Q&A Hero

Q: Which of the following is always true for a reaction where Kcis at 25ºC?A) The reaction mixture contains mostly reactants at equilibrium.B) The reaction mixture contains mostly products at equilibrium.C) The rate of reaction is very slow.D) There are approximately equal moles of reactants and products at equilibrium.E) Both A and C.

Q: Which of the following can we determine by using an equilibrium constant for a gaseous reaction system? 1) the effect of changing the volume of the reaction system 2) the extent of a reaction at equilibrium 3) the direction of a reaction upon adding both reactants and products A) 1 only B) 2 only C) 3 only D) 1 and 2 E) 1, 2 and 3

Q: Which of the following is true for a system whose equilibrium constant is much greater than one? A) The reaction mixture contains mostly products at equilibrium. B) The reaction mixture contains mostly reactants at equilibrium. C) The rate of reaction is very fast. D) The moles of reactants and products are relatively similar at equilibrium. E) Both A and C.

Q: For which of the following reactions will the reactant experience the largest degree of decomposition upon reaching equilibrium at 500 K?A) 2NO2F(g) 2NO2(g) + F2(g); Kp= 6.6 x10-22B) 2SO3(g) 2SO2(g) + O2(g); Kp= 1.3 x10-5C) 2NOF(g) 2NO(g) + F2(g); Kp= 1.2 x10-26D) 2NOCl(g) 2NO(g) + Cl2(g); Kp= 1.7 x10-2E) 2NO2(g) 2NO(g) + O2(g); Kp= 5.9 x10-5

Q: For which of the following values of the equilibrium constant does the reaction mixture contain mostly reactants?A) 100B) 101C) 1019D) 10-1E) 109

Q: Consider the following equilibrium:O2(g) + 2F2(g) 2OF2(g); Kp= 2.3 x 10-15Which of the following statements is true?A) If the reaction mixture initially contains only OF2(g), then at equilibrium, the reaction mixture will consist of essentially only O2(g) and F2(g).B) For this equilibrium, Kc= Kp.C) If the reaction mixture initially contains only OF2(g), then the total pressure at equilibrium will be less than the total initial pressure.D) If the reaction mixture initially contains only O2(g) and F2(g), then at equilibrium, the reaction mixture will consist of essentially only OF2(g).E) If the reaction mixture initially contains only O2(g) and F2(g), then the total pressure at equilibrium will be greater than the total initial pressure.

Q: What is the Kcequilibrium-constant expression for the following equilibrium?FeO(s) + H2(g) Fe(s) + H2O(g)A) B) C) D) E)

Q: What is the Kpequilibrium-constant expression for the following equilibrium?S8(s) + 24F2(g) 8SF6(g)A) B) C) D) E)

Q: What is the Kcequilibrium-constant expression for the following equilibrium?S8(s) + 24F2(g) 8SF6(g)A) B) C) D) E)

Q: What is the Kpequilibrium-constant expression for the following equilibrium?Ti(s) + 2Cl2(g) TiCl4(l)A) B) C) D) E)

Q: Determine Kcfor reaction 3, given that reactions 1-3 may be rearranged and summed to give reaction 4.1) NH3(aq) + H2O(l) NH4+(aq) + OH-(aq); Kc= 1.76 x10-52) CH3COOH(aq) + H2O(l) CH3COO-(aq) + H3O+(aq); Kc= 1.75 x10-53) 4H2O(l) 2OH-(aq) + 2H3O+(aq); Kc= ?4) CH3COOH(aq) + NH3(aq) CH3COO-(aq) + NH4+(aq); Kc= 3.08 x104A) B) C) D) E)

Q: Given the equilibrium constants for the equilibria,2NH4+(aq) + 2H2O(l) 2NH3(aq) + 2H3O+(aq); Kc= CH3COOH(aq) + H2O(l) CH3COO-(aq) + H3O+(aq); Kc= determine Kcfor the following equilibrium.CH3COOH(aq) + NH3(aq) CH3COO-(aq) + NH4+(aq)A) 3.08 x 104B) 3.25 x 10-5C) 9.96 x 10-15D) 1.00 x 1014E) 1.75 x 10-5

Q: Given the equilibrium constants for the following reactions:4Cu(s) + O2(g) 2Cu2O(s); K12CuO(s) Cu2O(s) + O2(g); K2What is Kfor the system2Cu(s) + O2(g) 2CuO(s)equivalent to?A) (K2)2/(K1)B) K1xK2C) (K1)(K2)D) (K2)/(K1)E) (K1)/(K2)

Q: At 298 K, the value of Kcfor the reaction H2(g) + Br2(g) 2HBr(g) is 2.0 x 1019. What is Kcfor HBr(g) H2(g) + Br2(g)?A) 4.0 x 10-38B) 5.0 x 10-20C) 1.0 x 1019D) -2.0 x 1019E) 2.2 x 10-10

Q: Carbon tetrachloride may react with oxygen to produce chlorine and carbonyl chloride.2CCl4(g) + O2(g) 2COCl2(g) + 2Cl2(g); Kc= 9.9 x 1051What is Kc for the following equilibrium?COCl2(g) + Cl2(g) CCl4(g) + O2(g)A) 9.9 x 10-51B) 5.0 x 10-53C) 1.0 x 10-26D) 1.0 x 10-52E) -9.9 x 1051

Q: Consider the following equilibrium:N2O4(g) NO2(g); Kc= 3.3 at 100ºCFor which of the following equilibria is Kc less than 3.3 at 100ºC?A) N2O4(g) NO2(g)B) N2O4(g) 2NO2(g)C) 4N2O4(g) 8NO2(g)D) 3N2O4(g) 6NO2(g)E) 2N2O4(g) 4NO2(g)

Q: If Kc= 0.145 for A2+ 2B 2AB, what is the value of Kc for the reaction4AB 2A2+ 4B?A) 0.145B) 0.290C) 47.6D) -0.145E) 3.45

Q: For which of the following equilibria does Kc= Kp? A) N2(g) + 3H2(g) 2NH3(g) B) CO(g) + H2O(g) CO2(g) + H2(g) C) CO(g) + 3H2(g) CH4(g) + H2O(g) D) CaO(s) + CO2(g) CaCO3(s) E) HBr(g) H2(g) + Br2(l)

Q: For the reaction 2NO(g) + O2(g) 2NO2(g) at 750ºC, what is the relationship between Kc and Kp?A) Kc= KpB) Kc= Kp x (RT)-1C) Kc= Kp= 1.0D) Kc= Kp x (RT)E) Kc= Kp x (RT)1

Q: For which of the following reactions are the numerical values of Kp and Kc the same?1_ 2SO2(g) + O2(g) 2SO3(g)2_ N2(g) + O2(g) 2NO(g)3_ H2(g) + I2(g) 2HI(g)A) 1 onlyB) 2 onlyC) 1 and 2D) 2 and 3E) 1, 2, and 3

Q: A sample of ammonia gas was allowed to come to equilibrium at 400 K.2NH3(g) N2(g) + 3H2(g)At equilibrium, it was found that the concentration of H2 was 0.0283 M, the concentration of N2 was 0.00944 M, and the concentration of NH3 was 0.101 M. What is Kp for this equilibrium? (R= 0.0821 L·atm/(K·mol))A) 4.28B) 2.85C) 1.70 x 10-2D) 1.95 x 10-8E) 2.26 x 10-2

Q: A sample of ammonia gas was allowed to come to equilibrium at 400 K.2NH3(g) N2(g) + 3H2(g)At equilibrium, it was found that the concentration of H2 was 0.0367 M, the concentration of N2 was 0.0122 M, and the concentration of NH3 was 0.170 M. What was the initial concentration of ammonia?A) 0.122 MB) 0.146 MC) 0.218 MD) 0.182 ME) 0.194 M

Q: At 400 K, an equilibrium mixture of H2, I2, and HI consists of 0.065 mol H2, 0.079 mol I2, and 0.13 mol HI in a 4.50-L flask. What is the value of Kp for the following equilibrium? (R= 0.0821 L·atm/(K·mol))2HI(g) H2(g) + I2(g)A) 0.29B) 8.2C) 0.039D) 26E) 3.4

Q: A 4.50-mol sample of HI is placed in a 1.00-L vessel at 460ºC, and the reaction system is allowed to come to equilibrium. The HI partially decomposes, forming 0.343 mol H2 and 0.343 mol I2 at equilibrium. What is the equilibrium constant Kc for the following reaction at 460ºC?H2(g) + I2(g) HI(g)A) 1.23 x 102B) 8.10 x 10-3C) 3.09 x 10-2D) 11.1E) 5.69

