
At a certain temperature, the reaction 2HF(g) e H2(g) + F2(g) has K. = 1.2 × 10-13. Does this reaction proceed far towards completion when equilibrium is reached? If 0.029 mol HF was placed in a 1.00 L container, and permitted to come to equilibrium, what would be the concentration of H2 and F2 in the container? Concentration of F2 at equilibrium = i M Concentration of H2 at equilibrium = i M
A student ran the following reaction in the laboratory at 656 K: 2NH3 (9) N2 (9) + 3H₂(g) When she introduced 0.0783 moles of NH3(g) into a 1.00 liter container, she found the equilibrium concentration of H₂(g) to be 0.108 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc = for this question.
At equilibrium, an aqueous solution of formic acid (HCHO₂) has these concentrations: [H+] = 0.0029 M; |CHO;] = 0.0029 M; and |HCHO,] = 0.0467 M. HCHO₂(aq) = H+ (aq) + CHO₂ (aq) What is the value of K of this equilibrium? K= Does the equilibrium lie to the right or to the left? O left right