Multiple ChoiceFor the reaction:N2 (g) + 2 O2 (g) ⇌ 2 NO2 (g), Kc = 8.3 x 10 -10 at 25°C. What is the concentration of N2 gas at equilibrium when the concentration of NO2 is twice the concentration of O2 gas?2549views2rank8comments
Multiple ChoiceAt a given temperature the gas phase reaction:N2 (g) + O2 (g) ⇌ 2 NO (g) has an equilibrium constant of 4.00 x 10 -15. What will be the concentration of NO at equilibrium if 2.00 moles of nitrogen and 6.00 moles oxygen are allowed to come to equilibrium in a 2.0 L flask.1711views1rank17comments
Multiple ChoiceCalculate the reaction quotient for the reaction below where the concentrations are [SO3] = 0.500 M, [SO2] = 0.0500 M, and [O2] = 0.100 M. 2 SO3 (g) ⇆ 2 SO2 (g) + O2 (g)325views
Multiple ChoiceIf Kc for the following reaction is 5.4 × 1013, 2 NO (g) + O2 (g) ⇆ 2 NO2 (g) what is Kc for the reaction shown below? 4 NO2 (g) ⇆ 4 NO (g) + 2 O2 (g)233views
Multiple ChoiceThe following reaction has a Kc value of 4.1 × 10-31 at 25 ºC. Calculate Kp at this temperature. N2 (g) + O2 (g) ⇆ 2 NO (g)231views
Multiple ChoiceCalculate Kc for the following reaction at 300 K where the equilibrium concentrations are [SO3] = 0.400 M, [SO2] = 0.200 M, and [O2] = 0.600 M. 2 SO3 (g) ⇆ 2 SO2 (g) + O2 (g)303views
Multiple ChoiceWhich of the following is a false statement about the relationship between Q and K?205views
Multiple ChoiceAt a given temperature the gas phase reaction: N2 (g) + O2 (g) ⇄ 2 NO (g) has an equilibrium constant of 4.18 x 10-7. What will be the concentration of NO at equilibrium if 2.00 moles of nitrogen and 6.00 moles oxygen are allowed to come to equilibrium in a 2.0 L flask?325views2rank
Multiple ChoiceConsider the following reaction:COBr2 (g) ⇌ CO (g) + Br2 (g)A reaction mixture initially contains 0.15 atm COBr2. Determine the equilibrium concentration of CO if Kp for the reaction at 25°C is 4.08.289views2rank
Multiple ChoiceAt a certain temperature, 0.810 mol NO is placed in a 5.00 L container. At equilibrium, 0.075 mol N2 is present. Calculate Kc. 2 NO (g) ⇌ N2 (g) + O2 (g)242views4rank
Multiple ChoiceWhen 0.600 atm of NO2 was allowed to come to equilibrium the total pressure was 0.875 atm. Calculate the Kp of the reaction. 2 NO2 (g) ⇌ 2 NO (g) + O2 (g)227views5rank
Textbook QuestionA mixture of 0.2000 mol of CO2, 0.1000 mol of H2, and 0.1600 mol of H2O is placed in a 2.000-L vessel. The following equilibrium is established at 500 K: CO21g2 + H21g2 Δ CO1g2 + H2O1g2 (d) Calculate Kc for the reaction.1563views
Textbook QuestionAt 2000 C, the equilibrium constant for the reaction 2 NO1g2 Δ N21g2 + O21g2 is Kc = 2.4 * 103. If the initial concentration of NO is 0.175 M, what are the equilibrium concentrations of NO, N2, and O2?981views
Textbook QuestionConsider the reaction and the associated equilibrium constant: aA(g) ⇌ bB(g) Kc = 4.0 Find the equilibrium concentrations of A and B for each value of a and b. Assume that the initial concentration of A in each case is 1.0 M and that no B is present at the beginning of the reaction. c. a=1;b=22235views1rank
Textbook QuestionFor the equilibrium Br21g2 + Cl21g2 Δ 2 BrCl1g2 at 400 K, Kc = 7.0. If 0.25 mol of Br2 and 0.55 mol of Cl2 are introduced into a 3.0-L container at 400 K, what will be the equilibrium concentrations of Br2, Cl2, and BrCl?1287views1rank
