menu
bartleby
search
close search
Hit Return to see all results
close solutoin list

A sample of iron(II) sulfate was heated in an evacuated container to 920 K, where the following reactions occurred: 2 FeSO 4 ( s ) ⇌ Fe 2 O 3 ( s ) + SO 3 ( g ) + SO 2 ( g ) SO 3 ( g ) ⇌ SO 2 ( g ) + 1 2 O 2 ( g ) After equilibrium was reached, the total pressure was 0.836 atm and the partial pressure of oxygen was 0.0275 atm. Calculate K p for each of these reactions.

BuyFindarrow_forward

Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

Solutions

Chapter
Section
BuyFindarrow_forward

Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 12, Problem 110CP
Textbook Problem
24 views

A sample of iron(II) sulfate was heated in an evacuated container to 920 K, where the following reactions occurred:

2 FeSO 4 ( s ) Fe 2 O 3 ( s ) + SO 3 ( g ) + SO 2 ( g ) SO 3 ( g ) SO 2 ( g ) + 1 2 O 2 ( g )

After equilibrium was reached, the total pressure was 0.836 atm and the partial pressure of oxygen was 0.0275 atm. Calculate Kp for each of these reactions.

Interpretation Introduction

Interpretation: The equilibrium constants for the given reactions are to be calculated.

Concept introduction: The equilibrium constant Kp describes the ratio of the reactant to the product on the equilibrium conditions in terms of the partial pressure.

Partial pressure of a gas is defined as the pressure applied by the each gas to the surroundings.

The equilibrium constant depends upon temperature.

At equilibrium sum of all the partial pressure is equal to the total pressure.

Law of mass action is applicable on the equilibrium reactions.

Law of mass action states that at a given temperature the equilibrium constant is equal to the partial pressure of the products to the reactants raised the power of stoichiometric coefficient.

To determine: The equilibrium constants for the given reactions.

Explanation of Solution

Explanation

Given

The first reaction is given as,

2FeSO4(s)Fe2O3(s)+SO3(g)+SO2(g)

In this reaction equal amounts of SO3 and SO2 are produced.

The second reaction is given as’

SO3(g)SO2(g)+12O2(g)

Partial pressure of O2=0.0275atm

In order to solve the equilibrium constant (ICE-chart) that is the initial pressure, change in pressure and equilibrium pressure is determined.

The initial partial pressure is supposed to be P0 and the change in partial pressure is x . The ICE table for the given reaction is,

SO3(g)SO2(g)1/2O2(g)InitialP0P0P0Changex+x+x/2EquilibriumP0xP0+xx/2

At equilibrium the partial pressure is equal to the sum of the individual pressure of the all gases. Therefore,

Ptotal=Ppartial

Where,

  • Ptotal is the total pressure at equilibrium.
  • Ppartial is the partial pressure of the gases.
  • represents the sum of all partial pressures.

Substitute the given value of total pressure and value of partial pressure of all gases from the ICE-chart.

Ptotal=Ppartial0.836atm=P0+x+P0+x+x/20.836atm=2P0+x/2 (1)

At equilibrium the given partial pressure of O2=0.0275atm .

Therefore, from the ICE table the value of x calculated as,

PO2=x/20.0275atm=x/2x=0.0550atm

Substitute the value of x in equation (1).

0.836atm=2P0+x/20.836atm=2P0+0.0550atm2P0=0.405atm

Therefore, from the ICE table the partial pressure of SO2 and SO3 is as follows,

PSO2=P0x=0.4050.0550=0.350atm_

PSO3=P0+x=0

Still sussing out bartleby?

Check out a sample textbook solution.

See a sample solution

The Solution to Your Study Problems

Bartleby provides explanations to thousands of textbook problems written by our experts, many with advanced degrees!

Get Started

Chapter 12 Solutions

Chemistry: An Atoms First Approach
Show all chapter solutions
add
Ch. 12 - Consider an equilibrium mixture of four chemicals...Ch. 12 - The boxes shown below represent a set of initial...Ch. 12 - For the reactionH2(g)+I2(g)2HI(g), consider two...Ch. 12 - Given the reactionA(g)+B(g)C(g)+D(g), consider the...Ch. 12 - Consider the reaction A(g)+2B(g)C(g)+D(g) in a...Ch. 12 - Consider the reactionA(g)+B(g)C(g)+D(g). A friend...Ch. 12 - Consider the following statements: Consider the...Ch. 12 - Le Chteliers principle is stated (Section 12-7) as...Ch. 12 - The value of the equilibrium constant K depends on...Ch. 12 - Consider an initial mixture of N2 and H2 gases...Ch. 12 - Consider the following reaction:...Ch. 12 - Consider the same reaction as in Question 11. In...Ch. 12 - Suppose a reaction has the equilibrium constant K...Ch. 12 - Suppose a reaction has the equilibrium constant K...Ch. 12 - Consider the following reaction at some...Ch. 12 - Consider the following generic reaction:...Ch. 12 - Explain the difference between K, Kp, and Q.Ch. 12 - Consider the following reactions:...Ch. 12 - For a typical equilibrium problem, the value of K...Ch. 12 - Which of the following statements is(are) true?...Ch. 12 - Write the equilibrium expression (K) for each of...Ch. 12 - Write the equilibrium expression (Kp) for each...Ch. 12 - At a given temperature, K = 1.3 102 for the...Ch. 12 - For the reaction H2(g)+Br2(g)2HBr(g) Kp = 3.5 104...Ch. 12 - For the reaction 2NO(g)+2H2(g)N2(g)+2H2O(g) it is...Ch. 12 - At high temperatures, elemental nitrogen and...Ch. 12 - At a particular temperature, a 3.0-L flask...Ch. 12 - At a particular temperature a 2.00-L flask at...Ch. 12 - The following equilibrium pressures at a certain...Ch. 12 - The following equilibrium pressures were observed...Ch. 12 - At 327c, the equilibrium concentrations are...Ch. 12 - At 1100 K, Kp = 0.25 for the reaction...Ch. 12 - Write expressions for K and Kp for the following...Ch. 12 - Write expressions for Kp for the following...Ch. 12 - For which reactions in Exercise 33 is Kp equal to...Ch. 12 - For which reactions in Exercise 34 is Kp equal to...Ch. 12 - Consider the following reaction at a certain...Ch. 12 - In a study of the reaction...Ch. 12 - The equilibrium constant is 0.0900 at 25C for the...Ch. 12 - The equilibrium constant is 0.0900 at 25C for the...Ch. 12 - At 900c, Kp = 1.04 for the reaction...Ch. 12 - Ethyl acetate is synthesized in a nonreacting...Ch. 12 - For the reaction 2H2O(g)2H2(g)+O2(g) K = 2.4 103...Ch. 12 - The reaction 2NO(g)+Br2(g)2NOBr(g) has Kp = 109 at...Ch. 12 - A 1.00-L flask was filled with 2.00 moles of...Ch. 12 - A sample of S8(g) is placed in an otherwise empty...Ch. 12 - At a particular temperature, 12.0 moles of SO3 is...Ch. 12 - At a particular temperature, 8.0 moles of NO2 is...Ch. 12 - An initial mixture of nitrogen gas and hydrogen...Ch. 12 - Nitrogen gas (N2) reacts with hydrogen gas (H2) to...Ch. 12 - At a particular temperature, K = 3.75 for the...Ch. 12 - At a particular temperature, K = 1.00 102 for the...Ch. 12 - At 2200C, Kp = 0.050 for the reaction...Ch. 12 - At 25c, K = 0.090 for the reaction...Ch. 12 - At 1100 K, KP = 0.25 for the reaction...Ch. 12 - At a particular temperature, Kp = 0.25 for the...Ch. 12 - At 35C, K = 1.6 105 for the reaction...Ch. 12 - At o particular temperature, K = 4 .0 107 for the...Ch. 12 - At a particular temperature, K = 2.0 106 for the...Ch. 12 - Lexan is a plastic used to make compact discs,...Ch. 12 - At 25C, Kp. = 2.9 103 for the reaction...Ch. 12 - A sample of solid ammonium chloride was placed in...Ch. 12 - Suppose the reaction system...Ch. 12 - Predict the shift in the equilibrium position that...Ch. 12 - An important reaction in the commercial production...Ch. 12 - What will happen to the number of moles of SO3 in...Ch. 12 - In which direction will the position of the...Ch. 12 - Hydrogen for use in ammonia production is produced...Ch. 12 - Old-fashioned smelling salts consist of ammonium...Ch. 12 - Ammonia is produced by the Haber process, in which...Ch. 12 - Calculate a value for the equilibrium constant for...Ch. 12 - Given the following equilibrium constants at...Ch. 12 - Consider the decomposition of the compound C5H6O3...Ch. 12 - At 25C. Kp 1 1031 for the reaction a. Calculate...Ch. 12 - The gas arsine, AsH3, decomposes as follows:...Ch. 12 - At a certain temperature, K = 9.1 10-4 for the...Ch. 12 - At a certain temperature, K = 1.1 l03 for the...Ch. 12 - For the reaction PCl5(g)PCl3(g)+Cl2(g) at 600. K,...Ch. 12 - At 25C, gaseous SO2Cl2 decomposes to SO2(g) and...Ch. 12 - For the following reaction at a certain...Ch. 12 - Novelty devices for predicting rain contain...Ch. 12 - Consider the reaction Fe3+(aq)+SCN(aq)FeSCN2+(aq)...Ch. 12 - Chromium(VI) forms two different oxyanions, the...Ch. 12 - The synthesis of ammonia gas from nitrogen gas and...Ch. 12 - Suppose K = 4.5 103 at a certain temperature for...Ch. 12 - For the reaction below, Kp = 1.16 at 800C....Ch. 12 - Many sugars undergo a process called mutarotation,...Ch. 12 - Peptide decomposition is one of the key processes...Ch. 12 - The creation of shells by mollusk species is a...Ch. 12 - Methanol, a common laboratory solvent, poses a...Ch. 12 - For the reaction: 3O2(g)2O3(g) K = 1.8 107 at a...Ch. 12 - An equilibrium mixture contains 0.60 g solid...Ch. 12 - At a particular temperature, 8.1 moles of NO2 gas...Ch. 12 - A sample of solid ammonium chloride was placed in...Ch. 12 - In a given experiment, 5.2 moles of pure NOCl was...Ch. 12 - For the reactionN2O4(g)2NO2(g),Kp=0.25 at a...Ch. 12 - Consider the following exothermic reaction at...Ch. 12 - For the following endothermic reaction at...Ch. 12 - A 1.604-g sample of methane (CH4) gas and 6.400 g...Ch. 12 - A 4.72-g sample of methanol (CH3OH) was placed in...Ch. 12 - At 35C, K = 1.6 105 for the reaction...Ch. 12 - Nitric oxide and bromine at initial partial...Ch. 12 - At 25C. Kp = 5.3 105 for the reaction...Ch. 12 - Consider the reaction P4(g)2P2(g) where Kp = 1.00 ...Ch. 12 - The partial pressures of an equilibrium mixture of...Ch. 12 - At 125C, KP = 0.25 for the reaction...Ch. 12 - A mixture of N2, H2, and NH3 is at equilibrium...Ch. 12 - Consider the decomposition equilibrium for...Ch. 12 - An 8.00-g sample of SO3 was placed in an evacuated...Ch. 12 - A sample of iron(II) sulfate was heated in an...Ch. 12 - At 5000 K and 1.000 atm, 83.00% of the oxygen...Ch. 12 - A sample of N2O4(g) is placed in an empty cylinder...Ch. 12 - A sample of gaseous nitrosyl bromide (NOBr) was...Ch. 12 - The equilibrium constant Kp for the reaction...Ch. 12 - For the reaction NH3(g)+H2S(g)NH4HS(s) K = 400. at...Ch. 12 - Given K = 3.50 at 45C for the reaction...Ch. 12 - In a solution with carbon tetrachloride as the...Ch. 12 - The hydrocarbon naphthalene was frequently used in...Ch. 12 - A gaseous material XY(g) dissociates to some...

Additional Science Textbook Solutions

Find more solutions based on key concepts
Show solutions add
Vitamin E is famous for its role: a. in maintaining bone tissue integrity. b. in maintaining connective tissue ...

Nutrition: Concepts and Controversies - Standalone book (MindTap Course List)

One yard is slightly ___ than 1 meter. (1.4)

An Introduction to Physical Science

6.43 Define the term spin paired.

Chemistry for Engineering Students

How does hydrostatic equilibrium relate to hot-air ballooning?

Horizons: Exploring the Universe (MindTap Course List)

List the differences between mitosis and meiosis in the following chart:

Human Heredity: Principles and Issues (MindTap Course List)

25. Name each compound:

Chemistry In Focus

How do you think oxygen reaches the deep ocean for use by the animals living there?

Oceanography: An Invitation To Marine Science, Loose-leaf Versin

At the Earths surface, a projectile is launched straight up at a speed of 10.0 km/s. To what height will it ris...

Physics for Scientists and Engineers, Technology Update (No access codes included)