Q&A Hero

Q: Which acid has the strongest conjugate base in aqueous solution? A) HF B) HNO3 C) HClO4 D) HI E) H2SO4

Q: Which of the following species cannot act as a Lewis acid?A) BeCl2B) H+C) Ag+D) BF3E) NH4+

Q: Which of the following is/are an appropriate classification of the reaction given below?KOH(aq) + CO2(g) → KHCO3(aq)1) The above reaction may be classified as an Arrhenius acid-base reaction.2) The above reaction may be classified as a Brnsted-Lowry acid-base reaction.3) The above reaction may be classified as a Lewis acid-base reaction.A) 1 onlyB) 2 onlyC) 3 onlyD) 1 and 3E) none

Q: Which of the following is not an example of an acid-base reaction?A) Al(OH)3(s) + 3H+(aq) → Al3+(aq) + 3H2O(l)B) C2H6(g) → C2H4(g) + H2(g)C) MgO(s) + CO2(g) → MgCO3(s)D) Al(OH)3(s) + OH-(aq) → Al(OH)4-(aq)E) CN-(aq) + H2O(l) HCN(aq) + OH-(aq)

Q: Consider the following reaction:AgBr(s) + 2CN"(aq) → Ag(CN)2"(aq) + Br"(aq)The species that are acting as a Lewis acid and Lewis base, respectively, areA) Br"and CN".B) Ag+and CN".C) AgBr and Ag(CN)2".D) Ag(CN)2"and Ag+.E) Ag+and Br".

Q: In the reactionCuO(s) + SO2(g) → CuSO3(s),A) O2-acts as a Lewis base and SO2acts as a Lewis acid.B) O2-acts as a Lewis base and Cu2+acts as a Lewis acid.C) CuO is the Lewis acid and CuSO3 is its conjugate base.D) SO2is the Lewis acid and CuSO3is its conjugate base.E) Cu2+acts as a Lewis acid and SO32-acts as a Lewis base.

Q: Which of the following species cannot act as a Lewis acid?A) H+B) H-C) K+D) Mg2+E) Al3+

Q: Which of the following species cannot act as a Lewis base?A) NH3B) NH4+C) N3-D) NH2-E) NH2-

Q: Which of the following species cannot act as a Lewis base?A) H2O2B) OH-C) O2-D) H2OE) Be2+

Q: Which of the following species cannot act as a Lewis base?A) H2SB) S2-C) Al3+D) SH-E) H2O

Q: Which of the following species is amphiprotic in aqueous solution?A) CH3NH2B) H3O+C) NH4+D) F-E) H2O

Q: What is a conjugate acid"base pair for the following equilibrium? H2O(l) + NH4+(aq) NH3(aq) + H3O+(aq) A) H2O is an acid and NH3is its conjugate base. B) H2O is an acid and H3O+is its conjugate base. C) NH4+is an acid and NH3is its conjugate base. D) H2O is a base and NH3is its conjugate acid. E) H2O is a base and NH4+is its conjugate acid.

Q: What is the conjugate base of H2PO4-(aq)?A) PO43-B) H3O+C) HPO42-D) H3PE) H3PO4

Q: What is a conjugate acid-base pair for the following equilibrium?H2O(l) + HPO42-(aq) H2PO4-(aq) + OH-(aq)A) H2O is an acid and HPO42-is its conjugate base.B) HPO42- is an acid and OH-is its conjugate base.C) H2O is an acid and OH-is its conjugate base.D) HPO42- is an acid and H2PO4-is its conjugate base.E) HPO42- is an acid and H2O is its conjugate base.

Q: Which of the following pairs of species is not a conjugate acid-base pair?A) HOCl, OCl-B) HNO2, NO2+C) O2-, OH-D) HSO4-, SO42-E) H2CO3, HCO3-

Q: Which are the Brnsted"Lowry bases in the following equilibrium?CH3COO-(aq) + H2O(l) CH3COOH(aq) + OH-(aq)A) CH3COO-and OH-B) H2O and OH-C) H2O, CH3COOH, and OH-D) CH3COO-and CH3COOHE) H2O and CH3COOH

Q: Which of the following statements is/are consistent with the Brnsted-Lowry concept of acids and bases? 1) A conjugate acid-base pair may differ by only one proton. 2) A base is defined as a hydroxide ion donor. 3) Brnsted-Lowry acid-base reactions are restricted to aqueous solutions. A) 1 only B) 2 only C) 3 only D) 1 and 2 E) 1, 2, and 3

