Exercise 15.36 Enhanced - with Feedback%3DPart AMISSED THIS? Watch IWE 15.5; Read Section 15.6.You can click on the Review link to access the section inyour e Text.What is the value of the equilibrium constant (Kc) at this temperature?Consider the following reaction:Express the equilibrium constant to three significant figures.NH,HS (s) = NH3 (g) + H2S (g)ΑΣφAn equilibrium mixture of this reaction at a certaintemperature was found to have [NH3] = 0.272 M and[H2S] = 0.370 M.%3D

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Exercise 15.36 Enhanced - with Feedback Part A MISSED THIS? Watch IWE 15.5; Read Section 15.6. You can click on the Review link to access the section in your e Text. What is the value of the equilibrium constant (K.) at this temperature? Consider the following reaction: Express the equilibrium constant to three significant figures. NH,HS (s) - NH3 (g) + H2S (g) ΑΣφ An equilibrium mixture of this reaction at a certain temperature was found to have [NH3] = 0.272 M and [H2S] = 0.370 M. K =

Exercise 15.36 Enhanced - with Feedback Part A MISSED THIS? Watch IWE 15.5; Read Section 15.6. You can click on the Review link to access the section in your e Text. What is the value of the equilibrium constant (K.) at this temperature? Consider the following reaction: Express the equilibrium constant to three significant figures. NH,HS (s) - NH3 (g) + H2S (g) ΑΣφ An equilibrium mixture of this reaction at a certain temperature was found to have [NH3] = 0.272 M and [H2S] = 0.370 M. K =

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

Chapter14: Chemical Equilibirum

Section14.7: Removing Products Or Adding Reactants

Problem 14.12E

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issue 13Balance the reaction below and write the expression for the equilibrium constant. NO(g) + Cl2(g) ⇌ NOCl(g)I found as a balanced equation: 2NO(g) + Cl2(g) ⇌ 2NOCl(g) and as Kc= 2.5 x 103.Is it correct ?
Consider the following hypothetical reactions. The equilibrium constants K given for each reaction are defined in terms of a concentration unit of molecules per liter. A(g)B(g)K=2X(g)2Y(g)K=62C(g)D(g)K=1 Assume that the reactions have reached equilibrium. Match each of these reactions with one of the containers I to IV (each of which has a volume of 1 L). Identify the color of each molecule (for example, is A red or blue?).
Solid calcium hydroxide is dissolved in water until the pH of the solution is 11.44. What is the hydroxide ion concentration [OH–] of the solution? Show work.
Reaction: 1 A + 1B → 3C The initial [A] is 0.80 M and [B] is 4.90 M. At equilibrium, [A] is 0.40 M. What is the value of K? Answer: 19.44 (0.96)
K=4.9x10-3 for the reaction CO2(g)+H2(g)⇄ CO(g)+H2O(g). If [CO2]=0.00025 M, [H2]=0.0010 M, & [CO]=0.000015 M, what is the concentration at equilibrium of H2O? Answer 8.2x10-5M I got 1.84x10^-14? Can someone explain this to me please.
Exercise: At 373 K, the equilibrium constant for the reaction COCl2(g) D CO(g) + Cl2(g) is 2.9x10-10. The concentrations of the gases in a 1-L reaction flask are [COCl2]= 3.50x10-3 M, [Cl2]=3.25x10-6 M, and [CO]=1.11x10-5 M. (a) Is the mixture of gases at equilibrium? Answer should be supported with calculations. (b) If not, which direction will the reaction proceed to reach equilibrium?
Exercise 17.5 For the exothermic reaction 2SO2(g)+O2(g)2SO3(g)predict the equilibrium shift caused by each of the following changes. a. SO2is added. b. SO3is removed. c. The volume is decreased. d. The temperature is decreased.
Give the expression for K for each of the following reactions. a. CaCO3(s)CaO(s)+CO2(g) b. PbI2(s)Pb2+(aq)+2I(aq) c. H+(aq)+HCO3(aq)H2O(l)+CO2(g)
Use the data from Table 18.2 to obtain the equilibrium constant Kp at 25C for the reaction CaCO3(s)CaO(s)+CO2(g) Note that values of Gf are needed for CaCO3 and CaO, even though the substances do not appear in Kp=PCO2.
The Mond process for purifying nickel involves the formation of nickel tetracarbonyl, Ni(CO)4, a volatile liquid, from nickel metal and carbon monoxide. Carbon monoxide is passed over impure nickel to form nickel carbonyl vapor, which, when healed, decomposes and deposits pure nickel. Ni(s)+4CO(g)Ni(CO)4(g) Write the expression for Kc for this reaction.
Calculate the equilibrium constant of the reaction CO(g) + 2 H2S(g) CS2(g) + H2O(g) + H2(g) from the following information: CO(g) + 3 H2(g) CH4(g) + H2O(g) K = 9.17 x 10-2 CH4(g) + 2 H2S(g) CS2(g) + H2(g) K = 3.3 x 104 Answer: [3.03 x 103 ]
What is the equilibrium constant of the following reaction at 25˚C? F⁻(aq) + H⁺(aq) ⇄ HF(aq) 1) 1.0 × 10⁻⁷ 2) 6.3 × 10⁻⁴ 3) 6.3 × 10¹⁰ 4) 1.6 × 10³ 5) 1.6 × 10⁻¹¹ Pls give typed answer no hand written .

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