For a reaction involving nitrogen monoxide inside a sealed flask, the value for the reaction quotient (Q) was found to be 1.1 × 102 at a given point. If, after this point, the amount of NO gas in the flask increased, which reaction is most likely taking place in the flask?

NOBr(g) ↔ NO(g) + ½Br2(g) Kc = 3.4 × 10-2

2NOCl(g) ↔ 2NO(g) + Cl2(g) Kc = 1.6 × 10-5

2NO(g) + 2H2(g) ↔ N2(g) + 2H2O(g) Kc = 4.0 × 106

N2(g) + O2(g) ↔ 2NO(g) Kc = 4.2 × 102

Chemistry

College Board

Exam No：AP Chemistry Problem Set 3 Year：2024 Question No：APChemistry2024AP0096

Answer:

7.1 Introduction to Equilibrium

7.10 Reaction Quotient and Le Châtelier’s Principle

7.11 Introduction to Solubility Equilibria

7.12 Common-Ion Effect

7.2 Direction of Reversible Reactions

7.3 Reaction Quotient and Equilibrium Constant

7.4 Calculating the Equilibrium Constant

7.5 Magnitude of the Equilibrium Constant

7.6 Properties of the Equilibrium Constant

7.7 Calculating Equilibrium Concentrations

7.8 Representations of Equilibrium

7.9 Introduction to Le Châtelier’s Principle

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