Q: Which of the following statements is correct concerning the neutralization of sulfurous acid by a strong base?2OH-(aq) + H2SO3(aq) → SO32-(aq) + 2H2O(l)A) H2SO3is both an Arrhenius acid and a Brnsted-Lowry acid.B) H2SO3is a Brnsted-Lowry acid, but not an Arrhenius acid.C) H2SO3is neither an Arrhenius acid nor a Brnsted-Lowry acid.D) H2SO3is an Arrhenius acid, but not a Brnsted-Lowry acid.E) H2SO3is a Lewis base.

Q: Which of the following species is not capable of acting as an Arrhenius acid in aqueous solution?A) CHCl3B) HNO3C) H2SO4D) H3O+E) HClO4

Q: Which of the following species is not capable of acting as an Arrhenius acid in aqueous solution?A) Br-B) HFC) H2SO3D) H3O-E) HNO3

Q: Which of the following statements does not describe a characteristic of an Arrhenius acid?A) An Arrhenius acid reacts with an Arrhenius base to produce a salt.B) An Arrhenius acid turns red litmus blue.C) An Arrhenius acid is an electrolyte.D) An Arrhenius acid reacts with CaCO3to produce CO2.E) An Arrhenius acid tastes sour.

Q: Which of the following statements is/are consistent with the Arrhenius concept of acids and bases?1) An Arrhenius acid will increase the concentration of hydronium ion in an aqueous or nonaqueous solvent.2) All Arrhenius acids are strong electrolytes in water.3) All strong acid-strong base reactions have the same heat of reaction (Hº) per mole of water formed.A) 1 onlyB) 2 onlyC) 3 onlyD) 1 and 3E) 1, 2 and 3

Q: Which of the following reactions is not readily explained by the Arrhenius concept of acids and bases?A) HCl(g) + NH3(g) → NH4Cl(s)B) HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)C) HClO4(aq) + H2O(l) → H3O+(aq) + ClO4-(aq)D) HC2H3O2(aq) + H2O(l) H3O+(aq) + C2H3O2-(aq)E) H3O+(aq) + OH-(aq) → 2H2O(l)

Q: Which of the following statements is incorrect concerning the addition of a catalyst to an equilibrium reaction system?A) The catalyst speeds up the attainment of equilibrium.B) If the reactants are capable of forming many different products, a catalyst may selectively speed up one reaction over another.C) The catalyst increases the rate of both the forward and the reverse reaction.D) The catalyst increases the yield of the products.E) The catalyst is not consumed in either the forward or the reverse reaction.

Q: For the endothermic reaction 2CO2(g) + N2(g) 2NO(g) + 2CO(g), the conditions that favor maximum conversion of the reactants to products are A) high temperature and low pressure. B) high temperature, pressure being unimportant. C) low temperature and low pressure. D) low temperature and high pressure. E) high temperature and high pressure.

Q: Consider the following system at equilibrium: N2(g) + 3H2(g) 2NH3(g); Hº= -92.94 kJ Which of the following changes will shift the equilibrium to the right?I. increasing the temperatureII. decreasing the temperatureIII. increasing the volumeIV. decreasing the volumeV. removing some NH3VI. adding some NH3VII. removing some N2VIII. adding some N2A) II, III, V, VIIIB) I, III, V, VIIC) I, VI, VIIID) I, IV, VI, VIIE) II, IV, V, VIII

Q: Consider the reactionS2Cl2(l) + CCl4(l) CS2(g) + 3Cl2(g); Hº= 84.3 kJIf the above reactants and products are contained in a closed vessel and the reaction system is at equilibrium, the number of moles of CS2 can be increased byA) increasing the size of the reaction vessel.B) adding some Cl2 to the system.C) adding some S2Cl2 to the system.D) decreasing the temperature of the reaction system.E) adding some CCl4 to the system.

Q: The following equilibrium is exothermic. How could the yield of diiodine pentoxide be increased? I2(g) + 5CO2(g) 5CO(g) + I2O5(g) A) by decreasing the pressure B) by increasing the pressure C) by decreasing the volume of the reaction vessel D) by decreasing the temperature E) by increasing the temperature

Q: Consider the following equilibrium:N2O4(g) 2NO2(g)Suppose two different experiments were conducted on this equilibrium, at two different temperatures.TrialTemperatureInitial Moles of N2O4Equilibrium Moles of N2O4125C1.000.815255C1.000.500What conclusion may be drawn from the above data?A) Kc> Kpat all temperatures.B) The reaction is exothermic.C) The forward reaction proceeds faster than the reverse reaction.D) Kp= 1 at 55ºC.E) The equilibrium constant increases with increasing temperature.