Q: A sample of ammonia gas was allowed to come to equilibrium at 400 K.2NH3(g) N2(g) + 3H2(g)At equilibrium, it was found that the concentration of H2 was 0.0591 M, the concentration of N2was 0.0197 M, and the concentration of NH3 was 0.441 M. What is Kc for this equilibrium?A) 3.97 x 10"3B) 1.58 x 10"5C) 2.10 x 10"5D) 2.24 x 10"1E) 2.65 x 10"3

Q: For the reaction Br2(g) + Cl2(g) 2BrCl(g), at equilibrium, it is found that the concentrations of Br2, Cl2, and BrCl are 0.398 M, 0.351 M, and 2.05x10-3M, respectively. What is the value of Kc?A) 3.01 x 10-5B) 1.20 x 10-4C) 1.47 x 10-2D) 6.81 x 101E) 3.32 x 104

Q: Nitrogen trifluoride decomposes to form nitrogen and fluorine gases according to the following equation:2NF3(g) N2(g) + 3F2(g)When 2.12 mol of NF3 is placed in a 5.00-L container and allowed to come to equilibrium at 800 K, the mixture is found to contain 0.0362 mol of N2. What is the value of Kp at this temperature? (R = 0.0821 L·atm·mol-1·K-1)A) 1.07 x 10-5B) 1.91 x 10-3C) 1.78 x 10-3D) 1.11 x 10-5E) 4.43 x 10-7

Q: Which expression correctly describes the equilibrium constant Kcfor the following reaction?4NH3(g) + 5O2(g) 4NO(g) + 6H2O(g)A) B) C) D) E)

Q: Which of the following correctly describes the equilibrium constant for the gas-phase reaction between H2and O2to form gaseous H2O?A) Kc= B) Kc= C) Kc= [H2O]D) Kc= E) Kc=

Q: What balanced equation is the following equilibrium expression derived from?A) H2(g) + I2(g) HI(g)B) HI(g) H2(g) + I2(g)C) H2(aq) + I2(aq) HI(aq)D) HI(aq) H2(aq) + I2(aq)E) 2HI(g) H2(g) + I2(g)

Q: What is the balanced equation for the following equilibrium expression? A) 6SO2(g) + 3O2(g) 6SO3(g) B) 6SO3(g) 6SO2(g) + 3O2(g) C) 6SO3(aq) 6SO2(aq) + 3O2(aq) D) 6SO2(aq) + 3O2(aq) 6SO3(aq) E) SO2(g) + O2(g) SO3(g)

Q: The reaction of a mixture of SO2and O2at a given temperature is represented by the equation2SO2(g) + O2(g) 2SO3(g)When equilibrium is established, which of the following ratios is constant regardless of the initial concentrations of SO2 and O2?A) B) C) D) E)

Q: What is the expression for Kcfor the following equilibrium?CaCO3(s) CaO(s) + CO2(g)A) B) C) D) E)

Q: Which of the following can we predict from an equilibrium constant for a reaction? 1) The extent of a reaction 2) Whether the reaction is fast or slow 3) Whether the reaction is exothermic or endothermic A) 1 only B) 3 only C) 3 only D) 1 and 2 E) 1 and 3

Q: Apply the law of mass action to obtain the equilibrium-constant expression for the following reaction:2X(g) + Y(g) 3W(g) + V(g)A) [X]2[Y][W]3[V]B) C) D)

Q: The following reaction is investigated (assume an ideal gas mixture):2N2O(g) + N2H4(g) 3N2(g) + 2H2O(g)Initially there are 0.100 mol of N2O and 0.25 mol of N2H4, in a 10.0-L container. If there are 0.062mol of N2O at equilibrium, how many moles of N2are present at equilibrium?A) 3.8 x 10-2B) 1.1 x10-1C) 5.7 x 10-2D) 1.9 x 10-2E) none of these

Q: The Ostwald process converts ammonia (NH3) to nitric oxide (NO) by reaction with oxygen in the presence of a catalyst at high temperatures. In a test of the process a reaction vessel is initially charged with 3.90 mol NH3(g) and 4.90 mol O2(g), sealed, and heated at a fixed high temperature. When equilibrium is established the reaction mixture is analyzed and found to contain 2.90 mol NO(g). What is the quantity of NH3(g) in the equilibrium reaction mixture?4NH3(g) + 5O2(g) 4NO(g) + 6H2O(g)A) 1.00 mol NH3(g)B) 6.80 mol NH3(g)C) 3.90 mol NH3(g)D) 1.28 mol NH3(g)E) 2.00 mol NH3(g)

Q: Sulfur dioxide combines with O2in the presence of a catalyst as represented by the equation2SO2(g) + O2(g) 2SO3(g)Suppose 0.10 mol of SO2 and 0.10 mol of O2 are added to a 1-L vessel. At equilibrium, which of the following conditions must be true?A) [O2] = 2[SO3]B) [SO2] = [O2]C) [SO2] > [O2]D) [SO2] < [O2]E) [SO2] = [O2] = [SO3]

Q: A 15.00-L vessel at 700 K initially contains HI(g) at a pressure of 4.00 atm; at equilibrium, it is found that the partial pressure of H2(g) is 0.387 atm. What is the partial pressure of HI(g) at equilibrium? 2HI(g) H2(g) + I2(g) A) 4.00 atm B) 3.61 atm C) 3.23 atm D) 4.39 atm E) 0.387 atm

Q: Which of the following is/are true concerning a chemical reaction at equilibrium?1) The system will be a mixture of reactant and products.2) The rate of the forward and reverse reactions are equal.3) The amount of each reactant and product is constant.A) 1 onlyB) 2 onlyC) 3 onlyD) 1 and 2E) 1, 2, and 3

Q: Which of the following represents a dynamic equilibrium? A) a stoppered flask half full of water B) a coin spinning in mid-air C) two people of equal mass balanced on the ends of a seesaw D) an open pan of boiling water E) an object traveling at a constant speed

Q: When gaseous carbon monoxide and hydrogen are combined in a sealed vessel and heated they will eventually form an equilbrium mixture of reactants and products according to the balanced chemical equilibrium below. CO(g) + 3H2(g) CH4(g) + H2O(g) In one such reaction 3 moles of one reactant were combined with 1 mole of the other reactant in a fixed volume vessel and heated to 1200 K. Analysis of the reaction mixture at various times gave the results below. Which component of the reaction mixture is represented by curve B? A) carbon monoxide B) either methane or water C) hydrogen D) either hydrogen or carbon monoxide E) not enough information to decide

Q: Which of the following statements is true in a reaction system at equilibrium? A) The equilibrium constant is zero. B) The number of collisions per unit time between reactants is equal to the number of collisions per unit time between products. C) Reactants are reacting to form products at the same rate as products are reacting to form reactants. D) Reactants and products are present in equimolar amounts. E) The product of the concentrations of the products divided by the product of the concentrations of the reactants is always a constant.

Q: Which of the following changes will affect the rate constant of a reaction?1) Increasing or decreasing the reaction temperature.2) Adding a catalyst.3) Increasing or decreasing the reactant concentrations.A) 1 onlyB) 2 onlyC) 3 onlyD) 1 and 2E) 1, 2, and 3

Q: Which of the following statements best describes the condition(s) needed for a successful formation for a product according to the collision model?A) The relative orientation of the particles has an effect only if the kinetic energy of the particles is below some minimum value.B) The collision must involve a sufficient amount of energy, provided from the motion of the particles, to overcome the activation energy.C) The relative orientation of the particles must allow for formation of the new bonds in the product.D) The energy of the incoming particles must be above a certain minimum value, and the relative orientation of the particles must allow for formation of new bonds in the product.E) The relative orientation of the particles has little or no effect on the formation of the product.

Q: For the hypothetical reaction aA → products, the concentration of A was monitored with time. Given the following graph of the experimental data, what is the rate constant for the loss of reactant A?A) 2.42 µM -1·min-1B) 400.00 µM -1·min-1C) -2.42 µM -1·min-1D) -400 µM -1·min-1E) 24.2 µM -1·min-1

Q: For the hypothetical reaction A → products, the concentration of A was monitored with time. From the following graph, what is the rate constant for the decomposition of A?A) -0.07238 M-1s-1B) -10.00 M-1s-1C) 0.07238 M-1s-1D) 10.00 M-1s-1E) 0.007238 M-1s-1

Q: For the hypothetical reaction aA → products, the experimental data showed the following behavior (below). What is the reaction order with respect to reactant A?A) first-orderB) second-orderC) zero-orderD) third-orderE) fourth-order

Q: For the hypothetical reaction A → products, the concentration of A was monitored over time. From the following graph, what is the rate constant for the decomposition of A?A) -0.02735 s-1B) 2.3026 s-1C) -2.3026 s-1D) 0.02735 s-1E) 0.01188 s-1

Q: For a certain reaction of the general form aA → products, the experimental data plotted as 1/[A] versus time is linear. The slope of this plot must equalA) -1.B) the rate constant.C) one over the rate constant.D) the negative of the rate constant.E) 1.

Q: For a certain reaction of the general form aA → products, a plot of the experimental data as [A] versus time is linear. What is the reaction order with respect to reactant A?A) zeroB) firstC) secondD) fourthE) third

Q: The OH radical disproportionates according to the elementary chemical reactionThis reaction is second-order in OH. The rate constant for the reaction is 2.0 x 10-12cm3/molecules at room temperature. If the initial OH concentration is 1.7 x 1013molecules/cm3, what is the first half-life for the reaction?A) 3.4 x 101sB) 2.9 x 10-2sC) 1.5 x 10-2sD) 3.5 x 1011sE) 5.9 x 10-14s

Q: In a first-order reaction, the half-life is 137 minutes. What is the rate constant?A) 1.22 x 10-4 s-1B) 5790 s-1C) 0.304 s-1D) 5.06 x 10-3 s-1E) 8.43 x 10-5 s-1

Q: A first-order chemical reaction is observed to have a rate constant of 25 min-1. What is the corresponding half-life for the reaction?A) 1.7 sB) 1.7 minC) 36 minD) 2.4 sE) 35.8 s

Q: Which of the following corresponds to the correct equation for the half-life of a first-order reaction?A) B) C) D) E)

Q: For which order reaction is the half-life of the reaction proportional to 1/k (k is the rate constant)? A) second-order reaction only B) first-order reaction only C) zero-order reaction only D) all of the above E) none of the above

Q: The reaction 3NO → N2O + NO2 is found to obey the rate law Rate = k[NO]2. If the first half-life of the reaction is found to be 2.0 s, what is the length of the fourth half-life?A) 4.0 sB) 8.0 sC) 2.0 sD) 16.0 sE) 12.0 s

Q: The reaction A → products is first-order in A. If the concentration of A is cut in half, the half-life of the reaction willA) decrease by a factor of 1/2.B) double.C) decrease by a factor of 1/4.D) remain constant.E) quadruple.

Q: The half-life of a reaction is A) twice as long for a second-order reaction as it is for a first-order reaction. B) one-half of the time the reaction will take to go to completion. C) how long the reaction can run before stopping. D) the time it takes for the amount of product formed to equal half the initial amount of reactant. E) the time it takes for the reactant concentration to decrease to one-half of its initial value.

Q: A second-order reaction starts with an initial concentration of 0.100 mol/L of the reactant. If the rate constant is 3.6 x 10-2L/(mol·s), what is the time required to decrease the initial concentration to 0.050 mol/L?A) 280 sB) 420 sC) 19.3 sD) 1.39 sE) 830 s

Q: At 500oC, cyclopropane (C3H6) reacts to form its isomer, propene (C3H6). The reaction is first-order, and the rate constant is 6.7 x 10-4 s-1. If the initial concentration of cyclopropane is 0.500 Mand the initial concentration of propene is 0, determine the time required for the concentration of propene to reach 0.100 M.A) 3.4 x 103sB) 3.3 x 102sC) 1.2 x 104sD) 7.5 x 102sE) 2.4 x 103s

Q: Dinitrogen tetroxide decomposes to form nitrogen dioxide in a second-order reaction:N2O4(g) → 2NO2(g)At 400.0 K, the rate constant for this reaction has been measured to be 2.9 x 108L/(mol s). Suppose 0.222 mol of N2O4(g) is placed in a sealed 41.7-L container at 400.0 K and allowed to react. What is the total pressure inside the vessel after 32.9 ns has elapsed? (R= 0.0821 (L·atm)/(K·mol))A) 0.183 atmB) 0.175 atmC) 0.166 atmD) 0.524 atmE) 0.350 atm

Q: For the hypothetical second-order reaction A →products, k= 0.319 M-1 s-1. If the initial concentration of A is 0.834 M, how long would it take for A to be 94.8% consumed?A) 0.206 sB) 3.76 sC) 9.27 sD) 68.5 sE) 0.167 s

Q: For the hypothetical first-order reaction A → products, k= 0.0839 s-1. If the initial concentration of A is 0.640 M, how long would it take for A to be 66.4% consumed?A) 8.26 sB) 13.0 sC) 11.9 sD) 18.6 sE) 4.88 s

Q: The nuclide 188W decays by a first-order process with a rate constant of 1.0 x 10-2 d-1. How long will it take for 91% of the initial amount of 188W to be consumed?A) 4.1 dB) 220 dC) 9.4 dD) 240 dE) 110 d

Q: A reaction that is second-order in one reactant has a rate constant of 2.2 x 10-2L/(mols). If the initial concentration of the reactant is 0.360 mol/L, how long will it take for the concentration to become 0.180 mol/L?A) 320 sB) 63 sC) 1300 sD) 32 sE) 130 s

Q: The gas-phase decomposition of N2O5 is a first-order process with a rate constant of 1.50 x 10-3 s-1at 55ºC. The decomposition reaction isN2O5(g) → 2NO2(g) + O2(g)If 2.0 g of N2O5 is placed in vessel 1 and 1.0 g of N2O5in vessel 2 and the vessels are at the same temperature (55ºC) and the same pressure, how much time is required for half of the N2O5 to decompose in each vessel?A) Vessel 1 requires the same amount of time as vessel 2.B) Vessel 1 requires twice as much time as vessel 2.C) Vessel 1 requires three times as much time as vessel 2.D) Vessel 1 requires four times as much time as vessel 2.E) Vessel 2 requires twice as much time as vessel 1.

Q: The radioactive nuclide 63Ni decays by a first-order process via the emission of a beta particle. The 63Ni nuclide has a half-life of 100. years. How long will it take for 71% of 63Ni to decay? A) 49.4 years B) 21.5 years C) 0.858 years D) 179 years E) 77.6 years

Q: The nuclide 96Nb decays by a first-order process with a rate constant of 2.96 x 10-2 h-1. How long will it take for 82.0% of the initial amount of 96Nb to be consumed?A) 33.8 hB) 57.9 hC) 27.7 hD) 6.70 hE) 6.08 h

Q: A chemical reaction that is first-order in X is observed to have a rate constant of 2.20 x 10-2 s-1. If the initial concentration of X is 1.0 M, what is the concentration of X after 186s?A) 0.20 MB) 0.017 MC) 64 MD) 0.59 ME) 0.98 M

Q: At a given temperature, a first-order reaction has a rate constant of 3.5 x 10-3 s-1. How long will it take for the reaction to be 24% complete?A) 410 sB) 1200 sC) 910 sD) 34 sE) 78 s

Q: Which of the following is not a correct representation of the integrated rate expression for a first-order reaction?A) B) C) D) E)

Q: Which of the following corresponds to the correct integrated expression for a second-order reaction?A) B) C) D) E)

Q: The reaction between selenous acid and the iodide ion in acid solution isH2SeO3(aq) + 6I-(aq) + 4H+(aq) → Se(s) + 2I3-(aq) + 3H2O(l)The data in the following table were measured at 0C. Experiment[H2SeO3]0(M)[H+]0(M)[I"]0(M)Initial Rate [mol/(L·s)]11.00 x 10-42.00 x 10-23.00 x 10-25.30 x 10-722.00 x 10-42.00 x 10-23.00 x 10-21.06 x 10-633.00 x 10-44.00 x 10-23.00 x 10-26.36 x 10--643.00 x 10-48.00 x 10-23.00 x 10-22.54 x 10-553.00 x 10-48.00 x 10-26.00 x 10-22.04 x 10-462.00 x 10-42.00 x 10-26.00 x 10-28.48 x 10-6Tripling the initial concentration of I- while holding the initial concentrations of H2SeO3 and H+ constant increases the initial rate of the reaction by a factor ofA) 27.B) 9.C) 3.D) 8.E) 6.

Q: The reaction between selenous acid and the iodide ion in acid solution isH2SeO3(aq) + 6I-(aq) + 4H+(aq) → Se(s) + 2I3-(aq) + 3H2O(l)The data in the following table were measured at 0C. Experiment [H2SeO3]0(M)[H+]0(M)[I"]0(M)Initial Rate [mol/(L·s)]11.00 x 10-42.00 x 10-23.00 x 10-25.30 x 10-722.00 x 10-42.00 x 10-23.00 x 10-21.06 x 10-633.00 x 10-44.00 x 10-23.00 x 10-26.36 x 10-643.00 x 10-48.00 x 10-23.00 x 10-22.54 x 10-553.00 x 10-48.00 x 10-26.00 x 10-22.04 x 10-462.00 x 10-42.00 x 10-26.00 x 10-28.48 x 10-6Tripling the initial concentration of H+while holding the initial concentrations of H2SeO3 and I- constant increases the initial rate of the reaction by a factor ofA) 9.B) 16.C) 32.D) 2.E) 4.

Q: The reaction between selenous acid and the iodide ion in acid solution isH2SeO3(aq) + 6I-(aq) + 4H+(aq) → Se(s) + 2I3-(aq) + 3H2O(l)The data in the following table were measured at 0C. Experiment[H2SeO3]0(M)[H+]0(M)[I-]0(M)Initial Rate [mol/(L·s)]11.00 x 10-42.00 x 10-23.00 x 10-25.30 x 10-722.00 x 10-42.00 x 10-23.00 x 10-21.06 x 10-633.00 x 10-44.00 x 10-23.00 x 10-26.36 x 10-643.00 x 10-48.00 x 10-23.00 x 10-22.54 x 10-553.00 x 10-48.00 x 10-26.00 x 10-22.04 x 10-462.00 x 10-42.00 x 10-26.00 x 10-28.48 x 10-6Tripling the initial concentration of H2SeO3while holding the initial concentrations of H+ and I- constant increases the rate of the reaction by a factor ofA) 8.B) 4.C) 3.D) 2.E) 1.

Q: Two substances A and B react with each other in such a way that one-half of A remains after 25 min and one-fourth of A remains after 50 min. Doubling the concentration of B while keeping the concentration of A fixed doubles the rate of the reaction. This reaction is A) first-order in both A and B. B) zero-order in both A and B. C) second-order in A and first-order in B. D) first-order in A and second-order in B. E) second-order in both A and B.

Q: The reaction between selenous acid and the iodide ion in acid solution isH2SeO3(aq) + 6I-(aq) + 4H+(aq) → Se(s) + 2I3-(aq) + 3H2O(l)The data in the following table were measured at 0C. Experiment[H2SeO3]0(M)[H+]0(M)[I"]0(M)Initial Rate [mol/(L·s)]11.00 x 10-42.00 x 10-23.00 x 10-25.30 x 10-722.00 x 10-42.00 x 10-23.00 x 10-21.06 x 10-633.00 x 10-44.00 x 10-23.00 x 10-26.36 x 10-643.00 x 10-48.00 x 10-23.00 x 10-22.54 x 10-553.00 x 10-48.00 x 10-26.00 x 10-22.04 x 10-462.00 x 10-42.00 x 10-26.00 x 10-28.48 x 10-6What is the rate constant for this reaction?A) 1.5 x 104L5/(mol5·s)B) 1.5 x 1010L5/(mol5·s)C) 4.9 x 105L5/(mol5·s)D) 294 L5/(mol5·s)E) 8.8 L5/(mol5·s)

Q: The reaction between selenous acid and the iodide ion in acid solution isH2SeO3(aq) + 6I-(aq) + 4H+(aq) → Se(s) + 2I3-(aq) + 3H2O(l)The data in the following table were measured at 0C.Experiment[H2SeO3]0(M)[H+]0(M)[I-]0(M)Initial Rate [mol/(L·s)]11.00 x 10-42.00 x 10-23.00 x 10-5.30 x 10-722.00 x 10-42.00 x 10-23.00 x 10-21.06 x 10-633.00 x 10-44.00 x 10-23.00 x 10-26.36 x 10-643.00 x 10-48.00 x 10-23.00 x 10-22.54 x 10-553.00 x 10-48.00 x 10-26.00 x 10-22.04 x 10-462.00 x 10-42.00 x 10-26.00 x 10-28.48 x 10-6The overall order of this reaction isA) 4.B) 6.C) 2.D) 8.E) 3.

Q: In aqueous solution, iodine reacts with acetone as represented by the following equation:I2(aq) + CH3COCH3(aq) → CH3COCH2I(aq) + H+(aq) + I-(aq)The experimental rate law is Rate = k[H+][CH3COCH3]. According to the information above, an increase in the hydrogen ion concentration has what effect on the reaction?A) It decreases the rate of the reaction.B) It increases the rate of the reaction.C) It decreases the value of the equilibrium constant.D) It increases the value of the equilibrium constant.E) It does not affect the rate of the reaction.