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2. This reaction has an equilibrium constant of K, = 2.2 x 10 at 298K. %3! 2 COF, (g) + C02 (g) + CF, (g) Calculate K, for each rection and predict whether reactants or products will be favored at equilibrium. a. COF, (g) co2 (g) + CF, (g) b. 6 COF2 (g) + 3 CO2 (g) + 3 CF, (g) c. 2 CO2 (g) + 2 CF, (g) +4 COF2 (g)

2. This reaction has an equilibrium constant of K, = 2.2 x 10 at 298K. %3! 2 COF, (g) + C02 (g) + CF, (g) Calculate K, for each rection and predict whether reactants or products will be favored at equilibrium. a. COF, (g) co2 (g) + CF, (g) b. 6 COF2 (g) + 3 CO2 (g) + 3 CF, (g) c. 2 CO2 (g) + 2 CF, (g) +4 COF2 (g)

Chemistry
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...
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Need help understand question 2 a,b,c
Part IB: Answer the following questions and show your work. 1. Write the expression for the equilibrium constant for each chemical equation: a. 2 BRNO (g) + 2 NO (g) + Br2 (g) b. CO- (aq) + H20 (1) → HC0 (aq) + OH-(aq) c. 2 KC1O3 (s) → 2 KCI (s) + 3 02 (g) 2. This reaction has an equilibrium constant of K, = 2.2 x 106 at 298K. 2 COF, (g) C02 (g) + CF, (g) Calculate Kp for each rection and predict whether reactants or products will be favored at equilibrium. a. COF (g) CO2 (g) + CF, (g) b. 6 COF, (g) → 3 CO2 (g) + 3 CF, (g) c. 2 CO2 (g) + 2 CF, (g) 4 COF2 (g) 3. For the following calculate either K, if K, is given or calculate K, if K, is given. Use a temperature of 900. K. a. I2 (g) 21 (g) Kp = 6.26 * 10-22 b. N2 (g) +3 H2 (g) → 2 NH3 (g) K. = 3.7 * 10®
Transcribed Image Text:Part IB: Answer the following questions and show your work. 1. Write the expression for the equilibrium constant for each chemical equation: a. 2 BRNO (g) + 2 NO (g) + Br2 (g) b. CO- (aq) + H20 (1) → HC0 (aq) + OH-(aq) c. 2 KC1O3 (s) → 2 KCI (s) + 3 02 (g) 2. This reaction has an equilibrium constant of K, = 2.2 x 106 at 298K. 2 COF, (g) C02 (g) + CF, (g) Calculate Kp for each rection and predict whether reactants or products will be favored at equilibrium. a. COF (g) CO2 (g) + CF, (g) b. 6 COF, (g) → 3 CO2 (g) + 3 CF, (g) c. 2 CO2 (g) + 2 CF, (g) 4 COF2 (g) 3. For the following calculate either K, if K, is given or calculate K, if K, is given. Use a temperature of 900. K. a. I2 (g) 21 (g) Kp = 6.26 * 10-22 b. N2 (g) +3 H2 (g) → 2 NH3 (g) K. = 3.7 * 10®
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