Q: Consider the following equilibrium:CO2(g) + C(graphite) 2CO(g); Hº= 172.5 kJThe equilibrium constant for this reaction willA) increase if the temperature is decreased.B) decrease with increasing temperature.C) increase at some pressures and decrease at other pressures.D) increase with increasing temperature.E) not change if the temperature is increased.

Q: Solid HgO, liquid Hg, and gaseous O2are placed in a glass bulb and allowed to reach equilibrium.2HgO(s) 2Hg(l) + O2(g); Hº= 181.6 kJThe amount of Hg(l) in the bulb could be increasedA) by removing some HgO(s).B) by adding an inert gas.C) by adding some HgO(s).D) by increasing the pressure.E) by increasing the temperature.

Q: For the following reaction system at equilibrium, which one of the changes below would cause the equilibrium to shift to the right?Br2(g) + 2NO(g) 2NOBr(g); Hº= -30 kJA) Remove some NO.B) Remove some Br2.C) Add some NOBr.D) Increase the volume of the reaction vessel.E) Decrease the temperature.

Q: Consider the following equilibrium:2NH3(g) N2(g) + 3H2(g); Hº= 92 kJWhat change should be made in order to increase the value of Kp for this reaction?A) Increase the pressure.B) Decrease the temperature.C) Increase the temperature.D) Decrease the pressure.E) Nothing; Kpcannot be changed.

Q: One method for the decomposition of carbon dioxide proceeds as follows:2CO2(g) 2CO(g) + O2(g); Hº = 559 kJWhich of the following changes will cause an increase in the equilibrium concentration of CO?A) adding more O2to the systemB) adding a catalystC) removing CO2 from the systemD) increasing the pressure of the system at constant temperatureE) increasing the temperature of the system

Q: The following equilibrium is established in a sealed, rigid container. How could the partial pressure of SO2 at equilibrium be increased?SO2Cl2(g) SO2(g) + Cl2(g); Hº= +67 kJA) by adding an inert gas such as heliumB) by increasing the temperatureC) by removing SO2Cl2 as it is formedD) by adding Cl2 to the systemE) by decreasing the volume of the reaction vessel

Q: Consider the following equilibrium at 25ºC:2ICl(g) I2(g) + Cl2(g); Hº= 27 kJ; Kp= 6.2 x10-6Which of the following would be true if the temperature were increased to 100ºC?1) The value of Kp would increase.2) The concentration of ICl(g) would increase.3) The partial pressure of I2 would increase.A) 1 onlyB) 2 onlyC) 3 onlyD) 1 and 2E) 1 and 3

Q: When the pressure of an equilibrium mixture of SO2, O2, and SO3 is halved at constant temperature, what is the effect on Kp?2SO2(g) + O2(g) 2SO3(g)A) Kp is doubled.B) Kp is halved.C) Kp is unchanged.D) Kp is tripled.E) Kp is decreased by a third.

Q: Ammonia is prepared industrially by the reactionN2(g) + 3H2(g) 2NH3(g)For the reaction, Hº= -92.2 kJ and K(at 25ºC) =4.0x108. When the temperature of the reaction is increased to 500ºC, which of the following statements is true?A) At equilibrium, more NH3is present at 500ºC than at 25ºC.B) The reaction of N2with H2to form ammonia is endothermic.C) Kfor the reaction will be larger at 500ºC than at 25ºC.D) Product formation (at equilibrium) is less favored as the temperature is raised.E) None of the above statements is true.

Q: For a specific reaction, which of the following statements can be made about the equilibrium constant? A) It can be changed by the addition of a catalyst. B) It increases when the concentration of one of the products is increased. C) It increases when the concentration of one of the reactants is increased. D) It always remains the same. E) It changes with changes in the temperature.

