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Chemistry
Q:
Given the reaction at a certain temperature: 2 HI(g) H2(g) + I2(g). At equilibrium, the partial pressure of HI is 1.8 10-3 atm, and the partial pressures for H2 and I2 are 0.10 atm each. Find Kp at that temperature.A) 3.2 10-4B) 5.6 101C) 3.1 103D) 3.1 104
Q:
The oxidation of sulfur dioxide by oxygen to sulfur trioxide has been implicated as an important step in the formation of acid rain: 2 SO2(g) + O2(g) 2 SO3(g). If the equilibrium partial pressures of SO2, O2, and SO3 are 0.564 atm, 0.102 atm, and 0.333 atm respectively at 1000 K, what is Kp at that temperature?A) 0.292B) 3.42C) 5.79D) 8.11
Q:
What is true about the relationship of Kp and Kc for the reaction:2 CH4(g) + 3 O2(g) 2 CO(g) + 4 H2O(g)?A) Kp < KcB) Kp = KcC) Kp > KcD) Kp and Kc are not related.
Q:
Write the equilibrium constant expression for the following reaction in the reverse direction:2 CH4(g) + 3 O2(g) 2 CO(g) + 4 H2O(g)A) Kp' = B) Kp' = C) Kp' = D) Kp' =
Q:
Write the equilibrium constant expression for the following reaction in the forward direction:2 CH4(g) + 3 O2(g) 2 CO(g) + 4 H2O(g)A) Kp = B) Kp= C) Kp = D) Kp =
Q:
Which one of the following statements about the equilibrium constant, Kp, is false?A) n is equal to the sum of the coefficients of the gaseous products minus the sum of the coefficients of the gaseous reactants.B) The relationship between Kp and Kc is: Kp =Kc (RT)nC) The units for Kp are usually omitted.D) Total pressures are used in the equilibrium equation in place of molar concentrations.
Q:
If Kc equals 0.11 at 25C for the reaction: N2O4(g) 2 NO2(g), what is Kc for the reaction: NO2(g) 1/2 N2O4(g)?A) 0.33B) 3.0C) 4.5D) 9.1
Q:
If Kc = 7.04 10-2 for the reaction: 2 HBr(g) H2(g) + Br2(g), what is the value of Kc for the reaction: ?A) 3.52 10-2B) 0.265C) 3.77D) 28.4
Q:
For the reaction: N2(g) + 2 O2(g) 2 NO2(g), Kc = 8.3 10-10 at 25C. What is the concentration of N2 gas at equilibrium when the concentration of NO2 is twice the concentration of O2 gas?A) 2.1 10-10 MB) 4.2 10-10 MC) 2.4 109 MD) 4.8 109 M
Q:
Given the reaction: 2 HI H2 + I2. If Kc' for the reverse reaction is 1.85 10-2 at 425C, what is Kc for the forward reaction at the same temperature?A) -1.85 10-2B) 1.85 10-2C) 3.70 10-2D) 54.1
Q:
A mixture of carbon monoxide, hydrogen, and methanol is at equilibrium. The balanced chemical equation is: . At 250C, the mixture contains 0.0960 M CO, 0.191 M H2, and 0.150 M CH3OH. What is the value for Kc?
A) 2.33 10-2
B) 0.244
C) 4.09
D) 42.8
Q:
Nitric oxide reacts with oxygen to form nitrogen dioxide:2 NO(g) + O2(g) 2 NO2(g)What is Kc'for the reverse reaction if the equilibrium concentration of NO is 0.300 M, O2 is 0.200 M, and NO2 is 0.530 M at ?A) 0.0340B) 0.0641C) 0.624D) 15.6
Q:
An aqueous reaction occurs by a two-step mechanism, shown below.Step 1: A2X2 + Y-> A2X + XYStep 2: A2X2 + XY -> A2X + X2 + YIn this reaction the intermediate is ________, and the catalyst is ________.
Q:
A gaseous reaction occurs by a two-step mechanism, shown below.Step 1: AX +Y2 -> AXY2Step 2: AXY2 + AX ->2 AXYIf the rate law for this reaction is Rate = k[AX]2[Y2], the intermediate is ________, and step ________ is the rate-determining step.
Q:
A reaction occurs by a two-step mechanism, shown below.Step 1: AX2(g)->AX(g) + X(g)Step 2: AX2(g) + X(g)-> AX + X2(g)The intermediate in this reaction is ________, and the molecularity of the second step is ________.
