(a)
Interpretation:
The direction of the equilibrium shift in the given equilibrium is to be predicted.
Concept introduction:
The equilibrium constant is a parameter which describes the relationship between concentration of the reactants and the products at equilibrium stage. Equilibrium constant of a reaction is expressed by the ratio of concentration of product species raised to the power of their
Answer to Problem 8.58E
The shift in the equilibrium will be towards the right direction.
Explanation of Solution
According to the Le Chȃtelier’s principle the change in concentration, volume, pressure and temperature affects the equilibrium of the reaction.
The given equilibrium reaction is shown below.
It is considered that when some amount of
The shift in the equilibrium will be towards the right direction.
(b)
Interpretation:
The direction of the equilibrium shift in the given equilibrium is to be predicted.
Concept introduction:
The equilibrium constant is a parameter which describes the relationship between concentration of the reactants and the products at equilibrium stage. Equilibrium constant of a reaction is expressed by the ratio of concentration of product species raised to the power of their stoichiometric coefficients to the concentration of reactant species raised to the power of their stoichiometric coefficients.
Answer to Problem 8.58E
The shift in the equilibrium will be towards the left direction.
Explanation of Solution
According to the Le Chȃtelier’s principle the change in concentration, volume, pressure and temperature affects the equilibrium of the reaction.
The given equilibrium reaction is shown below.
The given reaction is exothermic reaction. The reaction is at equilibrium when the heat is given out from the system. It is considered that the temperature of the system increases. Thus, the temperature of the system on the right hand side increases. Hence, according to the Le Chȃtelier’s principle, the equilibrium will shift towards left direction to compensate the increase in temperature.
The shift in the equilibrium will be towards the left direction.
(c)
Interpretation:
The direction of the equilibrium shift in the given equilibrium is to be predicted.
Concept introduction:
The equilibrium constant is a parameter which describes the relationship between concentration of the reactants and the products at equilibrium stage. Equilibrium constant of a reaction is expressed by the ratio of concentration of product species raised to the power of their stoichiometric coefficients to the concentration of reactant species raised to the power of their stoichiometric coefficients.
Answer to Problem 8.58E
The shift in the equilibrium will be towards the right direction.
Explanation of Solution
According to the Le Chȃtelier’s principle the change in concentration, volume, pressure and temperature affects the equilibrium of the reaction.
The given equilibrium reaction is shown below.
It is considered that when some amount of
The shift in the equilibrium will be towards the right direction.
(d)
Interpretation:
The direction of the equilibrium shift in the given equilibrium is to be predicted.
Concept introduction:
The equilibrium constant is a parameter which describes the relationship between concentration of the reactants and the products at equilibrium stage. Equilibrium constant of a reaction is expressed by the ratio of concentration of product species raised to the power of their stoichiometric coefficients to the concentration of reactant species raised to the power of their stoichiometric coefficients.
Answer to Problem 8.58E
The shift in the equilibrium will be towards the left direction.
Explanation of Solution
According to the Le Chȃtelier’s principle the change in concentration, volume, pressure and temperature affects the equilibrium of the reaction.
The given equilibrium reaction is shown below.
It is considered that when some amount of
The shift in the equilibrium will be towards the left direction.
(e)
Interpretation:
The direction of the equilibrium shift in the given equilibrium is to be predicted.
Concept introduction:
The equilibrium constant is a parameter which describes the relationship between concentration of the reactants and the products at equilibrium stage. Equilibrium constant of a reaction is expressed by the ratio of concentration of product species raised to the power of their stoichiometric coefficients to the concentration of reactant species raised to the power of their stoichiometric coefficients.
Answer to Problem 8.58E
The equilibrium does not shift on addition of a catalyst.
Explanation of Solution
According to the Le Chȃtelier’s principle the change in concentration, volume, pressure and temperature affects the equilibrium of the reaction.
The given equilibrium reaction is shown below.
It is considered that when a catalyst is added, it will only increase the
The equilibrium does not shift on addition of a catalyst.
(f)
Interpretation:
The direction of the equilibrium shift in the given equilibrium is to be predicted.
Concept introduction:
The equilibrium constant is a parameter which describes the relationship between concentration of the reactants and the products at equilibrium stage. Equilibrium constant of a reaction is expressed by the ratio of concentration of product species raised to the power of their stoichiometric coefficients to the concentration of reactant species raised to the power of their stoichiometric coefficients.
Answer to Problem 8.58E
The shift in the equilibrium will be towards the left direction.
Explanation of Solution
According to the Le Chȃtelier’s principle the change in concentration, volume, pressure and temperature affects the equilibrium of the reaction.
The given equilibrium reaction is shown below.
The given reaction is exothermic reaction. The reaction is at equilibrium when the heat is given out from the system. It is considered that the temperature of the system increases and some amount of
The shift in the equilibrium will be towards the left direction.
Want to see more full solutions like this?
Chapter 8 Solutions
Chemistry for Today: General, Organic, and Biochemistry
- Consider the following equilibria involving SO2(g) and their corresponding equilibrium constants. SO2(g) + |o2(g)^SO}(g) A, £ 2 SO,(g) «=* 2 SO,(g) + O,(g) A, Which of the following expressions relates A, to A2? A2 = A,2 A,2 = A, A2 = A, A2 = 1/A, A2 = 1/A,2arrow_forwardA necessary step in the manufacture of sulfuric acid is the formation of sulfur trioxide. SO3, from sulfur dioxide, SO2, and oxygen, O2, shown here. At high temperatures, the rate of formation of SO3 is higher, but the equilibrium amount (concentration or partial pressure) of SO3 is lower than it would be at lower temperatures. 2SO2(g)+O2(g)2SO3(g) (a) Does the equilibrium constant for the reaction increase, decrease, or remain about the same as the temperature increases? (b) Is the reaction endothermic or exothermic?arrow_forwardThe equilibrium constant is 0.0900 at 25C for the reaction H2O(g)+Cl2O(g)2HOCl(g) For which of the following sets of conditions is the system at equilibrium? For those that are not at equilibrium, in which direction will the system shift? a. PH2O=1.00atm,PCl2O=1.00atm,PHOCl=1.00atm b. PH2O=200.torr,PCl2O=49.8torr,PHOCl=21.0torr c. PH2O=296torr,PCl2O=15.0torr,PHOCl=20.0torrarrow_forward
- The equilibrium constant is 0.0900 at 25C for the reaction H2O(g)+Cl2O(g)2HOCl(g) For which of the following sets of conditions is the system at equilibrium? For those that are not at equilibrium, in which direction will the system shift? a.PH2O=1.00atm,PCI2O=1.00atm,PHOCI=1.00atm b.PH2O=200.torr,PCI2O=49.8torr,PHOCI=21.0torr c. PH2O=296torr,PCI2O=15.0torr,PHOCI=20.0torrarrow_forwardThe following reaction occurs when a burner on a gas stove is lit: CH4+2O2(g)CO2(g)+2H2O(g) Is an equilibrium among CH4, O2, CO2, and H2O established under these conditions? Explain your answer.arrow_forwardWater gas, a mixture of H2 and CO, is an important industrial fuel produced by the reaction of steam with red hot coke, essentially pure carbon. (a) Write the expression for the equilibrium constant for the reversible reaction C(s)+H2O(g)CO(g)+H2(g)H=131.30kJ (b) What will happen to the concentration of each reactant and product at equilibrium if more C is added? (c) What will happen to the concentration of each reactant and product at equilibrium if H2O is removed? (d) What will happen to the concentration of each reactant and product at equilibrium if CO is added? (e) What will happen to the concentration of each reactant and product at equilibrium if the temperature of the system is increased?arrow_forward
- Limestone decomposes at high temperatures. CaCO3(s) CaO(s) + CO2(g) At 1000 C, Kp = 3.87. If pure CaCO3 is placed in a 5.00-L flask and heated to 1000 C, what quantity of CaCO3 must decompose to achieve the equilibrium pressure of CO2?arrow_forwardDinitrogen trioxide decomposes to NO and NO2, in an endothermic process (rH = 40.5 kJ/mol-rxn). N2O3(g) NO(g) + NO2(g) Predict the effect of the following changes on the position of the equilibrium; that is, state which way the equilibrium will shift (left, right, or no change) when each of the following changes is made. (a) adding more N2O3(g) (b) adding more NO2(g) (c) increasing the volume of the reaction flask (d) lowering the temperaturearrow_forward. Consider the reaction 2CO(g)+O2(g)2CO2(g)Suppose the system is already at equilibrium, and then an additional mole of CO2(g) is injected into the system at constant temperature. Does the amount of O2(g) in the system increase or decrease? Does the value of K for the reaction change?arrow_forward
- Methanol, CH3OH, formerly known as wood alcohol, is manufactured commercially by the following reaction: CO(g)+2H2(g)CH3OH(g) A 1.500-L vessel was filled with 0.1500 mol CO and 0.3000 mol H2. When this mixture came to equilibrium at 500 K. the vessel contained 0.1187 mol CO. How many moles of each substance were in the vessel?arrow_forwardNitrogen and oxygen react at high temperatures. (a) Write the expression for the equilibrium constant (Kc) for the reversible reaction N2(g)+O2(g)2NO(g)H=181kJ (b) What will happen to the concentrations of N2, O2, and NO at equilibrium if more O2 is added? (c) What will happen to the concentrations of N2, O2, and NO at equilibrium if N2 is removed? (d) What will happen to the concentrations of N2, O2, and NO at equilibrium if NO is added? (e) What will happen to the concentrations of N2, O2, and NO at equilibrium if the pressure on the system is increased by reducing the volume of the reaction vessel? (f) What will happen to the concentrations of N2, O2, and NO at equilibrium if the temperature of the system is increased? (g) What will happen to the concentrations of N2, O2, and NO at equilibrium if a catalyst is added?arrow_forwardConsider the following reaction at some temperature: H2O(g)+CO(g)H2(g)+CO2(g)K=2.0 Some molecules of H2O and CO are placed in a 1.0-L container as shown below. When equilibrium is reached, bow many molecules of H2O, CO, H2, and CO2 are present? Do this problem by trial and error-that is, if two molecules of CO react, is this equilibrium; if three molecules of CO react, is this equilibrium; and so on.arrow_forward
- Introductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStax
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning