The following reaction was performed in a sealed vessel at 793 °C: H₂(g) + I2(g) 2HI(g) Initially, only H₂ and I were present at concentrations of [H₂] =3.05M and [1₂] =2.10M. The equilibrium concentration of I₂ is 0.0100 M. What is the equilibrium constant, Ke, for the reaction at this temperature? Express your answer numerically. ▸ View Available Hint(s) Ke= 5 ΑΣΦ www ? L
The following reaction was performed in a sealed vessel at 793 °C: H₂(g) + I2(g) 2HI(g) Initially, only H₂ and I were present at concentrations of [H₂] =3.05M and [1₂] =2.10M. The equilibrium concentration of I₂ is 0.0100 M. What is the equilibrium constant, Ke, for the reaction at this temperature? Express your answer numerically. ▸ View Available Hint(s) Ke= 5 ΑΣΦ www ? L
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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Solve both as they are subparts and get like.
Hand written solutions are strictly prohibited.
![reaction. The standard state of a pure substance is the pure
substance itself, and although the quantity may change the sample
remain pure. The constant value is incorporated into the value of
K, and does not need to be accounted for separately.
Deriving concentrations from data
In Part A, you were given the equilibrium pressures, which could be plugged directly into the formula for K. In Part B however, you will be given initial
concentrations and only one equilibrium concentration. You must use this data to find all three equilibrium concentrations before you can apply the formula for K.
▾ Part B
The following reaction was performed in a sealed vessel at 793 °C:
H₂(g) + I2(g) 2HI(g)
Initially, only H₂ and I₂ were present at concentrations of [H₂] = 3.05M and [1₂] =2.10M. The equilibrium concentration of I₂ is 0.0100 M. What is the
equilibrium constant, Ke, for the reaction at this temperature?
Express your answer numerically.
▸ View Available Hint(s)
Ke=
Submit
[7] ΑΣΦ/
Provide Feedback
6
?
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Next >](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F35862325-ca63-40be-a5be-4ed6b9a19979%2Fd0c74775-cc36-4ab2-b99d-d2e48c3f8e07%2Fjgdvqpa_processed.jpeg&w=3840&q=75)
Transcribed Image Text:reaction. The standard state of a pure substance is the pure
substance itself, and although the quantity may change the sample
remain pure. The constant value is incorporated into the value of
K, and does not need to be accounted for separately.
Deriving concentrations from data
In Part A, you were given the equilibrium pressures, which could be plugged directly into the formula for K. In Part B however, you will be given initial
concentrations and only one equilibrium concentration. You must use this data to find all three equilibrium concentrations before you can apply the formula for K.
▾ Part B
The following reaction was performed in a sealed vessel at 793 °C:
H₂(g) + I2(g) 2HI(g)
Initially, only H₂ and I₂ were present at concentrations of [H₂] = 3.05M and [1₂] =2.10M. The equilibrium concentration of I₂ is 0.0100 M. What is the
equilibrium constant, Ke, for the reaction at this temperature?
Express your answer numerically.
▸ View Available Hint(s)
Ke=
Submit
[7] ΑΣΦ/
Provide Feedback
6
?
Copyright © 2022 Doarcer Educ ion Inc. All rights
All rights recopied | Tor
Privacy Policy | Dermissions Contact Us L
Next >
![<HW 1 - Equilibrium
+ Calculating Equilibrium Constants
The equilibrium constant, K, of a reaction at a particular
temperature is determined by the concentrations or pressures of the
reactants and products at equilibrium.
For a gaseous reaction with the general form
aA + bB cC + dD
the Ke and Kp expressions are given by
[CD]d
[A]ª[B]b
Ke
Kc =
Kp =
(Pc)(Pb)
(PA)" (P)
The subscript c or p indicates whether K is expressed in terms of
concentrations or pressures. Equilibrium-constant expressions do
not include a term for any pure solids or liquids that may be
involved since their composition does not change throughout the
reaction. The standard state of a pure substance is the pure
substance itself, and although the quantity may change the sample
remain pure. The constant value is incorporated into the value of
K, and does not need to be accounted for separately.
Review | Constants | Periodic Table
Phosgene (carbonyl chloride), COC1₂, is an extremely toxic gas that is used in manufacturing certain dyes and plastics. Phosgene can be produced by reacting
carbon monoxide and chlorine gas at high temperatures:
CO(g) + Cl₂(g) = COC12(g)
Carbon monoxide and chlorine gas are allowed to react in a sealed vessel at 454 °C. At equilibrium, the concentrations were measured and the following
results obtained:
What is the equilibrium constant, Kp, of this reaction?
Express your answer numerically.
► View Available Hint(s)
Kp =
Submit
IVE ΑΣΦ 4
?
Gas
6 of 17
CO
Cl₂
COC,
Partial Pressure
(atm)
0.740
1.29
0.190
H
Deriving concentrations from data
In Part A, you were given the equilibrium pressures, which could be plugged directly into the formula for K. In Part B however, you will be given initial
concentrations and only one equilibrium concentration. You must use this data to find all three equilibrium concentrations before you can apply the formula for K.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F35862325-ca63-40be-a5be-4ed6b9a19979%2Fd0c74775-cc36-4ab2-b99d-d2e48c3f8e07%2F7srhod_processed.jpeg&w=3840&q=75)
Transcribed Image Text:<HW 1 - Equilibrium
+ Calculating Equilibrium Constants
The equilibrium constant, K, of a reaction at a particular
temperature is determined by the concentrations or pressures of the
reactants and products at equilibrium.
For a gaseous reaction with the general form
aA + bB cC + dD
the Ke and Kp expressions are given by
[CD]d
[A]ª[B]b
Ke
Kc =
Kp =
(Pc)(Pb)
(PA)" (P)
The subscript c or p indicates whether K is expressed in terms of
concentrations or pressures. Equilibrium-constant expressions do
not include a term for any pure solids or liquids that may be
involved since their composition does not change throughout the
reaction. The standard state of a pure substance is the pure
substance itself, and although the quantity may change the sample
remain pure. The constant value is incorporated into the value of
K, and does not need to be accounted for separately.
Review | Constants | Periodic Table
Phosgene (carbonyl chloride), COC1₂, is an extremely toxic gas that is used in manufacturing certain dyes and plastics. Phosgene can be produced by reacting
carbon monoxide and chlorine gas at high temperatures:
CO(g) + Cl₂(g) = COC12(g)
Carbon monoxide and chlorine gas are allowed to react in a sealed vessel at 454 °C. At equilibrium, the concentrations were measured and the following
results obtained:
What is the equilibrium constant, Kp, of this reaction?
Express your answer numerically.
► View Available Hint(s)
Kp =
Submit
IVE ΑΣΦ 4
?
Gas
6 of 17
CO
Cl₂
COC,
Partial Pressure
(atm)
0.740
1.29
0.190
H
Deriving concentrations from data
In Part A, you were given the equilibrium pressures, which could be plugged directly into the formula for K. In Part B however, you will be given initial
concentrations and only one equilibrium concentration. You must use this data to find all three equilibrium concentrations before you can apply the formula for K.
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