HW#7Kc = 5 x 1012CHEM 185 Skills Class1. Consider the following equilibrium:Equilibrium2 NO (g) + O2 (g) 2 NO2 (g)a. Calculate the equilibrium constants, Kc, for the following reactions:O2(g) NO2 (g)NO (g) +2 NO2 (g)NO2 (g)2 NO (g) + O2(g)NO (g) + ½ O2 (g)b. Calculate the value of K, at 298 K for 2 NO (g) + O2 (g) 2 NO2 (g)

For the reaction 𝑁𝑂(𝑔)+1/2𝑂2(𝑔)⇌𝑁𝑂2(𝑔)NO(g)+1/2O2(g)⇌NO2(g)- the equilibrium constant is…

Answered: HW#7 Kc = 5 x 1012 CHEM 185 Skills…

Chemistry

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ISBN:9781305957404

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Chapter1: Chemical Foundations

Section: Chapter Questions

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

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(Q97) What is the value of the equilibrium constant (Keg) for the following hypothetical reaction: 2 W (g) + X (g) 3 Y (g) Using the related hypothetical equations should be helpful: X (g) + 1/2 Y (g) W (g) + 1/2 Z (g) K = 0.211 2 Y + Z 3 X (g) K2 = 140
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4. Write an equilibrium equation, keq for the following reactions: a. N2 (g) + 3H2 (g) → 2NH3 (g) b. H2 (g) + I2 (g) → 2HI (g)
For the following equilibrium, Kc = 56 at a given temperature. At equilibrium, [CH4] = 0.2 and [Cl2] = 0.4. What are the equilibrium concentrations of CH3Cl and HCl if they are equal?
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On the basis of Kc for the following reaction, would you expect the reaction to go almost completely to product at equilibrium? N2(g) + 2O2(g) ↔ 2NO(g); Kc = 3x10-17 yes or no
Examine the following reaction. 2 N2OH( aq) + H 2(g) 5 2 Na(s)+ 2 H 2 O(1) What is the equilibrium expression for the reaction? O K = [NAOH][H2] / ([Na] [H2O]) OK = [NaOH]² [H2] O K = 1/[N2OH]? [H2] O K = [N2OH] [H2) O K = 1/[N2OH][H2] O Kc = [Na]? [H2O]² / ([NaOH]? [H2]) O K = [Na][H2O]/ ([NaOH] [H2]) O K = [Na][H2O] O K = 1/ [Na] [H2O] O K = [N2OH]? [H2] / ([Na]² [H2O]?) %3D
At 200 °C, Kc = 1.40 x 10-10 for the reaction N₂O(g) + NO₂(g) = 3NO(g) If 0.272 mol of N₂O and 0.523 mol NO2 are placed in a 4.00 L container, what would the NO concentration be if this equilibrium were established? [NO] = i M
Can you show me how to answer this type of question I found on a online practice organic chemistry review.
Given the following reactions and equilibrium constants: (1) HCN(g) + OH* — CN- + H₂O (g) K₁ =4.9 x 104 (2) H₂O(g) H¹(g) + OH- K₂ = 1.0 x 10-14 - What will be the equilibrium constant for: HCN(g) → CN- + H* (g) ? um constant 5.9 x 104 4.9 x 10-10 5.0 x 10-10 4.9 x 10-40 4.9 x 1018
Given the following reaction what is the expression for Kc? 2SO2(g)+O2(g)->2SO3(g) a.What is the expression for the equilibrium constant? b.If the equilibrium constant for this reaction is 3.70 X 10-7, are the products or the reactants favored? c.What is the equilibrium constant for the reverse reaction? d.What is the equilibrium constant for the reaction below? 6 SO3(g)-> 6 SO2(g)+3O2(g)

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