Consider the endothermic reaction: 5CO(g) + 1205(g) 12(g) + 5CO2(g) The following conditions favorably support the forward reaction (to the right) to achieve equilibrium EXCEPT increase in temperature decrease in the concentration of CO2(g) increase in pressure increase in the concentration of Cola)

Consider the endothermic reaction: 5CO(g) + 1205(g) 12(g) + 5CO2(g) The following conditions favorably support the forward reaction (to the right) to achieve equilibrium EXCEPT increase in temperature decrease in the concentration of CO2(g) increase in pressure increase in the concentration of Cola)

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter16: Spontaneity Of Reaction

Section: Chapter Questions

Problem 100QAP: Consider the reaction 2HI(g)H2(g)+I2(g)At 500C a flask initially has all three gases, each at a...

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. Gaseous phosphorus pentachloride decomposes according to the reaction PCl5(g)PCl3(g)+Cl2(g)The equilibrium system was analyzed at a particular temperature, and the concentrations of the substances present were determined to be [PCl5]=1.1102M,[PCl3]=0.325M. and [Cl2]=3.9103M. Calculate the value of K for the reaction.
The diagram represents an equilibrium mixture for the reaction N2(g) + O2(g) ⇌ 2 NO(g) Estimate the equilibrium constant.
At 2300 K the equilibrium constant for the formation of NO(g) is 1.7 103. N2(g) + O2(g) 2 NO(g) (a) Analysis shows that the concentrations of N2 and O2 are both 0.25 M, and that of NO is 0.0042 M under certain conditions. Is the system at equilibrium? (b) If the system is not at equilibrium, in which direction does the reaction proceed? (c) When the system is at equilibrium, what are the equilibrium concentrations?
Given the following descriptions of reversible reactions, write a balanced net ionic equation (simplest whole-number coefficients) and the equilibrium constant expression (K) for each. (a) Liquid acetone (C3H6O) is in equilibrium with its vapor. (b) Hydrogen gas reduces nitrogen dioxide gas to form ammonia and steam. (c) Hydrogen sulfide gas (H2S) bubbled into an aqueous solution of lead(ll) ions produces lead sulfide precipitate and hydrogen ions.
For the reactionN2O4(g)2NO2(g),Kp=0.25 at a certain temperature. If 0.040 atm of N2O4 is reacted initially, calculate the equilibrium partial pressures of NO2(g) and N2O4(g).
Kc = 5.6 1012 at 500 K for the dissociation of iodine molecules to iodine atoms. I2(g) 2 I(g) A mixture has [I2] = 0.020 mol/Land [I] = 2.0 108 mol/L. Is the reaction at equilibrium (at 500 K)? If not, which way must the reaction proceed to reach equilibrium?
The atmosphere consists of about 80% N2 and 20% O2, yet there are many oxides of nitrogen that are stable and can be isolated in the laboratory. (a) Is the atmosphere at chemical equilibrium with respect to forming NO? (b) If not, why doesnt NO form? If so, how is it that NO can be made and kept in the laboratory for long periods?
The initial concentrations or pressures of reactants and products are given for each of the following systems. Calculate the reaction quotient and determine the direction in which each system will proceed to reach equilibrium. (a) 2NH3(g)N2(g)+3H2(g) Kc=17;[NH3]=0.50M,[N2]=0.15M,[H2]=0.12M (b) 2NH3(g)N2(g)+3H2(g) Kp=6.8104 initial pressures NH3=2.00atm,N2=10.00atm,H2=10.00atm (c) 2SO3(g)2SO2(g)+O2(g) Kc=0.230;[SO3]=2.00M,[SO2]=2.00M,[O2]=2.00M (d) 2SO3(g)2SO2(g)+O2(g) Kp=16.5 initial pressures SO2=1.00atm,O2=1.130atm,SO3=0atm (e) 2NO(g)+CI2(g)2NOCI(g) Kp=2.5103 ; initial pressures; NO=1.00atm,CI2=1.00atm,NOCI=0atm (f) N2(g)+O2(g)2NO(g) Kc=0.050 ; [N2]=1.00M,[O2]=0.200M,[NO]=1.00M
The following data are for the system A(g)2B(g) (a) How long does it take the system to reach equilibrium? (b) How does the rate of the forward reaction compare with the rate of the reverse reaction after 30 s? After 90 s?
The following equilibrium is established in a closed container: C(s)+O2(g)CO2(g)H=393kJmol1 How does the equilibrium shift in response to each of the following stresses? (a) The quantity of solid carbon is increased. (b) A small quantity of water is added, and CO2 dissolves in it. (c) The system is cooled. (d) The volume of the container is increased.
Given the following descriptions of reversible reactions, write a balanced equation (smallest whole-number coefficients) and the equilibrium constant expression for each. (a) Nickel metal reacts with carbon monoxide to form nickel tetracarbonyl (Ni(CO)4) gas. (b) Aqueous nitrous acid in equilibrium with hydrogen and nitrite ions. (c) Chlorine gas and bromide ions in equilibrium with liquid bromine and chloride ions.
Many sugars undergo a process called mutarotation, in which the sugar molecules interconvert between two isomeric forms, finally reaching an equilibrium between them. This is true for the simple sugar glucose, C6H12O6, which exists in solution in isomeric forms called alpha-glucose and beta-glucose. If a solution of glucose at a certain temperature is analyzed, and it is found that the concentration of alpha-glucose is twice the concentration of beta-glucose, what is the value of K for the interconversion reaction?