Q:
A gaseous compound, C, undergoes catalytic decomposition at an initial rate of 0.45 M/s when [C]o = 3.0 10-3 M and 0.45 M/s when [C]o = 9.0 10-3 M. Therefore, this is a ________ order reaction.
Q:
At an elevated temperature the decomposition of a gaseous oxide, AO2 occurs with a rate constant, k = 0.54 M-1s-1. If the half-life of this reaction is 926 seconds when [AO2] = 2.0 10-3 M and 462 seconds when [AO2] = 4.0 10-3 M, this reaction is ________ order.
Q:
Carbon-14 has a half-life of 5715 years. Currently living organisms decay at a rate of 15.3 disintegrations/ min per gram of carbon. If an archeological artifact has a carbon-14 decay rate of 12.0 disintegrations/ min per gram of carbon, the approximate age of the artifact is ________ years old.
Q:
At 55 the decomposition of N2O5 is first order, having a rate constant, k = 1.7 10-3 s-1. If the initial concentration of N2O5 is 6.4 10-3 M, the number of half-lives that are required for the N2O5 concentration to fall to 2.0 10-4 M is ________, and the amount of time required is ________ minutes.
Q:
The decomposition of hydrogen peroxide occurs according to the equation2 H2O2(aq)->2 H2O(l) + O2(g)A concentration-time study of this reaction produces a straight line when ln[H2O2] is plotted versus time. Therefore, this is a ________ order reaction.
Q:
At 300C decomposition of NO2(g) occurs with a rate law: Rate = - k[NO2]x. If the initial rate of decomposition is 3.2 10-5 M/s when [NO2]o = 8.0 10-3 M and the initial rate of decomposition is 8.0 10-6 M/s when [NO2]o = 4.0 10-3 M, then the order of reaction with respect to NO2, x = ________.
Q:
The reaction shown below has the rate law: Rate = k[BrO3-][Br-][H+]2. The order of reaction with respect to H+ is ________ and the overall order is ________.BrO3-(aq) + 5 Br-(aq) + 6 H+(aq) -> 3 Br2(aq) + 3 H2O(l)
Q:
For the reaction shown below, if the rate of formation of O2 is 6.0 10-6 M/s, the rate of decomposition of N2O5 over the same time interval is ________.2 N2O5(g) -> 4 NO2(g) + O2(g)
Q:
The aquation of tris(1,10-phenanthroline)iron(II) in acid solution takes place according to the equation:Fe(phen)32+ + 3 H3O+ + 3 H2O -> Fe(H2O)62+ + 3 phenH+.If the activation energy, Ea, is 126 kJ/mol and the rate constant at 30C is 9.8 10-3 min-1, what is the rate constant at 35C?A) 4.4 10-3 min-1B) 2.2 10-2 min-1C) 4.5 101 min-1D) 2.3 102 min-1
Q:
The activation for the following reaction is 180 kJ/mol:(g) + (g) -> (g)If the rate constant at 202C is 4.13 1, what is the rate constant at 277C?A) 2.10 1B) 1.66 1C) 5.39 D) 3.99
Q:
The second-order reaction 2 Mn(CO)5 -> Mn2(CO)10, has a rate constant equal to 3.0 109 M-1 s-1 at 25C. If the initial concentration of Mn(CO)5 is 2.0 10-5 M, how long will it take for 90.% of the reactant to disappear?A) 6.7 10-16 sB) 7.4 10-15 sC) 1.5 10-4 sD) 6.0 103 s
Q:
In aqueous solution, hypobromite ion, BrO-, reacts to produce bromate ion, BrO3-, and bromide ion, Br-, according to the following chemical equation. A plot of 1/[BrO-] vs. time is linear and the slope is equal to 0.056 M-1s-1. If the initial concentration of BrO- is 0.80 M, how long will it take one-half of the BrO- ion to react?
