Q&A Hero

Q: The conjugate base of OH- is ____.A.H3O+B.OH+C.O2-D.H+E.OH-

Q: In the following reactionSO32-(aq) + H2O() HSO3-(aq) + OH-(aq)A. SO32- is and acid and HSO3- is its conjugate base.B. SO32- is a base and HSO3- is its conjugate acid.C. SO32- is a base and H2O is its conjugate acidD. SO32- is an acid and OH- is its conjugate base.E.HSO3- is an acid and OH- is its conjugate base.

Q: In the following reaction,HCO3-(aq) + H2O() CO32-(aq) + H3O+(aq)A.H3O+ is an acid and HCO3- is its conjugate base.B.HCO3- is an acid and CO32- is its conjugate base.C.HCO3- is an acid and H2O is its conjugate base.D.H2O is an acid and CO32- is its conjugate base.E.H3O+ is an acid and CO32- is its conjugate base.

Q: Which equation depicts hydrogen phosphate ion behaving as a Brnsted-Lowry base in water?A.HPO42-(aq) + H2O() H2PO4-(aq) + OH-(aq)B.HPO42-(aq) + OH-(aq) PO43-(aq) + H2O()C.HPO42-(aq) + H2O() PO43-(aq) + H3O+(aq)D.2 HPO42-(aq) + O2-(aq) PO43-(aq) + H2O()E.2 HPO42-(aq) + H2O() 2 H2O() + P2O7(s)

Q: Which equation depicts aqueous hydrogen sulfide, behaving as a Brnsted-Lowry acid in water?A.H2S(aq) + 2 OH-(aq) SO2(aq) + 2 H2(g)B.H2S(aq) + H3O+(aq) H3S+(aq) + H2O()C.H2S(aq) + H2O() HS-(aq) + H3O+(aq)D.HS-(aq) + H3O+(aq) H2S(aq) + H2O()E.HS-(aq) + H2O() HSO+(aq) + H2(s)

Q: Which of the following substances is never a Brnsted-Lowry base in an aqueous solution? A.potassium hydroxide, NaOH(g) B.sodium hydrogen phosphate, Na2HPO4(s) C.sodium phosphate, Na3PO4(s) D.ammonium chloride, NH4Cl(g) E.sodium bicarbonate, NaHCO3(s)

Q: Which of the following substances is never a Brnsted-Lowry acid in an aqueous solution? A.sodium dihydrogen phosphate, NaH2PO4(s) B.sodium acetate, NaCH3CO2(s) C.ammonium nitrate, NH4NO3(s) D.hydrogen bromide, HCl(g) E.sodium bicarbonate, NaHCO3(s)

Q: According to the Brnsted-Lowry definition, a baseA.is a weak electrolyte.B.increases the OH- concentration in an aqueous solution.C.is an electron-pair donor.D.increases the pH of a solution.E.is a proton acceptor.

Q: According to the Brnsted-Lowry definition, an acid A.increases the H3O+ concentration in an aqueous solution. B.is a strong electrolyte. C.is a proton acceptor. D.increases the pH of a solution. E.is a proton donor.

Q: According to the Arrhenius definition, a base is a substance that when dissolved in water increases the concentration of A.hydroxide ion. B.hydronium ion. C.protons. D.electrolytes. E.cations.

Q: The standard enthalpy of formation of ammonia is -46.1 kJ/mol.1/2 N2(g) + 3/2 H2(g) NH3(g)Commercially, the reaction is carried out at high temperatures. Using your knowledge of kinetics and equilibrium, explain an advantage and a disadvantage of synthesizing ammonia at high temperatures.

Q: When 1.0 mole of acetic acid is diluted with water to a volume of 1.0 L at 25 C, 0.42% of the acetic acid ionizes to form acetate ion and hydronium ion.CH3CO2H(aq) + H2O() CH3CO2-(aq) + H3O+(aq)What percentage of the acid ionizes when 0.75 mole of acetic acid is diluted with water to 1.0 L at 25 C?

Q: If a stress is applied to an equilibrium system, the system will respond in such a way as to relieve that stress. This is a statement of ________ principle.

Q: In 1913, the Haber-Bosch process was patented. The product of the Haber-Bosch process is ________.

Q: The symbol Q is called the ________.

Q: A flask contains the following chemical system at equilibrium.CuCO3(s) Cu2+(aq) + 2 CO32-(aq)Addition of which of the following substances will increase the solubility of CuCO3(s) in water?1/ aqueous hydrochloric acid2/ aqueous sodium carbonate3/ solid copper(II) carbonateA.1 onlyB.2 onlyC.3 onlyD.1 and 3E.1, 2, and 3

Q: In which of the following equilibrium systems will an increase in the pressure have no effect on the concentrations of products and reactants? A.H2(g) + F2(g) 2 HF(g) B.N2(g) + 3 H2(g) 2 NH3(g) C.CaCO3(s) CaO(s) + CO2(g) D.2 NOBr(g) 2 NO(g) + Br2(g) E.2 H2O(g) + O2(g) 2 H2O2(g)

Q: The thermochemical equation for the formation of ammonia from elemental nitrogen and hydrogen is as follows.N2(g) + 3 H2(g) 2 NH3(g) DH = -92.2 kJGiven a system that is initially at equilibrium, which of the following actions cause the reaction to proceed to the left?A.adding N2(g)B.removing NH3(g)C.adding a catalystD.decreasing the temperatureE.removing H2(g)

Q: Assume that the following endothermic chemical reaction is at equilibrium. C(s) + H2O(g) H2(g) + CO(g) Which of the following statements is/are CORRECT? 1/ Increasing the concentration of H2(g) will cause the reaction to proceed in the backward direction, increasing the equilibrium concentration of H2O(g). 2/ Decreasing the temperature will cause the reaction to proceed in the forward direction, increasing the equilibrium concentration of CO(g). 3/ Increasing the amount of C(s) will cause the reaction to proceed in the forward direction, increasing the equilibrium concentration of CO(g). A.1 only B.2 only C.3 only D.1 and 2 E.1, 2, and 3

Q: Assume that the following chemical reaction is at equilibrium. 2 ICl(g) I2(g) + Cl2(g) DH = +26.9 kJ At 25 C, Kp = 2.0 105. If the temperature is increase to 45 C, which statement applies? A.Kp will decrease and the reaction will proceed in the backward direction. B.Kp will decrease and the reaction will proceed in the forward direction. C.Kp will remain unchanged and the reaction will proceed in the forward direction. D.Kp will increase and the reaction will proceed in the backward direction. E.Kp will increase and the reaction will proceed in the forward direction.

Q: Given the following equilibria,Ni2+(aq) + 2 OH-(aq) Ni(OH)2(s) K1 = 1.8 1015Ni2+(aq) + 4 CN-(aq) Ni(CN)42-(aq) K2 = 2.0 1031determine the equilibrium constant, Kc, for the following reaction.Ni(OH)2(s) + 4 CN-(aq) Ni(CN)42-(aq) + 2 OH-(aq)A.2.8 10-47B.9.0 10-17C.1.8 1015D.1.1 1016E.3.6 1046

Q: Given the following equilibria,PbBr2(s) Pb2+(aq) + 2 Br-(aq) K1 = 6.6 10-6Pb(OH)2(s) Pb2+(aq) + 2 OH-(aq) K2 = 1.4 10-15determine the equilibrium constant, Kc, for the following reaction.PbBr2(s) + 2 OH-(aq) Pb(OH)2(s) + 2 Br-(aq)A.9.2 10-21B.2.1 10-10C.6.6 10-6D.4.7 109E.1.1 1020

Q: Determine the equilibrium constant for the following reactionMg(OH)2(s) + 2 H+(aq) Mg2+(aq) + 2 H2O()given the chemical reactions below.Mg(OH)2(s) Mg2+(aq) + 2 OH-(aq) K = 5.6 10-12H2O() H+(aq) + OH-(aq) K = 1.0 10-14A.1.1 10-25B.5.6 10-12C.5.6 102D.1.1 103E.5.6 1016

Q: Given the following chemical equilibria, N2(g) + O2(g) 2 NO(g) K1 N2(g) + 3 H2(g) 2 NH3(g) K2 H2(g) + 1/2 O2(g) H2O(g) K3 Determine the method used to calculate the equilibrium constant for the reaction below. 4 NH3(g) + 5 O2(g) 4 NO(g) + 6 H2O(g) Kc A. B. C. D. E.

