Practice ProblemATTEMPT
Show that the following two-step mechanism is consistent with the experimentally determined rate law of rate
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Chemistry
- If the rate law for the reaction A ⟶Products is rate = k[A], calculate the value of k from the following data: [A] (M) Initial Rate (M/s) 0.10 0.015 (A)6.7 s-1 (B)0.015 s-1 (C)0.15 s-1 (D)67 s-1arrow_forwardQuestion 3 of 8 Submit What are the units for the rate constant of a reaction with the rate law, Rate = k[A][B]? %3D A) s-1 B) M s-1 С) М-1 s-1 D) M-2 s-1 E) s M-1arrow_forwardWhen [A] is doubled, the rate doubles; when [B] is doubled, the rate quadruples; when [C] is doubled, the rate does not change. How would the rate change if the concentration of A and C are doubled when the concentration of B is tripled? A(g) + B(g) + C(g) => products A) The rate decreases by a factor of 4. B) The rate decreases by a factor of 2. C) The rate increases by a factor of 2. D) The rate increases by a factor of 4. E) The rate increases by a factor of 8. F) The rate increases by a factor of 16. G) The rate increase by a factor of 18. H) The rate does not change.arrow_forward
- Sulfur dioxide is oxidized to sulfur trioxide in the following sequence of reactions:2 SO2 (g) + 2 NO2 (g) ⇄ 2 SO3 (g) + 2 NO (g)2 NO (g) + O2 (g) ⇄ 2 NO2 (g)(4a): What is the overall reaction?(4b): Identify any molecule that acts as a catalyst or intermediate in this reactionarrow_forwardThe initial rate of the reaction 2 A + B → C + D was studied in a series of kinetics experiments. Trial Conc A (M) Conc B (M) Initial Rate (M/s) 1 0.300 0.100 0.000704 2 0.900 0.100 0.006334 3 0.900 0.300 0.006334 What is the experimental rate law for this reaction? Question 16 options: A) Rate = k[B]2 B) Rate = k[A]2 C) Rate = k[A] D) Rate = k[A]2[B] E) Rate = k[A][B]arrow_forwardSulfur dioxide reacts with carbon monoxide according to the following balanced reaction. The initial rate of reaction was measured in a series of experiments at 25 ∘C∘C as shown in the table below. SO2(g)+3 CO(g) → 2 CO2(g)+SCO(g) Experiment [SO2], M[SO2], M [CO], M[CO], M Initial reaction rate 1 0.0100 0.0100 0.0291 2 0.0250 0.0250 0.1150 3 0.0250 0.0100 0.0460 Part A Determine the overall order for the reaction. Enter your answer as a numerical value. Part B Calculate the value of the rate constant for the reaction. Express your answer with three significant figures. Do not include the unit. Part C What is the correct unit of the rate constant? Select one option. M−1.5⋅s−1M−1.5⋅s−1 M−2⋅s−0.5M−2⋅s−0.5 M−0.5⋅s−1M−0.5⋅s−1 M⋅s−1M⋅s−1 M−1⋅s−1M−1⋅s−1 None of the above are correct. Calculate the intial rate of appearance of carbon dioxide when 0.0500 MM SO2SO2 and 0.0675 MM COCO are…arrow_forward
- Sulfur dioxide reacts with carbon monoxide according to the following balanced reaction. The initial rate of reaction was measured in a series of experiments at 25 ∘C∘C as shown in the table below. SO2(g)+3 CO(g) → 2 CO2(g)+SCO(g) Experiment [SO2], M[SO2], M [CO], M[CO], M Initial reaction rate 1 0.0100 0.0100 0.0291 2 0.0250 0.0250 0.1150 3 0.0250 0.0100 0.0460 Part A Determine the overall order for the reaction. Calculate the value of the rate constant for the reaction. Express your answer with three significant figures. Do not include the unit. Calculate the intial rate of appearance of carbon dioxide when 0.0500 MM SO2SO2 and 0.0675 MM COCO are reacted. Express your answer with three significant figures and include the unit.arrow_forwardA reaction was experimentally determined to follow the rate law, Rate = k[A] 2 where k = 0.456 s -1M -1. Starting with [A] o = 0.500 M, how many seconds will it take for [A] t = 0.250 M? answer options 2.85 x 10 -2 s 1.14 x 10 -1 s 5.48x10 -1 s 1.52 s 4.39 sarrow_forwardCurrent Attempt in Progress The reaction 2A + 2B M+Nhas the rate law: Rate = k[A]?. At 25°C, k = 0.0376 L mol1s1. If the initial concentrations of A and B are 0.387 M and O.459 M, respectively Your answer is correct. (a) What is the half-life of the reaction? 68.7 seconds Hint Your answer is incorrect. (b) What will be the concentrations of A and B after 30.0 minutes? [A] = i ! M [B] = i M Hintarrow_forward
- Consider the hypothetical reaction: 2A + B D which is believed to follow this mechanism: Step (1): A+ A C Step (2): C+B→ D where Step (1) is the slowest step. The reaction is also known to be exothermic. Which of the following reaction coordinate diagrams is most likely the correct one for this reaction? in Progress (A) Progress (B) Progress (C) Arogress CE) (D) a Chp 近arrow_forwardQuestion I (from the University of Arizona) Nitric oxide (NO) reacts with H2 to form N2O and H2O. It is known that there are two elementarysteps to this reaction:Step I: NO(g) + NO(g) ---> N2O2(g)Step II: N2O2(g) + H2(g) ---> N2O(g) + H2O(g)The measured rate law for this overall reaction is:Rate = k[NO]2 [H2]What can we conclude about the above elementary reaction steps based on this rate law?(A) Steps I & II are about the same rate.(B) Step I is much faster than step II.(C) Step II is much faster than step I.(D) Not enough information to tell. Question II (from the University of Guelph)Consider the possible mechanisms for the following reaction:2NO + O2 → 2NO21.NO(g) + NO(g) → N2O2(g) (slow)N2O2(g) + O2(g) → 2NO2(g) (fast)2. NO(g) + NO(g) → N2O2(g) (fast)N2O2(g) + O2(g) → 2NO2(g) (slow)3.NO(g) + O2(g) → NO2(g) + O(g) (slow)NO(g) + O(g) → NO2(g) (fast)Given that the empirical rate law for this reaction isfound to be rate = k[NO]2[O2]. Which mechanism(s) is consistant with the…arrow_forwardIdentify the order of the following reactions H Instructions Categorize the following rate laws with corresponding overall order of the reaction. F G E A B C D Rate = K[CO₂] Rate = k Rate = K[HC]2 Rate = K[NO]2[0₂] Rate = K[NO2][F2] Rate = K[SO3] Rate = K[H₂][NO]2 Rate = K[SO₂Cl₂] Which of the reaction(s) are first-order reaction(s)? Select all that apply. Incorrect will be penalized. choices 0000 I FOU EA 000 Which of the reaction(s) are second-order reaction(s)? Select all that apply. Incorrect choices will be penalized. 000000 IVO E CAarrow_forward
- Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning