Enter your answer in the provided box.Gaseous ammonia was introduced into a sealed container and heated to a certain temperature:2 NH3(g) N2(g) + 3 H2(g)At equilibrium, [NH3] = 0.0232 M, [N2] = 0.119 M, and [H2] = 0.367 M.Calculate Ke for the reaction at this temperature.Kc=

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Introductory Chemistry: A Foundation

8th Edition

ISBN:9781285199030

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 34QAP

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Indicate whether or not product formation increases with increasing temperature in each of the following equilibrium systems. a. N2(g)+2O2(g)+heat2NO2(g) b. heat+2N2(g)+6H2O(g)4NH3(g)+3O2(g) c. C2H4(g)+3O2(g)2CO2(g)+2H2O(g)+heat d. 2KClO3(s)+heat2KCl(s)+3O2(g)
When a mixture of hydrogen and bromine is maintained at normal atmospheric pressure and heated above 200. °C in a closed container, the hydrogen and bromine react to form hydrogen bromide and a gas-phase equilibrium is established. Write a balanced chemical equation for the equilibrium reaction. Use bond enthalpies from Table 6.2 ( Sec. 6-6b) to estimate the enthalpy change for the reaction. Based on your answers to parts (a) and (b), which is more important in determining the position of this equilibrium, the entropy effect or the energy effect? In which direction will the equilibrium shift as the temperature increases above 200. °C? Explain. Suppose that the pressure were increased to triple its initial value. In which direction would the equilibrium shift? Why is the equilibrium not established at room temperature?
Write an equation for an equilibrium system that would lead to the following expressions (ac) for K. (a) K=(Pco)2 (PH2)5(PC2H6)(PH2O)2 (b) K=(PNH3)4 (PO2)5(PNO)4 (PH2O)6 (c) K=[ ClO3 ]2 [ Mn2+ ]2(Pcl2)[ MNO4 ]2 [ H+ ]4 ; liquid water is a product
According to the Resource Conservation and Recovery Act (RCRA), waste material is classified as toxic and must be handled as hazardous if the lead concentration exceeds 5 mg/L. By adding chloride ion, the lead ion will precipitate as PbCl2, which can be separated from the liquid portion. Once the lead has been removed, the rest of the waste can be sent to a conventional waste treatment facility. How many grams of sodium chloride must be added to 500 L of a waste solution to reduce the concentration of the Pb2+ ion from 10 to 5 mg/L?
For the equilibrium reaction in Question 4, write the expression for the equilibrium constant. (a) How would this equilibrium constant change if the total pressure on the system were doubled? (b) How would the equilibrium constant change if the temperature were increased?
Characterize each of the following as product- or reactant-favored at equilibrium. (a) CO(g) + O2(g) CO2(g)Kp = 1.2 1045 (b) H2O(g) H2(g) + O2(g)Kp = 9.1 1041 (c) CO(g) + Cl2(g) COCl2(g)Kp = 9.1 1011
Complete each of these reactions by filling in the blanks. Predict whether each reaction is product-favored or reactant-favored, and explain your reasoning. (a) (aq)+HSO4(aq)HCN(aq)+SO42(aq) (b) H2S (aq) + H2O() H3O+(aq) + _____ (aq) (c) H(aq) + H2O() OH(aq) +_____ (g)
. Explain what it means that a reaction has reached a state of chemical equilibrium. Explain why equilibrium is a dynamic state: Does a reaction really “stop” when the system reaches a state of equilibrium? Explain why, once a chemical system has reached equilibrium, the concentrations of all reactants remain constant with time. Why does this constancy of concentration not contradict our picture of equilibrium as being dynamic? What happens to the rates of the forward and reverse reactions as a system proceeds to equilibrium from a starting point where only reactants are present?
Suppose a reaction has the equilibrium constant K = 1.3 108. What does the magnitude of this constant tell you about the relative concentrations of products and reactants that will be present once equilibrium is reached? Is this reaction likely to be a good source of the products?
Write the equilibrium constant expression for each of the following reactions in terms of concentrations. (a) CO2(g) + C(s) 2 CO(g) (b) [Cu(NH3)4)2+(aq) Cu2+(aq) + 4 NH3(aq) (c) CH3CO2H(aq) + H2O() CH3CO2(aq) + H3O+(aq)
Consider the reaction 2N2O(g) + O2(g) 4NO(g) Suppose the system is at equilibrium, and then an additional mole of N2O(g) is injected into the system at constant temperature. Once the reaction reestablishes equilibrium, has the amount of N2O increased or decreased from its original equilibrium amount? Explain. What happens to the value of the equilibrium constant with this change?
The value of the equilibrium constant, K, is dependent on which of the following? (There may be more than one answer.) a. the initial concentrations of the reactants b. the initial concentrations of the products c. the temperature of the system d. the nature of the reactants and products Explain.

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Enter your answer in the provided box. Gaseous ammonia was introduced into a sealed container and heated to a certain temperature: 2 NH3(g) N2(g) + 3 H2(g) At equilibrium, [NH3] = 0.0232 M, [N2] = 0.119 M, and [H2] = 0.367 M. Calculate Ke for the reaction at this temperature. Kc =