Q: Consider the following equilibrium:NH4Cl(s) NH3(g) + HCl(g)Suppose a vessel containing NH4Cl(s), NH3(g) and HCl(g) is at equilibrium. If the volume of the vessel is instantaneously doubled while keeping the temperature constant, when a new equilibrium is reached, which of the following statements is incorrect?A) The value of Kp remains unchanged.B) The number of moles of NH4Cl decreases.C) The total pressure is halved.D) The partial pressures of NH3and HCl in the vessel remain unchanged.E) The amount of NH3and HCl doubles.

Q: In which of the following reactions does an instantaneous increase in the volume of the reaction vessel favor formation of the products? A) PCl5(g) PCl3(g) + Cl2(g) B) N2(g) + 3H2(g) 2NH3(g) C) H2(g) + I2(g) 2HI(g) D) MgO(s) + CO2(g) MgCO3(s) E) N2(g) + O2(g) 2NO(g)

Q: For which of the following systems at equilibrium and at constant temperature will increasing the volume have no effect on the equilibrium? A) C(s) + CO2(g) 2CO(g) B) SO2Cl2(g) SO2(g) + Cl2(g) C) COCl2(g) CO(g) + Cl2(g) D) I2(g) 2I(g) E) CO(g) + H2O(g) CO2(g) + H2(g)

Q: For which of the following systems at equilibrium and at constant temperature will decreasing the volume cause the equilibrium to shift to the right? A) NH4Cl(s) NH3(g) + HCl(g) B) 2NO2(g) 2NO(g) + O2(g) C) H2(g) + Cl2(g) 2HCl(g) D) N2(g) + 3H2(g) 2NH3(g) E) 2H2O(g) 2H2(g) + O2(g)

Q: Which of the following equilibria would be affected by volume changes at constant temperature? 1) 2NO(g) + 3F2(g) 2F3NO(g) 2) PCl3(g) + Cl2(g) PCl5(g) 3) O3(g) + NO(g) NO2(g) + O2(g) A) 1 only B) 2 only C) 3 only D) 1 and 2 E) 1, 2, and 3

Q: In which of the following reactions does a decrease in the volume of the reaction vessel at constant temperature favor formation of the products? A) 2H2(g) + O2(g) 2H2O(g) B) NO2(g) + CO(g) NO(g) + CO2(g) C) H2(g) + I2(g) 2HI(g) D) 2O3(g) 3O2(g) E) MgCO3(s) MgO(s) + CO2(g)

Q: Which of the following equilibria would be affected by volume changes at constant temperature? A) HCl(aq) + NaOH(aq) H2O(l) + NaCl(aq) B) C2H4(g) + H2(g) C2H6(g) C) 2HCl(g) H2(g) + Cl2(g) D) SO3(g) + NO(g) NO2(g) + SO2(g) E) 2HF(g) H2(g) + F2(g)

Q: Which of the following equilibria would not be affected by pressure changes at constant temperature?A) CO2(g) + H2(g) CO(g) + H2O(g)B) CO(g) + O2(g) CO2(g)C) 2Hg(l) + O2(g) 2HgO(s)D) 2H2(g) + O2(g) 2H2O(l)E) CaCO3(s) CaO(s) + CO2(g)

Q: Consider the reaction represented by the equation N2(g)+3H2(g)2NH3(g). What happens to the equilibrium position when an inert gas is added to this system (as represented above) at equilibrium? A) If the container is rigid, the equilibrium position shifts. If the container is fitted with a movable piston, nothing happens to the equilibrium position. B) If the container is rigid, nothing happens to the equilibrium position. If the container is fitted with a movable piston, the equilibrium position shifts. C) Nothing happens to the equilibrium position no matter what the container is like. D) The equilibrium position shifts no matter what the container is like. E) The value of the equilibrium constant must be known to answer this question.

Q: When cobalt chloride is added to pure water, the Co2+ions hydrate. The hydrated form then reacts with the Cl-ions to set up the equilibrium shown here:Co(H2O)62++ 4Cl-CoCl42-+ 6H2O(pink) (blue)Which statement describes the change that the system will undergo if potassium chloride is added?A) It should become more pink.B) Nothing will change.C) The silver ion will react with the CoCl42-.D) Water will be produced.E) It should become more blue.

Q: What effect will spraying liquid water into the equilibrium given below have if NH3is far more soluble in water than is N2or H2? N2(g) + 3H2(g) 2NH3(g) A) More NH3(g) will form. B) More H2(g) will form. C) Less NH3(g) will form. D) This will not affect the system. E) More N2(g) will form.

Q: Carbon monoxide is toxic because it can successfully compete with oxygen for hemoglobin (Hb) sites according to the following equilibrium: Hb(O2)4(aq) + 4CO(g) Hb(CO)4(aq) + 4O2(g) From Le Chtelier's principle, CO poisoning is reversed by A) increasing the O2pressure. B) decreasing the amount of Hb. C) increasing the CO2pressure. D) increasing the CO pressure. E) increasing the amount of Hb.

Q: When cobalt chloride is added to pure water, the Co2+ions hydrate. The hydrated form then reacts with the Cl-ions to set up the equilibrium shown here:Co(H2O)62++ 4Cl-CoCl42"+ 6H2O(pink) (blue)Which statement accurately describes the change that the system will undergo if water is added?A) The color will become more blue.B) The equilibrium will shift to the right.C) More water will be produced.D) More chloride ions will be produced.E) There will be less of the hydrated cobalt ion at the new equilibrium position.

Q: Consider the following equilibrium:PCl3(g) + Cl2(g) PCl5(g); Hº= -92 kJThe concentration of PCl3at equilibrium may be increased byA) decreasing the temperature.B) adding Cl2 to the system.C) adding PCl5 to the system.D) increasing the pressure.E) adding a catalyst.

Q: Which of the following, when added to an equilibrium mixture represented by the equlibrium below, will not alter the composition of the original equilibrium mixture?Mg(OH)2(s) Mg2+(aq) + 2OH-(aq)A) Addition of Mg(NO3)2(s) to the equilibrium mixture.B) Addition of Fe(NO3)3(aq) from the equilibrium mixture.C) Addition of Mg(OH)2(s) to the equilibrium mixture.D) Addition of HCl(aq) to the equilibrium mixture.E) Addition of NaOH(s) to the equilibrium mixture.

Q: Consider the following equilibrium:CO2(g) + H2(g) CO(g) + H2O(g); Kc= 1.6 at 1260 KSuppose 0.038 mol CO2and 0.022 mol H2 are placed in a 1.50-L vessel at 1260 K. What is the equilibrium partial pressure of CO(g)? (R= 0.0821 L·atm/(K·mol))A) 9.9 atmB) 1.1 atmC) 4.1 atmD) 2.6 atmE) 1.5 atm

Q: Exactly 1.0 mol N2O4 is placed in an empty 1.0-L container and allowed to reach equilibrium described by the equation N2O4(g) 2NO2(g).If at equilibrium the N2O4 is 28.0% dissociated, what is the value of the equilibrium constant, Kc, for the reaction under these conditions?A) 0.44B) 2.3C) 0.31D) 0.78E) 0.11

Q: At 550 K, Kp= 7.7 x 102 for the following equilibrium.SO2(g) + NO2(g) SO3(g) + NO(g)If 0.496 mol each of SO3 and NO are placed in a 5.00-L container at 550 K, what is the concentration of SO3 at equilibrium? (R= 0.0821 L·atm/(K·mol))A) 4.3 MB) 0.096 MC) 0.099 MD) 17 ME) 0.025 M

Q: At 800 K, Kc for the following equilibrium is 4.2 x 10-3.2HgO(s) 2Hg(l) + O2(g)Suppose 10.9 g of mercury (II) oxide is placed in a sealed 3.50-L vessel at 800 K. What is the partial pressure of oxygen gas at equilibrium? (R= 0.0821 L·atm/(K·mol))A) 0.83 atmB) 0.41 atmC) 0.28 atmD) 0.0042 atmE) 16 atm

Q: At 700 K, Kpfor the following equilibrium is 5.6 x 10-3.2HgO(s) 2Hg(l) + O2(g)Suppose 51.2 g of mercury(II) oxide is placed in a sealed 3.00-L vessel at 700 K. What is the partial pressure of oxygen gas at equilibrium? (R= 0.0821 L·atm/(K·mol))A) 0.075 atmB) 0.0056 atmC) 4.5 atmD) 19 atmE) 2.3 atm

Q: Hydrogen iodide undergoes decomposition according to the equation2HI(g) H2(g) + I2(g)The equilibrium constant Kp at 500 K for this equilibrium is 0.060. Suppose 0.520 mol of HI is placed in a 1.00-L container at 500 K. What is the equilibrium concentration of H2(g)?(R= 0.0821 L·atm/(K·mol))A) 0.14 MB) 0.085 MC) 4.2 MD) 0.025 ME) 0.10 M

Q: In an experiment, 0.42 mol H2and 0.42 mol I2are mixed in a 1.00-L container, and the reaction forms HI. If Kc= 49. for this reaction, what is the equilibrium concentration of HI? I2(g) + H2(g) 2HI(g) A) 0.81 M B) 0.74 M C) 0.65 M D) 0.105 M E) 0.056 M

Q: Consider the following equilibrium:2NO(g) + 3F2(g) 2NOF3(g)Suppose 0.20 mol of NO and 0.30 mol of F2 are added to a 5.0-L container. If x mol of NOF3is present at equilibrium, what is the equilibrium concentration of NO?A) 0.20xB) 0.05 - 0.50xC) 0.20 - 2xD) 0.04 - 0.20xE) 0.20 - x

Q: Consider the following equilibrium:2NO(g) + 3F2(g) 2NOF3(g)Suppose 0.20 mol of NO and 0.30 mol of F2 are added to a 5.0-L container. If xmol of NOF3 is present at equilibrium, how many moles of fluorine are present at equilibrium?A) 0.30 - xB) 0.30 - 2xC) 0.06 - 0.20xD) 0.30 - xE) 0.20 - x

Q: Consider the following equilibrium.4NH3(g) + 3O2(g) 2N2(g) + 6H2O(g)Suppose 0.30 mol of NH3and 0.40 mol of oxygen are added to a 5.0-L container. If xmol of water is present at equilibrium, what is the equilibrium concentration of oxygen?A) 0.40 - 0.50xB) 0.30 - 0.50xC) 0.08 - 0.10xD) 0.06 - 0.13xE) 0.40 - x

Q: Consider the following equilibrium:4NH3(g) + 3O2(g) 2N2(g) + 6H2O(g)Suppose 0.30 mol of NH3 and 0.40 mol of oxygen are added to a 5.0-L container. If x mol of water is present at equilibrium, how many moles of ammonia will remain at equilibrium?A) 0.30 - xB) 0.30 - xC) 0.30 - xD) 0.40 - xE) x

Q: The equilibrium constant for the reaction H2(g) + I2(g) 2HI(g) is 62.5 at 800 K. What is the equilibrium concentration of I2 if at equilibrium [HI] = 0.18 Mand [H2] = 0.11 M?A) 4.7 x 10-3MB) 0.25 MC) 5.2 x 10-2MD) 0.18 ME) 2.6 x 10-2M

Q: For the equilibrium PCl5(g) PCl3(g) + Cl2(g), Kc= 2.0 x 101 at 240ºC. If pure PCl5is placed in a 1.00-L container and allowed to come to equilibrium, and the equilibrium concentration of PCl3(g) is 0.47 M, what is the equilibrium concentration of PCl5(g)?A) 0.94 MB) 0.24 MC) 0.024 MD) 0.011 ME) 6.5 M

Q: For the equilibrium N2O4(g) 2NO2(g), at 298 K, Kp= 0.15. For this reaction system, it is found that the partial pressure of N2O4 is 3.2 x 10-2atm at equilibrium. What is the partial pressure of NO2at equilibrium? (R= 0.0821 L·atm/K·mol))A) 4.6 atmB) 21 atmC) 0.0022 atmD) 0.0048 atmE) 0.069 atm

Q: For the equilibrium PCl5(g) PCl3(g) + Cl2(g), Kc= 4.0 at 228ºC. If pure PCl5 is placed in a 1.00-L container and allowed to come to equilibrium, and the equilibrium concentration of PCl5(g) is 0.26 M, what is the equilibrium concentration of PCl3?A) 0.13 MB) 0.37 MC) 0.26 MD) 1.0 ME) 0.017 M

Q: Hydrogen iodide undergoes decomposition according to the equation2HI(g) H2(g) + I2(g)The equilibrium constant Kcat 425ºC for this system is 0.018. If 1.0 mol each of H2, I2, and HI were placed together in a 1-L container at 425ºC, thenA) because of reaction, the total number of molecules would increase.B) the concentration of HI would decrease.C) because of reaction, the total number of molecules would decrease.D) the value of Kwould increase to 1.0.E) the concentration of H2would decrease.

Q: For the reaction 2HI(g) H2(g) + I2(g), Kc= 0.290 at 400 K. If the initial concentrations of HI, H2, and I2are all 1.50 x10-3Mat 400 K, which one of the following statements is correct?A) The concentrations of HI and I2will increase as the system is approaching equilibrium.B) The concentrations of H2and I2will increase as the system is approaching equilibrium.C) The system is at equilibrium.D) The concentrations of H2and HI will decrease as the system is approaching equilibrium.E) The concentration of HI will increase as the system is approaching equilibrium.

Q: CS2(g) + 3Cl2(g) CCl4(g) + S2Cl2(g) At a given temperature, the reaction above is at equilibrium when [CS2] = 0.050 M, [Cl2] = 0.25 M, [CCl4] = 0.15 M, and [S2Cl2] = 0.35 M. What will be the direction of the reaction when the reactants and products have the following concentrations: CS2= 0.15 M, Cl2= 0.21 M, CCl4= 0.29 M, and S2Cl2= 0.34 M? A) to the left B) to the right C) no change D) cannot predict unless we know the temperature E) cannot predict unless we know whether the reaction is endothermic or exothermic

Q: The reaction quotient for a system is . If the equilibrium constant for the system is , what will happen as the reaction mixture approaches equilibrium? A) The equilibrium constant will increase until it equals the reaction quotient. B) There will be a net gain in both product(s) and reactant(s). C) There will be a net gain in product(s). D) There will be a net gain in reactant(s). E) The equilibrium constant will decrease until it equals the reaction quotient.

Q: What is the reaction quotient (Q) for the equilibriumCuSCN(s) Cu+(aq) + SCN-(aq)when 0.3317 L of M Cu+ is combined with 0.1018 L of M SCN- in the presence of an excess of CuSCN(s)?A) B) C) D) E)

Q: For the reaction TlCl(s) Tl+(aq) + Cl-(aq), Kc= at 25ºC. Which of the following concerning a 125 mL solution containing M Tl+, M Cl-and a large excess of TlCl(s) is/are correct?1) The mixture is at equilibrium.2) Additional TlCl(s) must dissolve to attain equilibrium.3) The reaction quotient (Q) is less than one.A) 1 onlyB) 2 onlyC) 3 onlyD) 2 and 3E) 1 and 3

Q: For the reaction 2H2S(g) 2H2(g) + S2(g), Kc= 9.1 x102 at 750 K. What will happen when 0.10 mol of H2S, 1.0 mol of H2, and 1.5 mol of S2 are added to a 1.0-L container and the system is brought to 750 K?A) More S2 will be formed than H2.B) More H2 will be formed than S2.C) Nothing; the system is at equilibrium.D) The amount of H2formed will be half the amount of S2 formed.E) More H2S will be formed.

Q: Consider the following equilibrium: C2H6(g) + C5H12(g) CH4(g) + C6H14(g); Kp= 9.57 at 500 K Suppose 47.2 g each of CH4, C2H6, C5H12, and C6H14are placed in a 25.0-L reaction vessel at 500 K. Which of the following statements is correct? A) Because Qc< Kc, more products will be formed. B) Because Qc= 1, the system is at equilibrium. C) Because Qc= 1, more products will be formed. D) Because Qc= 1, more reactants will be formed. E) Because Qc> Kc, more reactants will be formed.

Q: Consider the following equilibrium: C2H6(g) + C5H12(g) CH4(g) + C6H14(g); Kp= 9.57 at 500 K Suppose 57.5 g each of CH4, C2H6, C5H12, and C6H14are placed in a 10.0-L reaction vessel at 500 K. What is the value of Qp? A) 1.00 B) 0.104 C) 1.57 D) 0.637 E) 9.57

Q: Consider the following reaction:2HF(g) H2(g) + F2(g) (Kc= 1.00 x 10-2)Given that 1.00 mol of HF(g), 0.371 mol of H2(g), and 0.750 mol of F2(g) are mixed in a 5.00-L flask, determine the reaction quotient, Q.A) Q= 0.0696B) Q= 0.278C) Q= 0.0557D) Q= 2.12E) none of these

Q: Which of the following is/are true concerning equilibrium constants? 1) When an equilibrium constant is very large, the equilibrium mixture contains more reactants than products. 2) When an equilibrium constant is very small, the equilibrium mixture contains more products than reactants. 3) When an equilibrium constant is neither large nor small, the equilibrium mixture contains approximately equal amounts of reactants and products. A) 1 only B) 2 only C) 3 only D) 1 and 3 E) 1, 2, and 3