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Choose the correct equilibrium expression for each of the following heterogeneous equilibriums: a. O₂(g) + C(s) ⇒ CO₂ (g) [CO₂] OK= [0₂][C] OK = [CO₂][0₂] [CO₂] OK= [C] [CO₂] [0₂] b. Fe(s) + H₂O(g) ⇒ FeO(s) + H₂ (9) [H₂] OK= [H₂ O] [FeO] OK= OK= OK= Ok= [H₂O] [FeO] c. 4B(s) + 30₂ (g) ⇒ 2B2O3 (s) 1 OK= OK= [Fe] [H₂O] [H₂] [0₂]³ 1 [0₂] OK= = [0₂] OK= 4 [0₂]³[B]¹ [B₂03]²

Choose the correct equilibrium expression for each of the following heterogeneous equilibriums: a. O₂(g) + C(s) ⇒ CO₂ (g) [CO₂] OK= [0₂][C] OK = [CO₂][0₂] [CO₂] OK= [C] [CO₂] [0₂] b. Fe(s) + H₂O(g) ⇒ FeO(s) + H₂ (9) [H₂] OK= [H₂ O] [FeO] OK= OK= OK= Ok= [H₂O] [FeO] c. 4B(s) + 30₂ (g) ⇒ 2B2O3 (s) 1 OK= OK= [Fe] [H₂O] [H₂] [0₂]³ 1 [0₂] OK= = [0₂] OK= 4 [0₂]³[B]¹ [B₂03]²

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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Choose the correct equilibrium expression for each of the following heterogeneous equilibriums: a. O₂(g) + C(s) ⇒ CO₂(g) OK= OK = OK= OK= b. Fe(s) + H₂O(g) ⇒ FeO(s) + H₂(g) [H₂] OK= [H₂O] [FeO] OK= Ok = OK= OK= OK= [CO₂] [0₂][C] [CO₂][0₂] [CO₂] [C] [CO₂] [0₂] c. 4B(s) +30₂(g) — 2B2O3(s) 1 OK= [0₂] ³ = OK= [H₂O] [FeO] [Fe] [H₂O] [H₂] [0₂] [0₂] [0₂] ³ [B]¹4 [B₂O3]²
Transcribed Image Text:Choose the correct equilibrium expression for each of the following heterogeneous equilibriums: a. O₂(g) + C(s) ⇒ CO₂(g) OK= OK = OK= OK= b. Fe(s) + H₂O(g) ⇒ FeO(s) + H₂(g) [H₂] OK= [H₂O] [FeO] OK= Ok = OK= OK= OK= [CO₂] [0₂][C] [CO₂][0₂] [CO₂] [C] [CO₂] [0₂] c. 4B(s) +30₂(g) — 2B2O3(s) 1 OK= [0₂] ³ = OK= [H₂O] [FeO] [Fe] [H₂O] [H₂] [0₂] [0₂] [0₂] ³ [B]¹4 [B₂O3]²
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Introduction

Equilibrium expression is a mathematical representation of the balance between reactants and products in a chemical reaction. It expresses the relationship between the concentrations (or partial pressures) of the reactants and products at equilibrium. The expression is derived from the balanced chemical equation for the reaction, with each species raised to a power equal to its stoichiometric coefficient. The equilibrium constant, K, is the numerical value of the equilibrium expression at a given temperature and pressure. It provides information about the position and extent of the reaction at equilibrium.

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