Textbook QuestionFor the reaction shown here, Kc = 0.513 at 500 K. N2O4(g) ⇌ 2NO2(g) If a reaction vessel initially contains an N2O4 concentration of 0.0500 M at 500 K, what are the equilibrium concentrations of N2O4 and NO2 at 500 K?2031views1comments
Textbook QuestionFor the reaction shown here, Kc = 255 at 1000 K. CO(g) + Cl2(g) ⇌ COCl2(g) If a reaction mixture initially contains a CO concentration of 0.1500 M and a Cl2 concentration of 0.175 M at 1000 K, what are the equilibrium concentrations of CO, Cl2, and COCl2 at 1000 K?3260views1rank
Textbook QuestionConsider the reaction: HC2H3O2(aq) + H2O(l) ⇌ H3O+(aq) + C2H3O2-(aq) Kc = 1.8 * 10-5 at25°C If a solution initially contains 0.210 M HC2H3O2, what is the equilibrium concentration of H3O + at 25 °C?3710views
Textbook QuestionConsider the reaction: SO2Cl2(g) ⇌ SO2(g) + Cl2(g) Kc = 2.99 * 10-7 at227°C If a reaction mixture initially contains 0.175 M SO2Cl2, what is the equilibrium concentration of Cl2 at 227 °C?2810views
Textbook QuestionConsider the reaction: A(g) ⇌ B(g) + C(g) Find the equilibrium concentrations of A, B, and C for each value of Kc. Assume that the initial concentration of A in each case is 1.0 M and that the reaction mixture initially contains no products. Make any appropriate simplifying assumptions. b. Kc = 0.0104055views1rank
Textbook QuestionWhen 2.00 mol of SO2Cl2 is placed in a 2.00-L flask at 303 K, 56% of the SO2Cl2 decomposes to SO2 and Cl2 : SO2Cl21g2 Δ SO21g2 + Cl21g2 (a) Calculate Kc for this reaction at this temperature.1257views1rank
Textbook QuestionAt 650 K, the reaction MgCO3(s) ⇌ MgO(s) + CO2(g) has Kp = 0.026. A 10.0-L container at 650 K has 1.0 g of MgO(s) and CO2 at P = 0.0260 atm. The container is then compressed to a volume of 0.100 L. Find the mass of MgCO3 that is formed.2251views
Textbook QuestionFor the equilibrium PH3BCl31s2 Δ PH31g2 + BCl31g2 Kp = 0.052 at 60 C. (b) After 3.00 g of solid PH3BCl3 is added to a closed 1.500-L vessel at 60 C, the vessel is charged with 0.0500 g of BCl31g2. What is the equilibrium concentration of PH3?1218views
Textbook QuestionA 0.831-g sample of SO3 is placed in a 1.00-L container and heated to 1100 K. The SO3 decomposes to SO2 and O2: 2 SO31g2 Δ 2 SO21g2 + O21g2 At equilibrium, the total pressure in the container is 1.300 atm. Find the values of Kp and Kc for this reaction at 1100 K.1347views
Textbook QuestionThe equilibrium constant Kc for C1s2 + CO21g2Δ 2 CO1g2 is 1.9 at 1000 K and 0.133 at 298 K. (b) If excess C is allowed to react with 25.0 g of CO2 in a 3.00-L vessel at 1000 K, how many grams of C are consumed?950views
Textbook QuestionA reaction vessel at 27 °C contains a mixture of SO2 (P = 3.00 atm) and O2 (P = 1.00 atm). When a catalyst is added, this reaction takes place: 2 SO2( g) + O2( g) ⇌ 2 SO3( g). At equilibrium, the total pressure is 3.75 atm. Find the value of Kc.3376views
Textbook QuestionThe industrial solvent ethyl acetate is produced by the reac-tion of acetic acid with ethanol: CH3CO2H1soln2 + CH3CH2OH1soln2 ∆ CH3CO2CH2CH31soln2 + H2O1soln2 Ethyl acetate (b) A solution prepared by mixing 1.00 mol of acetic acid and 1.00 mol of ethanol contains 0.65 mol of ethyl ace- tate at equilibrium. Calculate the value of Kc. Explain why you can calculate K without knowing the volume of the solution.642views
Textbook QuestionAt 70 K, CCl4 decomposes to carbon and chlorine. The Kp for the decomposition is 0.76. Find the starting pressure of CCl4 at this temperature that will produce a total pressure of 1.0 atm at equilibrium.1643views
Textbook QuestionThe equilibrium constant for the reaction SO2(g) + NO2(g) ⇌ SO3(g) + NO(g) is Kc = 3.0. Find the amount of NO2 that must be added to 2.4 mol of SO2 in order to form 1.2 mol of SO3 at equilibrium.2163views
Textbook QuestionAt 700 K, the equilibrium constant for the reaction CCl41g2 Δ C1s2 + 2 Cl21g2 is Kp = 0.76. A flask is charged with 2.00 atm of CCl4, which then reaches equilibrium at 700 K. (b) What are the partial pressures of CCl4 and Cl2 at equilibrium?1261views
Textbook QuestionCarbon monoxide and chlorine gas react to form phosgene: CO(g) + Cl2(g) ⇌ COCl2(g) Kp = 3.10 at 700 K If a reaction mixture initially contains 215 torr of CO and 245 torr of Cl2, what is the mole fraction of COCl2 when equilibrium is reached?3940views
Textbook QuestionConsider the hypothetical reaction A1g2 + 2 B1g2 Δ 2 C1g2, for which Kc = 0.25 at a certain temperature. A 1.00-L reaction vessel is loaded with 1.00 mol of compound C, which is allowed to reach equilibrium. Let the variable x represent the number of mol>L of compound A present at equilibrium. (e) From the plot in part (d), estimate the equilibrium concentrations of A, B, and C. (Hint: You can check the accuracy of your answer by substituting these concentrations into the equilibrium expression.)521views
Textbook QuestionRecalculate the equilibrium concentrations in Problem 15.93 if the initial concentrations are 2.24 M N2 and 0.56 M O2. (This N2>O2 concentration ratio is the ratio found in air.)294views
Textbook QuestionThe following equilibria were measured at 823 K: CoO1s2 + H21g2 ΔCo1s2 + H2O1g2 Kc = 67 H21g2 + CO21g2 ΔCO1g2 + H2O1g2 Kc = 0.14 (d) If the reaction vessel from part (c) is heated to 823 K and allowed to come to equilibrium, how much CoO1s2 remains?572views
Textbook QuestionAt 1000 K, the value of Kc for the reaction C1s2 + H2O1g2 ∆ CO1g2 + H21g2 is 3.0 * 10-2. Calculate the equilibrium concentrations of H2O, CO2, and H2 in a reac- tion mixture obtained by heating 6.00 mol of steam and an excess of solid carbon in a 5.00-L container. What is the molar composition of the equilibrium mixture?646views
Textbook QuestionAt 100 °C, Kc = 4.72 for the reaction 2 NO21g2 ∆ N2O41g2. An empty 10.0-L flask is filled with 4.60 g of NO2 at 100 °C. What is the total pressure in the flask at equilibrium?724views
Textbook QuestionThe equilibrium constant Kc for the reaction N21g2 + 3 H21g2 ∆ 2 NH31g2 is 4.20 at 600 K. When a quantity of gaseous NH3 was placed in a 1.00-L reaction vessel at 600 K and the reaction was allowed to reach equilibrium, the vessel was found to contain 0.200 mol of N2. How many moles of NH3 were placed in the vessel?432views
Textbook QuestionThe reaction of fumarate with water to form L-malate is catalyzed by the enzyme fumarase; Kc = 3.3 at 37°C. When a reaction mixture with [fumarate] = 1.56 * 10-3 M and [l -malate] = 2.27 * 10-3 M comes to equilibrium in the presence of fumarase at 37 °C, what are the equilibrium concentrations of fumarate and L-malate? (Water can be omit- ted from the equilibrium equation because its concentration in dilute solutions is essentially the same as that in pure water.)833views
Textbook QuestionVinegar contains acetic acid, a weak acid that is partially dissociated in aqueous solution: CH3CO2H1aq2 ∆ H+ 1aq2 + CH3CO-1aq2 (b) What is the value of Kc if the extent of dissociation in 1.0 M CH3CO2H is 0.42%?638views
Textbook QuestionHeavy water, symbolized D2O 1D = 2H2 finds use as a neutron moderator in nuclear reactors. In a mixture with ordinary water, exchange of isotopes occurs according to the following equation: H2O + D2O ∆ 2 HDO Kc = 3.86 at 298 K When 1.00 mol of H2O is combined with 1.00 mol of D2O, what are the equilibrium amounts of H2O, D2O, and HDO (in moles) at 298 K? Assume the density of the mixture is constant at 1.05 g>cm3.283views
Textbook QuestionRefining petroleum involves cracking large hydrocar- bon molecules into smaller, more volatile pieces. A simple example of hydrocarbon cracking is the gas-phase thermal decomposition of butane to give ethane and ethylene: (c) A sample of butane having a pressure of 50 atm is heated at 500 °C in a closed container at constant volume. When equilibrium is reached, what percentage of the butane has been converted to ethane and ethylene? What is the total pressure at equilibrium?326views
Textbook QuestionThe F ¬ F bond in F2 is relatively weak because the lone pairs of electrons on one F atom repel the lone pairs on the other F atom; Kp = 7.83 at 1500 K for the reaction F21g2 ∆ 2 F1g2. (b) What fraction of the F2 molecules dissociate at 1500 K?299views
Textbook QuestionAcetic acid tends to form dimers, 1CH3CO2H22, because of hydrogen bonding: The equilibrium constant Kc for this reaction is 1.51 * 102 in benzene solution but only 3.7 * 10-2 in water solution. (a) Calculate the ratio of dimers to monomers for 0.100 M acetic acid in benzene.370views
Textbook QuestionAcetic acid tends to form dimers, 1CH3CO2H22, because of hydrogen bonding: The equilibrium constant Kc for this reaction is 1.51 * 102 in benzene solution but only 3.7 * 10-2 in water solution. (b) Calculate the ratio of dimers to monomers for 0.100 M acetic acid in water.785views
Textbook QuestionA 79.2 g chunk of dry ice (solid CO2) and 30.0 g of graphite (carbon) were placed in an empty 5.00-L container, and the mixture was heated to achieve equilibrium. The reaction is CO 1g2 + C s ∆ 2 CO g (b) What is the value of Kp at 1100 K if the gas density at 1100 K is 16.9 g/L?794views
Textbook QuestionA 14.58 g quantity of N2O4 was placed in a 1.000-L reaction vessel at 400 K. The N2O4 decomposed to an equilibrium mix- ture of N2O4 and NO2 that had a total pressure of 9.15 atm. (b) How much heat (in kilojoules) was absorbed when the N2O4 decomposed to give the equilibrium mixture? (Stan- dard heats of formation may be found in Appendix B.)424views
Textbook QuestionThe equilibrium constant for the dimerization of acetic acid in benzene solution is 1.51 * 102 at 25 °C. 2 CH3CO2H ∆ 1CH3CO2H22 Kc = 1.51 * 102 at 25 °C (b) What is the osmotic pressure of the solution at 25 °C?886views
Textbook QuestionFor the decomposition reaction PCl51g2 ∆ PCl31g2 + Cl21g2, Kp = 381 at 600 K and Kc = 46.9 at 700 K. (b) If 1.25 g of PCl5 is introduced into an evacuated 0.500-L flask at 700 K and the decomposition reaction is allowed to reach equilibrium, what percent of the PCl5 will decompose and what will be the total pressure in the flask?503views