Q: The equilibrium constant (Kc) for the following reaction is 6.7 10-10 at 630 C.N2(s) + O2(g) 2 NO(g)What is the equilibrium constant for the reaction below at the same temperature?1/2 N2(g) + 1/2 O2(g) NO(g)A.4.5 10-19B.3.4 10-10C.1.3 10-9D.1.8 10-5E.2.6 10-5

Q: For the following reaction,2 SO3(g) 2 SO2(g) + O2(g)the equilibrium constant, Kp, is 1.32 at 627 C. What is the equilibrium constant, at 627 C, for the reaction below?SO2(g) + 1/2 O2(g) SO3(g)A.-1.15B.-0.66C.0.379D.0.870E.1.52

Q: Sulfuryl chloride decomposes to sulfur dioxide and chlorine. SO2Cl2(g) SO2(g) + Cl2(g) Kc is 0.045 at 648 K. If an initial concentration of 0.075 M SO2Cl2 is allowed to equilibrate, what is the equilibrium concentration of Cl2? A.0.0034 M B.0.030 M C.0.040 M D.0.058 M E.0.075 M

Q: At 800 K, the equilibrium constant, Kp, for the following reaction is 3.2 10-7.2 H2S(g) 2 H2(g) + S2(g)A reaction vessel at 800 K initially contains 3.00 atm of H2S. If the reaction is allowed to equilibrate, what is the equilibrium pressure of S2?A.8.5 10-5 atmB.6.2 10-3 atmC.9.0 10-3 atmD.1.1 10-2 atmE.1.4 10-2 atm

Q: The equilibrium constant, Kc, for the decomposition of ammonium hydrogen sulfide is 1.8 10-4 at 25 C.NH4HS(s) NH3(g) + H2S(g)If excess NH4HS(s) is allowed to equilibrate at 25 C, what is the equilibrium concentration of NH3?A.3.2 10-8 MB.9.0 10-5 MC.1.8 10-4 MD.6.7 10-3 ME.1.3 10-2 M

Q: If 0.64 mol PCl5 is placed in a 1.0 L flask and allowed to reach equilibrium at a given temperature, what is the final concentration of Cl2 in the flask? PCl5(g) PCl3(aq) + Cl2(g) Kc = 0.47 A.0.20 M B.0.31 M C.0.36 M D.0.55 M E.0.96 M

Q: Nitrogen and oxygen gases may react to form nitrogen monoxide. At 1500 C, Kc equals 1.0 10-5. N2(g) + O2(g) 2 NO(g) If 0.030 mol N2 and 0.030 mol O2 are sealed in a 1.0 L flask at 1500 C, what is the concentration of NO(g) when equilibrium is established? A.3.0 10-7 M B.4.7 10-5 M C.9.5 10-5 M D.3.0 10-2 M E.9.1 101 M

Q: The equilibrium constant at 25 C for the dissolution of silver iodide is 8.5 10-17.AgI(s) Ag+(aq) + I-(aq)If an excess quantity of AgI(s) is added to water and allowed to equilibrate, what is the equilibrium concentration of I-?A.7.2 10-33 MB.4.3 10-17 MC.8.5 10-17 MD.6.5 10-9 ME.9.2 10-9 M

Q: At 25 C, the decomposition of dinitrogen tetraoxide N2O4(g) 2 NO2(g) has an equilibrium constant (Kp) of 0.144. At equilibrium, the total pressure of the system is 0.0758 atm. What is the partial pressure of each gas? A.0.0745 atm NO2(g) and 0.0385 N2O4(g) B.0.0549 atm NO2(g) and 0.0209 N2O4(g) C.0.0531 atm NO2(g) and 0.0227 N2O4(g) D.0.0502 atm NO2(g) and 0.0256 N2O4(g) E.0.0381 atm NO2(g) and 0.0377 N2O4(g)

Q: A gaseous mixture of NO2 and N2O4 is in equilibrium. If the concentration of NO2 is 8.1 10-4 M, what is the concentration of N2O4?2 NO2(g) N2O4(g) Kc = 170A.5.6 10-5 MB.1.1 10-4 MC.2.2 10-4 MD.1.9 10-2 ME.1.4 10-1 M

Q: At an elevated temperature, the equilibrium constant, Kc, for the following reaction is 54.H2(g) + I2(g) 2 HI(g)If the equilibrium concentrations of H2 and I2 are 0.025 mol/L and 0.017 mol/L, what is the equilibrium concentration of HI?A.5.3 10-4 MB.2.8 10-3 MC.0.023 MD.0.15 ME.6.6 M

Q: Nitrosyl bromide decomposes according to the chemical equation below.2 NOBr(g) 2 NO(g) + Br2(g)When 0.260 atm of NOBr is sealed in a flask and allowed to reach equilibrium, 22% of the NOBr decomposes. What is the equilibrium constant, Kp, for the reaction?A.2.3 10-3B.4.5 10-3C.3.5 10-2D.4.8 10-2E.8.0 10-2