A) 4.5 10-2 s
B) 7.1 s
C) 12 s
D) 22 s
Q:
Carbon-14, which is present in all living tissue, radioactively decays via a first-order process. A one-gram sample of wood taken from a living tree gives a rate for carbon-14 decay of 13.6 counts per minute. If the half-life for carbon-14 is 5715 years, how old is a wood sample that gives a rate for carbon-14 decay of 11.9 counts per minute?A) 5.3 102 yrB) 7.6 102 yrC) 1.1 103 yrD) 9.4 103 yr
Q:
For the first-order reaction, 2 N2O(g) -> 2 N2(g) + O2(g), what is the concentration of N2O after 3 half-lives if mol of N2O is initially placed into a 1.00-L reaction vessel?A) 1.6 10-2 MB) 3.1 10-2 MC) 6.2 10-2 MD) 1.2 10-1 M
Q:
The first-order reaction, SO2Cl2 -> SO2 + Cl2, has a half-life of 8.75 hours at 593 K. How long will it take for the concentration of SO2Cl2 to fall to 16.5% of its initial value?A) 0.143 hrB) 2.28 hrC) 6.99 hrD) 22.7 hr
Q:
The following reaction is first order, C2H6 -> 2 CH3. If the rate constant is equal to 5.5 10-4 s-1 at 1000 K, how long will it take for 0.35 mol of C2H6 in a 1.00 L container to decrease to 0.20 mol in the same container?A) 4.5 minB) 17 minC) 53 minD) 65 min
Q:
The isomerization reaction, CH3NC -> CH3CN, is first order and the rate constant is equal to 0.46 s-1 at 600 K. What is the concentration of CH3NC after 0.20 minutes if the initial concentration is 0.30 M?A) 1.2 10-3 MB) 2.7 10-3 MC) 1.2 10-1 MD) 2.7 10-1 M
Q:
The first-order reaction, 2 N2O(g) -> 2 N2(g) + O2(g), has a rate constant equal to 0.76 s-1 at 1000 K. How long will it take for the concentration of N2O to decrease to 12% of its initial concentration?A) 0.62 sB) 2.8 sC) 6.3 sD) 8.4 s
Q:
The first-order reaction, SO2Cl2 -> SO2 + Cl2, has a rate constant equal to 2.20 10-5 s-1 at 593 K. What percentage of the initial amount SO2Cl2 will remain after 6.00 hours?A) 1.00%B) 37.8%C) 40.2%D) 62.2%
Q:
For a particular first-order reaction, it takes 24 minutes for the concentration of the reactant to decrease to 25% of its initial value. What is the value for rate constant (in s-1) for the reaction?
A) 2.0 10-4 s-1
B) 9.6 10-4 s-1
C) 1.2 10-2 s-1
D) 5.8 10-2 s-1
Q:
What is the overall reaction order for the reaction that has the rate law: Rate = k[O2][NO]2?
A) zero order
B) first order
C) second order
D) third order
Q:
For a reaction that follows the general rate law, Rate = k[A][B]2, what will happen to the rate of reaction if the concentration of B is increased by a factor of 3.00? The rate will
A) decrease by a factor of 1/9.00.
B) decrease by a factor of 1/3.00.
C) increase by a factor of 3.00.
D) increase by a factor of 9.00.
Q:
For a reaction that follows the general rate law, Rate = k[A][B]2, what will happen to the rate of reaction if the concentration of A is increased by a factor of 5.00? The rate will
A) decrease by a factor of 1/25.0.
B) decrease by a factor of 1/5.00.
C) increase by a factor of 5.00.
D) increase by a factor of 25.0.
Q:
The decomposition of dinitrogen pentoxide is described by the chemical equation2 N2O5(g) -> 4 NO2(g) + O2(g)If the rate of appearance of O2 is equal to 3.00 mol/min at a particular moment, what is the rate of disappearance of N2O5 at that moment?A) 0.750 mol/minB) 1.50 mol/minC) 6.00 mol/minD) 12.0 mol/min
Q:
The decomposition of dinitrogen pentoxide is described by the chemical equation2 N2O5(g) -> 4 NO2(g) + O2(g)If the rate of disappearance of N2O5 is equal to 1.60 mol/min at a particular moment, what is the rate of appearance of NO2 at that moment?A) 0.800 mol/minB) 1.60 mol/minC) 3.20 mol/minD) 6.40 mol/min
Q:
The reaction that occurs in a Breathalyzer, a device used to determine the alcohol level in a person's bloodstream, is given below. If the rate of appearance of Cr2(SO4)3 is 1.64 mol/min at a particular moment, what is the rate of disappearance of C2H6O at that moment?2 K2Cr2O7 + 8 H2SO4 + 3 C2H6O -> 2 Cr2(SO4)3 + 2 K2SO4 + 11 H2OA) 0.547 mol/minB) 1.09 mol/minC) 2.46 mol/minD) 4.92 mol/min
Q:
What is the activation energy for the destruction of ozone?A) 14 kJB) 392 kJC) 406 kJD) none of these
Q:
What is the activation energy for the formation of ozone?A) 14 kJB) 392 kJC) 406 kJD) none of these
Q:
Intermediates occur at which reaction stages?A) reaction stages 1 and 5B) reaction stages 2, 3, and 4C) reaction stages 2 and 4D) reaction stage 3
Q:
Consider a reaction that occurs by the following mechanism:A + BC -> AC + BAC + D -> A + CDThe potential energy profile for this reaction is shown below.Transition states occur at which reaction stages?A) reaction stages 1 and 5B) reaction stages 2, 3, and 4C) reaction stages 2 and 4D) reaction stage 3
Q:
The energy of reaction, E, is given by the difference in energy between which two reaction stages?A) reaction stage 2 reaction stage 1B) reaction stage 2 reaction stage 3C) reaction stage 1 reaction stage 3D) reaction stage 3 reaction stage 1
Q:
The activation energy for the forward reaction is given by the difference in energy between which two reaction stages?
A) reaction stage 2 reaction stage 1
B) reaction stage 2 reaction stage 3
C) reaction stage 1 reaction stage 3
D) reaction stage 3 reaction stage 1
Q:
What is the species present at reaction stage 3?
A) an intermediate
B) a product
C) a reactant
D) a transition state
Q:
What is the species present at reaction stage 2?
A) an intermediate
B) a product
C) a reactant
D) a transition state
Q:
Consider a reaction that occurs by the following one-step mechanism:A2 + B2 -> 2 ABThe potential energy profile for this reaction is shown below.What is the species present at reaction stage 1?A) an intermediateB) a productC) a reactantD) a transition state
Q:
Which of the elementary reactions shown above has a molecularity of three?A) elementary reaction (a)B) elementary reaction (b)C) elementary reaction (c)D) elementary reactions (a), (b), and (c)
Q:
Which of the elementary reactions shown above has a molecularity of two?
A) elementary reaction (a)
B) elementary reaction (b)
C) elementary reaction (c)
D) elementary reactions (a), (b), and (c)
Q:
Which of the elementary reactions shown above has a molecularity of one?A) elementary reaction (a)B) elementary reaction (b)C) elementary reaction (c)D) elementary reactions (a), (b), and (c)
Q:
What is the time required to achieve the molecular mixture in drawing (d)?A) 4 minB) 5 minC) 7 minD) 8 min
Q:
The following pictures represent the progress of a reaction in which two A molecules combine to give a more complex molecule A2, 2A ->A2.What is the order of reaction with respect to A?A) 0B) 1/2C) 1D) 2
Q:
Which drawing (a)-(d) represents the reaction mixture at t = 3 minutes?A) drawing (a)B) drawing (b)C) drawing (c)D) drawing (d)
Q:
Consider the first-order reaction A -> B in which A molecules (shaded spheres) are converted to B molecules (unshaded spheres).Which drawing (a)-(d) represents the reaction mixture at t = 2 minutes?A) drawing (a)B) drawing (b)C) drawing (c)D) drawing (d)
Q:
Consider the first-order decomposition of A molecules (shaded spheres) in two vessels of equal volume. How will the half-life of decomposition in vessel (a) be affected if the volume of the vessel is decreased by a factor of 2?A) decrease by 1/2B) increase by 2C) increase by 4D) stay the same
Q:
Consider the first-order decomposition of A molecules (shaded spheres) in two vessels of equal volume. How will the rate of decomposition in vessel (a) be affected if the volume of the vessel is decreased by a factor of 2? A) decrease by 1/2
B) increase by 2
C) increase by 4
D) stay the same
Q:
Consider the first-order decomposition of A molecules (shaded spheres) in two vessels of equal volume. What is the half-life of decomposition in vessel (b) relative to the half-life of decomposition in vessel (a)? A) half-life in vessel (b)/half-life in vessel (a) = 4:1
B) half-life in vessel (b)/half-life in vessel (a) = 2:1
C) half-life in vessel (b)/half-life in vessel (a) = 3:2
D) half-life in vessel (b)/half-life in vessel (a) = 1:1
Q:
Consider the first-order decomposition of A molecules (shaded spheres) in two vessels of equal volume. What is the half-life of decomposition in vessel (b) relative to the half-life of decomposition in vessel (a)? A) half-life in vessel (b)/half-life in vessel (a) = 4:1
B) half-life in vessel (b)/half-life in vessel (a) = 2:1
C) half-life in vessel (b)/half-life in vessel (a) = 3:2
D) half-life in vessel (b)/half-life in vessel (a) = 1:1
Q:
Consider the first-order reaction A ->B in which A molecules (unshaded spheres) are converted to B molecules (shaded spheres). Given the following pictures at t = 0 seconds and t = 100 seconds, which picture represents the number of A and B molecules remaining at 200 seconds?A) picture a)B) picture b)C) picture c)D) picture d)
Q:
Consider the first-order reaction A -> B in which A molecules (unshaded spheres) are converted to B molecules (shaded spheres). Given the following pictures at t = 0 seconds and t = 100 seconds, which picture represents the number of A and B molecules remaining at 300 seconds?A) picture a)B) picture b)C) picture c)D) picture d)
Q:
The following reaction is second order in A and first order in B:A + B ->Products Rate = k[A]2[B]What is the rate constant k of this reaction in vessel (b) relative to the rate constant k of this reaction in vessel (a)? Each vessel has the same volume. Shaded spheres represent A molecules, and unshaded spheres represent B molecules.A) rate constant k in vessel (b)/rate constant k in vessel (a) = 1:2B) rate constant k in vessel (b)/rate constant k in vessel (a) = 1:1C) rate constant k in vessel (b)/rate constant k in vessel (a) = 2:1D) rate constant k in vessel (b)/rate constant k in vessel (a) = 4:1
Q:
The following reaction is second order in A and first order in B:A + B -> Products Rate = k[A]2[B]What is the rate constant k of this reaction in vessel (b) relative to the rate constant k of this reaction in vessel (a)? Each vessel has the same volume. Shaded spheres represent A molecules, and unshaded spheres represent B molecules.A) rate constant k in vessel (b)/rate constant k in vessel (a) = 1:2B) rate constant k in vessel (b)/rate constant k in vessel (a) = 1:1C) rate constant k in vessel b)/rate constant k in vessel (a) = 2:1D) rate constant k in vessel (b)/rate constant k in vessel (a) = 4:1
Q:
The following reaction is second order in A and first order in B:A + B -> Products Rate = k[A]2[B]What is the rate constant k of this reaction in vessel (b) relative to the rate constant k of this reaction in vessel (a)? Each vessel has the same volume. Shaded spheres represent A molecules, and unshaded spheres represent B molecules.A) rate constant k in vessel (b)/rate constant k in vessel (a) = 1:2B) rate constant k in vessel (b)/rate constant k in vessel (a) = 1:1C) rate constant k in vessel (b)/rate constant k in vessel (a) = 2:1D) rate constant k in vessel (b)/rate constant k in vessel (a) = 4:1
Q:
The following reaction is first order in A and first order in B:A + B -> Products Rate = k[A][B]What is the rate constant k of this reaction in vessel (b) relative to the rate constant k of this reaction in vessel (a)? Each vessel has the same volume. Shaded spheres represent A molecules, and unshaded spheres represent B molecules.A) rate constant k in vessel (b)/rate constant k in vessel (a) = 1:2B) rate constant k in vessel (b)/rate constant k in vessel (a) = 1:1C) rate constant k in vessel (b)/rate constant k in vessel (a) = 2:1D) rate constant k in vessel (b)/rate constant k in vessel (a) = 4:1
Q:
The following reaction is first order in A and first order in B:A + B ->Products Rate = k[A][B]What is the rate constant k of this reaction in vessel (b) relative to the rate constant k of this reaction in vessel (a)? Each vessel has the same volume. Shaded spheres represent A molecules, and unshaded spheres represent B molecules.A) rate constant k in vessel (b)/rate constant k in vessel (a) = 1:2B) rate constant k in vessel (b)/rate constant k in vessel (a) = 1:1C) rate constant k in vessel (b)/rate constant k in vessel (a) = 2:1D) rate constant k in vessel (b)/rate constant k in vessel (a) = 4:1
Q:
The following reaction is first order in A and first order in B:A + B -> Products Rate = k[A][B]What is the rate constant k of this reaction in vessel (b) relative to the rate constant k of this reaction in vessel (a)? Each vessel has the same volume. Shaded spheres represent A molecules, and unshaded spheres represent B molecules.A) rate constant k in vessel (b)/rate constant k in vessel (a) = 1:2B) rate constant k in vessel (b)/rate constant k in vessel (a) = 1:1C) rate constant k in vessel (b)/rate constant k in vessel (a) = 2:1D) rate constant k in vessel (b)/rate constant k in vessel (a) = 4:1
Q:
The following reaction is second order in A and first order in B:A + B -> Products Rate = k[A]2[B]What is the initial rate of this reaction in vessel (b) relative to the initial rate of this reaction in vessel (a)? Each vessel has the same volume. Shaded spheres represent A molecules, and unshaded spheres represent B molecules present at the beginning of the reaction.A) rate in vessel (b)/rate in vessel (a) = 1:2B) rate in vessel (b)/rate in vessel (a) = 1:1C) rate in vessel (b)/rate in vessel (a) = 2:1D) rate in vessel (b)/rate in vessel (a) = 4:1
Q:
The following reaction is first order in A and first order in B:A + B -> Products Rate = k[A][B]What is the initial rate of this reaction in vessel (b) relative to the initial rate of this reaction in vessel (a)? Each vessel has the same volume. Shaded spheres represent A molecules, and unshaded spheres represent B molecules present at the beginning of the reaction.A) rate in vessel (b)/rate in vessel (a) = 1:2B) rate in vessel (b)/rate in vessel (a) = 1:1C) rate in vessel (b)/rate in vessel (a) = 2:1D) rate in vessel (b)/rate in vessel (a) = 4:1
Q:
The following reaction is first order in A and first order in B:A + B -> Products Rate = k[A][B]What is the initial rate of this reaction in vessel (b) relative to the initial rate of this reaction in vessel (a)? Each vessel has the same volume. Shaded spheres represent A molecules, and unshaded spheres represent B molecules present at the beginning of the reaction.A) rate in vessel (b)/rate in vessel (a) = 1:2B) rate in vessel (b)/rate in vessel (a) = 1:1C) rate in vessel (b)/rate in vessel (a) = 2:1D) rate in vessel (b)/rate in vessel (a) = 4:1
Q:
What is the rate law for this reaction?
A) Rate = k[A2]2
B) Rate = k[B2]2
C) Rate = k[A2][B2]
D) Rate = k[A2]2[B2]2
Q:
What is the overall order of reaction?
A) 0
B) 1
C) 2
D) 3
Q:
What is the order of reaction with respect to B2?
A) 0
B) 1
C) 2
D) 3
Q:
The relative initial rates of the reaction A2 + B2 -> products in vessels (a)-(d) are 1:1:4:4. Unshaded spheres represent A2 molecules, and shaded spheres represent B2 molecules present at the beginning of the reaction.What is the order of reaction with respect to A2?A) 0B) 1C) 2D) 3
Q:
Over the time interval 300 to 400 seconds, the rate of reaction with respect to A is [A]/t = 3.7 10-5 M/s. What is the rate of reaction with respect to A over the time interval 0 to 100 seconds?A) 0 M/sB) less than 3.7 10-5 M/sC) 3.7 10-5 M/sD) greater than 3.7 10-5 M/s
Q:
Over the time interval 300 to 400 seconds, the rate of reaction with respect to A is [A]/t = 3.7 10-5 M/s. What is the rate of reaction with respect to A over the time interval 700 to 800 seconds?A) 0 M/sB) less than 3.7 10-5 M/sC) 3.7 10-5 M/sD) greater than 3.7 10-5 M/s
Q:
Over the time interval 300 to 400 seconds, the rate of reaction with respect to A is [A]/t = 3.7 10-5 M/s. Over the same time interval what is the rate of reaction with respect to C, [C]/t?A) [C]/t = [A]/t = 3.7 10-5 M/sB) [C]/t = (1/4)([A]/t) = (1/4)(3.7 10-5 M/s) = 9.2 10-6 M/sC) [C]/t = (1/2)([A]/t) = (1/2)(3.7 10-5 M/s) = 1.8 10-5 M/sD) [C]/t = -(1/2)([A]/t) = -(1/2)(3.7 10-5 M/s) = -1.8 10-5 M/s
Q:
Over the time interval 300 to 400 seconds, the rate of reaction with respect to A is [A]/t = 3.7 10-5 M/s. Over the same time interval what is the rate of reaction with respect to B, [B]/t?A) [B]/t = [A]/t = 3.7 10-5 M/sB) [B]/t = (1/4)([A]/t) = (1/4)(3.7 10-5 M/s) = 9.2 10-6 M/sC) [B]/t = (1/2)([A]/t) = (1/2)(3.7 10-5 M/s) = 1.8 10-5 M/sD) [B]/t = -(1/2)([A]/t) = -(1/2)(3.7 10-5 M/s) = -1.8 10-5 M/s