3) Which of following represents the equilibrium constant for the reaction: 2 Hg (g) + Oz (g) +→ 2 HgO (s)? a. K = [Hg]*[Oz] b. K = #9*l0;] [Hg0]? %3D c. K = Hgo)? d. K =
3) Which of following represents the equilibrium constant for the reaction: 2 Hg (g) + Oz (g) +→ 2 HgO (s)? a. K = [Hg]*[Oz] b. K = #9*l0;] [Hg0]? %3D c. K = Hgo)? d. K =
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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Question
![**Equilibrium Constant for a Chemical Reaction**
**Question 3:**
Which of the following represents the equilibrium constant for the reaction:
\[ 2 \text{Hg (g)} + \text{O}_2 \text{(g)} \leftrightarrow 2 \text{HgO (s)} \]?
**Options:**
a. \[ K = [\text{Hg}]^2[\text{O}_2] \]
b. \[ K = \frac{[\text{Hg}]^2[\text{O}_2]}{[\text{HgO}]^2} \]
c. \[ K = \frac{[\text{HgO}]^2}{[\text{Hg}]^2[\text{O}_2]} \]
d. \[ K = \frac{1}{[\text{Hg}]^2[\text{O}_2]} \]
**Explanation:**
- The equilibrium constant, \( K \), for a reaction is expressed in terms of the concentrations (or pressures) of the products divided by the concentrations (or pressures) of the reactants, each raised to the power of their respective coefficients in the balanced equation.
- Solids and pure liquids do not appear in the expression for \( K \).
In this reaction, \(\text{HgO (s)}\) is a solid, so it is not included in the equilibrium expression. Therefore, the correct representation for the equilibrium constant is given by option **d**.
\[ K = \frac{1}{[\text{Hg}]^2[\text{O}_2]} \]
This expression considers only the concentrations of the gaseous reactants, \([\text{Hg}]\) and \([\text{O}_2]\), with their respective stoichiometric coefficients.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F07d00ca0-0430-458f-a009-3ccbf8c49c5a%2F04a7b505-96f6-49c9-80b8-5cbf1552b81d%2Fx2q7hzn_processed.png&w=3840&q=75)
Transcribed Image Text:**Equilibrium Constant for a Chemical Reaction**
**Question 3:**
Which of the following represents the equilibrium constant for the reaction:
\[ 2 \text{Hg (g)} + \text{O}_2 \text{(g)} \leftrightarrow 2 \text{HgO (s)} \]?
**Options:**
a. \[ K = [\text{Hg}]^2[\text{O}_2] \]
b. \[ K = \frac{[\text{Hg}]^2[\text{O}_2]}{[\text{HgO}]^2} \]
c. \[ K = \frac{[\text{HgO}]^2}{[\text{Hg}]^2[\text{O}_2]} \]
d. \[ K = \frac{1}{[\text{Hg}]^2[\text{O}_2]} \]
**Explanation:**
- The equilibrium constant, \( K \), for a reaction is expressed in terms of the concentrations (or pressures) of the products divided by the concentrations (or pressures) of the reactants, each raised to the power of their respective coefficients in the balanced equation.
- Solids and pure liquids do not appear in the expression for \( K \).
In this reaction, \(\text{HgO (s)}\) is a solid, so it is not included in the equilibrium expression. Therefore, the correct representation for the equilibrium constant is given by option **d**.
\[ K = \frac{1}{[\text{Hg}]^2[\text{O}_2]} \]
This expression considers only the concentrations of the gaseous reactants, \([\text{Hg}]\) and \([\text{O}_2]\), with their respective stoichiometric coefficients.
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