Q: A sealed tube is prepared with 1.66 atm PCl5 at 500 K. The PCl5 decomposes until equilibrium is established. PCl5(g) PCl3(aq) + Cl2(g) The equilibrium pressure in the tube is 2.28 atm. Calculate Kp. A.0.17 B.0.23 C.0.37 D.0.62 E.4.3

Q: When 0.20 mole HF is dissolved in water to a volume of 1.00 L, 5.8% of the HF dissociates to form F-(aq). What is the equilibrium constant for the reaction?HF(aq) + H2O() F-(aq) + H3O+(aq)A.1.3 10-4B.7.1 10-4C.1.2 10-2D.1.7 10-2E.6.2 10-2

Q: At a given temperature, 0.0664 mol N2O4(g) is placed in a 1.00 L flask. After reaching equilibrium, the concentration of NO2(g) is 6.1 10-3 M. What is Kc for the reaction below?N2O4(g) 2 NO2(g)A.3.7 10-5B.1.4 10-4C.5.9 10-4D.9.6 10-2E.1.8 103

Q: At 25 C, 0.138 mg AgBr dissolves in 10.0 L of water. What is the equilibrium constant for the reaction below?AgBr(s) Ag+(aq) + Br-(aq)A.5.40 10-13B.5.40 10-11C.1.90 10-8D.7.35 10-7E.1.90 10-6

Q: Excess Ag2SO4(s) is placed in water at 25 C. At equilibrium, the solution contains 0.029 M Ag+(aq). What is the equilibrium constant for the reaction below?Ag2SO4(s) 2 Ag+(aq) + SO42-(aq)A.1.8 10-7B.6.1 10-6C.1.2 10-5D.2.4 10-5E.8.4 10-4

Q: An aqueous mixture of phenol and ammonia has initial concentrations of 0.200 M C6H5OH(aq) and 0.120 M NH3(aq). At equilibrium, the C6H5O-(aq) concentration is 0.050 M. Calculate K for the reaction.C6H5OH(aq) + NH3(aq) C6H5O- + NH4+(aq)A.0.10B.0.24C.2.1D.4.2E.4.8

Q: At a high temperature, equal concentrations of 0.160 mol/L of H2(g) and I2(g) are initially present in a flask. The H2 and I2 react according to the balanced equation below. H2(g) + I2(g) 2 HI(g) When equilibrium is reached, the concentration of H2(g) has decreased to 0.036 mol/L. What is the equilibrium constant, Kc, for the reaction? A.3.4 B.4.0 C.12 D.22 E.48

Q: Consider the reaction A(aq) 2 B(aq) where Kc = 4.1 at 25 C. If 0.50 M A(aq) and 1.5 M B(aq) are initially present in a 1.0 L flask at 25 C, what change in concentrations (if any) will occur in time? A.[A] will decrease and [B] will decrease. B.[A] will decrease and [B] will increase. C.[A] will increase and [B] will decrease. D.[A] will increase and [B] will increase. E.[A] and [B] remain unchanged.

Q: A 2.5 L flask is filled with 0.25 mol SO3, 0.20 mol SO2, and 0.40 mol O2, and allowed to reach equilibrium. Assume the temperature of the mixture is chosen so that Kc = 0.12. Predict the effect on the concentration of SO3 as equilibrium is achieved by using Q, the reaction quotient. 2 SO3(g) 2 SO2(g) + O2(g) A.[SO3] will decrease because Q > K. B.[SO3] will decrease because Q < K. C.[SO3] will increase because Q < K. D.[SO3] will increase because Q > K. E.[SO3] will remain the same because Q = K.

Q: If the reaction quotient, Q, is equal to K in a gas phase reaction, then A.the chemical system has reached equilibrium. B.the temperature must be increased for the reaction to proceed in the forward direction. C.the reaction will proceed in the forward direction until equilibrium is established. D.the reaction will proceed in the backward direction until equilibrium is established. E.the reaction will proceed in the direction that increases the number of gas phase particles.

Q: If the reaction quotient, Q, is greater than K in a gas phase reaction, then A.the chemical system has reached equilibrium. B.the temperature must be increased for the reaction to proceed in the forward direction. C.the reaction will proceed in the forward direction until equilibrium is established. D.the reaction will proceed in the backward direction until equilibrium is established. E.the reaction will proceed in the direction that increases the number of gas phase particles.

Q: Given the following chemical equilibrium,COCl2(g) CO(g) + Cl2(g)calculate the value of Kc, given that Kp = 6.5 1011 at 298 K. (R = 0.08206 Latm/molK)A.1.5 10-12B.3.8 10-11C.1.1 109D.2.7 1010E.1.6 1013

Q: Ozone is formed from oxygen.3 O2(g) 2 O3(g)Calculate the value of Kp, given that Kc = 2.5 10-29 at 298 K. (R = 0.08206 Latm/molK)A.1.0 10-30B.2.1 10-30C.2.5 10-29D.3.3 10-28E.6.1 10-28

Q: What is the relationship between Kp and Kc for the reaction below? N2(g) + 3 H2(g) 2 NH3(g) A. B. C. D. E.

Q: For which one of the following reactions does Kp equal Kc? A.2 CO2(g) 2 CO(g) + O2(g) B.CH4(g) + 2 O2(g) CO2(g) + 2 H2O(g) C.C(s) + H2O(g) H2(g) + CO(g) D.NH3(g) 3/2 H2(g) + 1/2 N2(g) E.2 O3(g) 3 O2(g)

Q: Write a balanced chemical equation which corresponds to the following equilibrium constant expression.A.HNO2(aq) + H2O() NO2-(aq) + H3O+(aq)B.NO2-(aq) + H3O+(aq) HNO2(aq) + H2O()C.NO2-(aq) + H3O+(aq) HNO2(aq)D.H+(aq) + OH-(aq) H2O()E.HNO2(aq) NO2-(aq) + H3O+(aq)

Q: Write a balanced chemical equation which corresponds to the following equilibrium constant expression.A.PbF2(aq) Pb(s) + F2(aq)B.PbF2(s) Pb2+(aq) + 2 F-(aq)C.Pb2+(aq) + 2 F-(aq) PbF2(s)D.Pb(s) + F2(aq) PbF2(aq)E.PbF+(aq) + F-(aq) PbF2(aq)

Q: Write a balanced chemical equation which corresponds to the following equilibrium constant expression. A.1/2 N2(g) + 3/2 H2(g) NH3(g) B.N2(g) + 3 H2(g) 2 NH3(g) C.2 NH3(g) N2(g) + 3 H2(g) D.NH3(g) 1/2 N2(g) + 3/2 H2(g) E.2 N2(g) + 6 H2(g) 4 NH3(g)

Q: Write the expression for Kp for the reaction below. 2 NOBr(g) 2 NO(g) + Br2() A. B. C. D. E.

Q: Write the expression for Kp for the reaction below. MgCO3(s) MgO(s) + CO2(g) A. B. C. D. E.

Q: Write the expression for K for the reaction of hydrofluoric acid with water.HF(aq) + H2O() F-(aq) + H3O+(aq)A.B.C.D.E.

Q: Write the expression for K for the reaction below.Co2(CO3)3(s) 2 Co3+(aq) + 3 CO32-(aq)A.B.C.D.E.

Q: Write the expression for K for the reaction below.Al3+(aq) + 4 OH-(aq) Al(OH)4-(aq)A.B.C.D.E.

Q: Which of the following statements is/are CORRECT? 1/ Product concentrations appear in the numerator of an equilibrium constant expression. 2/ A reaction favors the formation of products if K >> 1. 3/ Stoichiometric coefficients are used as exponents in an equilibrium constant expression. A.1 only B.2 only C.3 only D.2 and 3 E.1, 2, and 3

Q: Which of the following statements is/are CORRECT? 1/ For a chemical system, if the reaction quotient (Q) is greater than K, reactant must be converted to products to reach equilibrium. 2/ For a chemical system at equilibrium, the forward and reverse rates of reaction are equal. 3/ For a chemical system at equilibrium, the concentrations of products divided by the concentrations of reactants equals one. A.1 only B.2 only C.3 only D.1 and 2 E.1, 2, and 3

Q: For a second-order decomposition reaction, 2A B rate = k[A]2 which of the following functions can be plotted versus time to give a straight line? A.[A] B. C. D.ln[A] E.

Q: Which of the following statements is correct for the first-order reaction: A 2B? A.The concentration of A decreases linearly with respect to time. B.The concentration of A is constant with respect to time. C.The natural logarithm of the concentration of A decreases linearly with respect to time. D.The rate of reaction is constant with respect to time. E.The rate constant,k, of the reaction decreases linearly with respect to time.

Q: How are the exponents in a rate law determined? A.They are equal to the inverse of the coefficients in the overall balanced chemical equation. B.They are determined by experimentation. C.They are equal to the coefficients in the overall balanced chemical equation. D.They are equal to the reactant concentrations. E.They are equal to the ln(2) divided by the rate constant.

Q: The reaction of NO and O2 produces NO2.2 NO(g) + O2(g) 2 NO2(g)The reaction is second-order with respect to NO(g) and first-order with respect to O2(g). At a given temperature, the rate constant, k, equals 4.7 102 M-2s-1. What is the rate of reaction when the initial concentrations of NO and O2 are 0.025 M and 0.015 M, respectively?A.2.6 10-3 M/sB.4.4 10-3 M/sC.0.18 M/sD.2.0 10-8 M/sE.3.8 102 M/s

Q: For the reaction 2A + B C, the rate law is . Which of the factor(s) will affect the value of the rate constant for this reaction? 1/ decreasing the temperature 2/ adding a catalyst 3/ decreasing the concentration of reactant A A.1 only B.2 only C.3 only D.1 and 2 E.2 and 3

Q: For the reaction A B, the rate law is . What are the units of the rate constant where time is measured in seconds? A. B. C. D. E.

Q: For the reaction A + 2B C, the rate law is . What are the units of the rate constant where time is measured in seconds? A. B. C. D. E.

Q: Given the initial rate data for the reaction A + B C, determine the rate expression for the reaction.[A], M [B], M D[C]/Dt (initial) M/s0418 0.488 2.73 10-4A.B.C.D.E.

Q: Given the initial rate data for the reaction A + B C, determine the rate expression for the reaction.[A], M [B], M D[C]/Dt (initial) M/s0344 0.272 6.10 10-2A.B.C.D.E.

Q: Given the initial rate data for the reaction A + B C, determine the rate expression for the reaction.[A], M [B], M D[C]/Dt (initial) M/s430 0.150 2.32 10-3A. B.C.D.E.

Q: Given the initial rate data for the decomposition reaction,A B + Cdetermine the rate expression for the reaction.[A], M -D[A]/Dt M/s042 6.2 10-6

Q: What is the overall order of the reaction below NO(g) + O3(g) NO2(g) + O2(g) if it proceeds via the following rate expression? A.zero-order B.first-order C.second-order D.third-order E.fourth-order

Q: Assume the reaction below 2 NO(g) + O2(g) 2 NO2(g) proceeds via the following rate expression: Which of the following statements concerning the above chemical reaction and rate equation is/are CORRECT? 1/ The reaction is second-order with respect to NO. 2/ The rate of disappearance of O2 is two times the rate of appearance of NO2. 3/ According to the balanced chemical equation, the reaction is fifth-order overall. A.1 only B.2 only C.3 only D.1 and 3 E.2 and 3

Q: What is the name given to a substance that increases the rate of a chemical reaction but is not itself consumed? A.catalyst B.reactant C.intermediate D.enthalpy E.rate constant

Q: Which of the following factors are likely to affect the rate of a chemical reaction? 1/ the presence of a catalyst 2/ the temperature of the reactants 3/ the physical state (solid, liquid, or gas) of the reactants A.1 only B.2 only C.3 only D.1 and 3 E.1, 2, and 3

Q: For the reaction below, if the rate of appearance of Br2 is 0.180 M/s, what is the rate of disappearance of NOBr?2 NOBr(g) 2 NO(g) + Br2(g)A.-0.360 M/sB.-0.090 M/sC.0.090 M/sD.0.180 M/sE.0.720 M/s

Q: Ozone decomposes to oxygen according to the balanced chemical equation below.2 O3(g) 3 O2(g)If the rate of disappearance of ozone is -2.4 10-6 M/s, what is the rate of formation of oxygen?A.-2.4 10-6 M/sB.1.6 10-6 M/sC.2.4 10-6 M/sD.3.6 10-6 M/sE.7.2 10-6 M/s

Q: Which relationship correctly compares the rates of the following reactants and products? 2 NOCl(g) 2 NO(g) + Cl2(g) A. B. C. D. E.

Q: Which statement concerning relative rates of reaction is correct for the chemical equation given below? 2 CH3OH(g) + 3 O2(g) 2 CO2(g) + 4 H2O(g) A.The rate of disappearance of CH3OH is equal to the rate of disapperance of O2. B.The rate of disappearance of CH3OH is two times the rate of appearance of H2O. C.The rate of disappearance of CH3OH is half the rate of appearance of CO2. D.The rate of appearance of H2O is two times the rate of appearance of CO2. E.The rate of appearance of H2O is four times the rate of disappearance of CH3OH.