The equilibrium constant, Kp, for the following reaction is 2.74 at 1.15×10°K. 2S03(g) 2sO,(g) + O2(g) If an equilibrium mixture of the three gases in a 13.7 L container at 1.15×10°K contains SOz at a pressure of 1.17 atm and SO2 at a pressure of 1.47 atm, the equilibrium partial pressure of 0, is atm.

The equilibrium constant, Kp, for the following reaction is 2.74 at 1.15×10°K. 2S03(g) 2sO,(g) + O2(g) If an equilibrium mixture of the three gases in a 13.7 L container at 1.15×10°K contains SOz at a pressure of 1.17 atm and SO2 at a pressure of 1.47 atm, the equilibrium partial pressure of 0, is atm.

General Chemistry - Standalone book (MindTap Course List)

11th Edition

ISBN:9781305580343

Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Chapter21: Chemistry Of The Main-group Elements

Section: Chapter Questions

Problem 21.196QP

See similar textbooks

Similar questions

The equilibrium constant for the reaction 2CrO42(aq)+2H+(aq)Cr2O72(aq)+H2O is 31014 . What must the pH be so that the concentrations of chromate and dichromate ion are both 0.10 M?
An important reaction involved in the operation of vacuum tubes is the following y BaO(s) + x M(XM, s) = MxOy(solid or gas) + y Ba(g) where M is an oxide-forming solute dissolved in the base nickel cathode. Calculate PBa, in equilibrium at 1175°K of M is C at 0.01% and MxOy is CO2(g). C is soluble to the extent of 0.1% in M.
(a) If the molar solubility of Cu3(PO4)2 at 25 oC is 1.67e-08 mol/L, what is the Ksp at this temperature?Ksp = _______(b) It is found that 1.75e-06 g of Cu3(AsO4)2 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Cu3(AsO4)2.Ksp = _______(c) The Ksp of ScF3 at 25 oC is 5.81e-24. What is the molar solubility of ScF3?solubility = ______ mol/L
Consider the insoluble compound iron(II) carbonate , FeCO3 . The iron(II) ion also forms a complex with cyanide ions . Write a balanced net ionic equation to show why the solubility of FeCO3 (s) increases in the presence of cyanide ions and calculate the equilibrium constant for this reaction.For Fe(CN)64- , Kf = 7.7×1036 . Be sure to specify states such as (aq) or (s).
Given the equilibrium constants for the following reactions: 4Cu (s)+O2 (g)》2Cu2O (s), K1=9.76 4 CuO(s)》2Cu2O (s)+ O2 (g), K=0.54. What is the K for the system 2Cu (s)+O2 (g)》2CuO (s) equivalent to?
Iodine is sparingly soluble in pure water. However, it does `dissolve' in solutions containing excess iodide ion because of the following reaction: I-(aq) + I2(aq) I3-(aq) K = 710. For each of the following cases calculate the equilibrium ratio of [I3-] to [I2]. 6.00×10-2 mol of I2 is added to 1.00 L of 6.00×10-1 M KI solution. the answer you provided (299) was not correct
Pbl, solid (Kps = 9.8 x 10-9) is placed in a beaker with water. After some time, the concentration of lead (II) in solution is determined, and the value is 1.1x10-3 mol/L. Is the solution in balance? If not, how will it be achieved?
What are the main equilibria involved in the CO2–Carbonate system and what kind of equilibrium constant is associated with each (K?)? What is the overall reaction for carbonate species in water that is exposed to the atmosphere and carbonate minerals?
(a) If the molar solubility of Tl2S at 25 oC is 5.31e-08 mol/L, what is the Ksp at this temperature?Ksp = (b) It is found that 1.75e-06 g of Cu3(AsO4)2 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Cu3(AsO4)2.Ksp = (c) The Ksp of BaCO3 at 25 oC is 2.58e-09. What is the molar solubility of BaCO3? solubility = ____ mol/L
. The solubility product of magnesium carbonate, MgCO3, has the value Ksp = 6. 82 × 10−6at 25°C. How many grams of MgCO3will dissolve in 1.00L of water?
The KspKsp of a salt corresponds to a reaction with the following general format: salt(s)⇌mcation(aq)+nanion(aq)where mm and nn are the coefficients that balance the equation. Equilibrium constants follow the general format of products over reactants (excluding pure liquids and solids) with each species raised to the power of its coefficient in the balanced equation. KspKsp is no exception, so Ksp=[cation]m[anion]nKsp=[cation]m[anion]n Part A If 500.0 mLmL of 0.10 mol L−1 Ca2+mol L−1 Ca2+ is mixed with 500.0 mLmL of 0.10 mol L−1 SO42−mol L−1 SO42−, what mass of calcium sulfate will precipitate? KspKsp for CaSO4CaSO4 is 2.40× 10−52.40×10−5. Express your answer to three significant figures and include the appropriate units
Dinitrogen tetroxide, N2O4, dissociates at room temperature to give nitrogen dioxide, NO2.N2O4 (g) ⇌ 2 NO2 (g) (a) The equilibrium constant Kc at 25°C is 0,125. What percentage of dinitrogen tetroxideis dissociated when 0,0300 mol N2O4 is placed in a 1,00 dm3 flask and left to reachequilibrium?

SEE MORE QUESTIONS

Recommended textbooks for you

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS