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10. Use the information given for each of the following reactions and predict the direction (right, left, etc.) and magnitude of x (large, small, etc.). If no initial concentration is given for a species, assume that species is not initially present. a.) AgNO3(aq) = Ag+ (aq) + NO3(aq) K = 8.9 x 10-8 [AgNO3];= 3.40 M b.) Ag+ (aq) + 2NH3 (aq) = [Ag(NH3)₂] (aq) K = 1.1 × 107 c.) H₂(g) + 12(g) = 2HI(g) K = 3.5 x 10-7 [Ag+]₁ = [NH3]; = 3.40M [HI]; = 2.44M

10. Use the information given for each of the following reactions and predict the direction (right, left, etc.) and magnitude of x (large, small, etc.). If no initial concentration is given for a species, assume that species is not initially present. a.) AgNO3(aq) = Ag+ (aq) + NO3(aq) K = 8.9 x 10-8 [AgNO3];= 3.40 M b.) Ag+ (aq) + 2NH3 (aq) = [Ag(NH3)₂] (aq) K = 1.1 × 107 c.) H₂(g) + 12(g) = 2HI(g) K = 3.5 x 10-7 [Ag+]₁ = [NH3]; = 3.40M [HI]; = 2.44M

Chemistry: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter14: Chemical Equilibrium
Section: Chapter Questions
Problem 14.3QE: Describe a nonchemical system that is not in equilibrium, and explain why equilibrium has not been...
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10. Use the information given for each of the following reactions and predict the direction (right, left, etc.) and magnitude of x (large, small, etc.). If no initial concentration is given for a species, assume that species is not initially present. a.) AgNO3(aq) = Ag+ (aq) + NO3(aq) K = 8.9 x 108 [AgNO3];= 3.40 M b.) Ag¹ (aq) + 2NH3 (aq) = [Ag(NH3)21+ (aq) K = 1.1 × 10² c.) H₂(g) + 1₂(g) = 2HI(g) [Ag+]₁ = [NH3]₁ = 3.40M Kc=3.5 × 10~ [HI]=2.44M 10-7
Transcribed Image Text:10. Use the information given for each of the following reactions and predict the direction (right, left, etc.) and magnitude of x (large, small, etc.). If no initial concentration is given for a species, assume that species is not initially present. a.) AgNO3(aq) = Ag+ (aq) + NO3(aq) K = 8.9 x 108 [AgNO3];= 3.40 M b.) Ag¹ (aq) + 2NH3 (aq) = [Ag(NH3)21+ (aq) K = 1.1 × 10² c.) H₂(g) + 1₂(g) = 2HI(g) [Ag+]₁ = [NH3]₁ = 3.40M Kc=3.5 × 10~ [HI]=2.44M 10-7
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