(a)
Interpretation:
The equilibrium expression for the given gaseous reaction is to be stated.
Concept Introduction:
The equilibrium constant of a reaction is expressed as the ratio of concentration of products and reactants each raised to the power of their
The equilibrium constant for the above
Where,
•
•
•
•
•
•
•
•
Answer to Problem 8.40E
The equilibrium constant for the given gaseous reaction is expressed as,
Explanation of Solution
The given gaseous reaction is represented as,
The concentration of the product
Therefore, the equilibrium constant for the above gaseous reaction is expressed as,
The equilibrium constant for the given gaseous reaction is expressed as,
(b)
Interpretation:
The equilibrium expression for the given gaseous reaction is to be stated.
Concept Introduction:
The equilibrium constant of a reaction is expressed as the ratio of concentration of products and reactants each raised to the power of their stoichiometric coefficients. A general equilibrium reaction is represented as,
The equilibrium constant for the above chemical reaction is expressed as,
Where,
•
•
•
•
•
•
•
•
Answer to Problem 8.40E
The equilibrium constant for the given gaseous reaction is expressed as,
Explanation of Solution
The given gaseous reaction is represented as,
The concentration of the product
Therefore, the equilibrium constant for the above gaseous reaction is expressed as,
The equilibrium constant for the given gaseous reaction is expressed as,
(c)
Interpretation:
The equilibrium expression for the given gaseous reaction is to be stated.
Concept Introduction:
The equilibrium constant of a reaction is expressed as the ratio of concentration of products and reactants each raised to the power of their stoichiometric coefficients. A general equilibrium reaction is represented as,
The equilibrium constant for the above chemical reaction is expressed as,
Where,
•
•
•
•
•
•
•
•
Answer to Problem 8.40E
The equilibrium constant for the given gaseous reaction is expressed as,
Explanation of Solution
The given gaseous reaction is represented as,
The concentration of the product
Therefore, the equilibrium constant for the above gaseous reaction is expressed as,
The equilibrium constant for the given gaseous reaction is expressed as,
(d)
Interpretation:
The equilibrium expression for the given gaseous reaction is to be stated.
Concept Introduction:
The equilibrium constant of a reaction is expressed as the ratio of concentration of products and reactants each raised to the power of their stoichiometric coefficients. A general equilibrium reaction is represented as,
The equilibrium constant for the above chemical reaction is expressed as,
Where,
•
•
•
•
•
•
•
•
Answer to Problem 8.40E
The equilibrium constant for the given gaseous reaction is expressed as,
Explanation of Solution
The given gaseous reaction is represented as,
The concentration of the product
Therefore, the equilibrium constant for the above gaseous reaction is expressed as,
The equilibrium constant for the given gaseous reaction is expressed as,
(e)
Interpretation:
The equilibrium expression for the given gaseous reaction is to be stated.
Concept Introduction:
The equilibrium constant of a reaction is expressed as the ratio of concentration of products and reactants each raised to the power of their stoichiometric coefficients. A general equilibrium reaction is represented as,
The equilibrium constant for the above chemical reaction is expressed as,
Where,
•
•
•
•
•
•
•
•
Answer to Problem 8.40E
The equilibrium constant for the given gaseous reaction is expressed as,
Explanation of Solution
The given gaseous reaction is represented as,
The concentration of the product
Therefore, the equilibrium constant for the above gaseous reaction is expressed as,
The equilibrium constant for the given gaseous reaction is expressed as,
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Chapter 8 Solutions
LMS Integrated OWLv2, 4 terms (24 months) Printed Access Card for Seager/Slabaugh/Hansen’s Chemistry for Today: General, Organic, and Biochemistry, 9th
- Consider the system SO3(g)SO2(g)+12 O2(g)H=98.9kJ (a) Predict whether the forward or reverse reaction will occur when the equilibrium is disturbed by 1. adding oxygen gas. 2. compressing the system at constant temperature. 3. adding argon gas. 4. removing SO2(g). 5. decreasing the temperature. (b) Which of the above factors will increase the value of K? Which will decrease it?arrow_forwardA mixture of SO2, O2, and SO3 at 1000 K contains the gases at the following concentrations: [SO2] = 5.0 103 mol/L, [O2] = 1.9 103 mol/L, and [SO3] = 6.9 103 mol/L. Is the reaction at equilibrium? If not, which way will the reaction proceed to reach equilibrium? 2 SO2(g) + O2(g) 2 SO3(g) Kc = 279arrow_forwardConsider the following generic reaction: 2A2B(g)2A2(g)+B2(g) Some molecules of A2B are placed in a 1.0-L container. As time passes, several snapshots of the reaction mixture are taken as illustrated below. Which illustration is the first to represent an equilibrium mixture? Explain. How many molecules of A2B reacted initially?arrow_forward
- A mixture of N2, H2, and NH3 is at equilibrium [according to the equationN2(g)+3H2(g)2NH3(g)] as depicted below: The volume is suddenly decreased (by increasing the external pressure) and a new equilibrium is established as depicted below: a. If the volume of the final equilibrium mixture is 1.00 L, determine the value of the equilibrium constant, K. for the reaction. Assume temperature is constant. b. Determine the volume of the initial equilibrium mixture assuming a final equilibrium volume of 1.00 L and assuming a constant temperature.arrow_forwardConsider the system 4 NH3(g) + 3 O2(g) ⇌ 2 N2(g) + 6 H20(ℓ) ΔrH° = −1530.4 kJ/mol How will the amount of ammonia at equilibrium be affected by removing O2(g) without changing the total gas volume? adding N2(g) without changing the total gas volume? adding water without changing the total gas volume? expanding the container? increasing the temperature? Which of these changes (i to v) increases the value of K? Which decreases it?arrow_forwardDecomposition of ammonium dichromate is shown in the designated series of photos. In a closed container this process reaches an equilibrium state. Write a balanced chemical equation for the equilibrium reaction. How is the equilibrium affected if more ammonium dichromate is added to the equilibrium system? more water vapor is added? more chromium(III) oxide is added? Decomposition of ammonium dichromate, for Question 4. Decomposition of (NH4)2Cr2O7. Orange, solid (NH4)2Cr2O7 (a) can be ignited by lighting a wick (b), which initiates decomposition (c) forming Cr2O3, the dark green solid in part (d), N2 gas, and water vapor. Energy is transferred to the surroundings by the process.arrow_forward
- What is Le Chteliers principle? Consider the reaction 2NOCI(g)2NO(g)+Cl2(g) If this reaction is at equilibrium. what happens when the following changes occur? a. NOCI(g) is added. b. NO(g) is added. c. NOCI(g) is removed. d. Cl2(g) is removed. e. The container volume is decreased. For each of these changes, what happens to the value of K for the reaction as equilibrium is reached again? Give an example of a reaction for which the addition or removal of one of the reactants or products has no effect on the equilibrium position. In general, how will the equilibrium position of a gas-phase reaction be affected if the volume of the reaction vessel changes? Are there reactions that will not have their equilibria shifted by a change in volume? Explain. Why does changing the pressure in a rigid container by adding an inert gas not shift the equilibrium position for a gas-phase reaction?arrow_forwardHydrogen and carbon dioxide react at a high temperature to give water and carbon monoxide. H2(g) + CO2(g) H2O(g) + CO(g) (a) Laboratory measurements at 986 C show that there are 0.11 mol each of CO and H2O vapor and 0.087 mol each of H2 and CO2 at equilibrium in a 50.0-L container. Calculate the equilibrium constant for the reaction at 986 C. (b) Suppose 0.010 mol each of H2 and CO2 are placed in a 200.0-L container. When equilibrium is achieved at 986 C, what amounts of CO(g) and H2O(g), in moles, would be present? [Use the value of Kc from part (a).]arrow_forwardWrite equilibrium expressions for each of the following equilibria. 2 C(s) + O2(g) «=* 2 CO(g) Zn (aq) + H2S(g) *=* ZnS(s) + 2 H (aq) HCl(g) + H2O(€) 5=i H,O+(aq) + Cl"(aq) (d) H2(g) + | O2(g) s=s H2O(g)arrow_forward
- Write an equilibrium expression for each of the following gaseous reactions: a.3O22O3 b.COCl2CO+Cl2 c.CS2+4H2CH4+2H2S d.2SO2+O22SO3 e.CO+H2OCO2+H2arrow_forwardLexan is a plastic used to make compact discs, eyeglass lenses, and bulletproof glass. One of the compounds used to make Lexan is phosgene (COCI2), an extremely poisonous gas. Phosgene decomposes by the reaction COCl2(g)CO(g)+Cl2(g) for which KP = 6.8 109 at 100C. If pure phosgene at an initial pressure of 1.0 atm decomposes, calculate the equilibrium pressures of all species.arrow_forwardConsider the following equilibrium: COBr2(g) CO(g) + Br2(g)Kc = 0.190 at 73 C (a) A 0.50 mol sample of COBr2 is transferred to a 9.50-L flask and heated until equilibrium is attained. Calculate the equilibrium concentrations of each species. (b) The volume of the container is decreased to 4.5 L and the system allowed to return to equilibrium. Calculate the new equilibrium concentrations. (Hint: The calculation will be easier if you view this as a new problem with 0.5 mol of COBr2 transferred to a 4.5-L flask.) (c) What is the effect of decreasing the container volume from 9.50 L to 4.50 L?arrow_forward
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