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
Chapter8: Reaction Rates And Equilibrium
Section: Chapter Questions
Problem 8.55E
Related questions
Question
![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](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb7f470a0-93f2-43bf-9ed3-2f125d19f075%2F419d1058-22d6-454e-9bb2-29ffa150b037%2Fdoidwq_processed.png&w=3840&q=75)
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
Expert Solution
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Step 1
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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