can you double check my work? 7A +413A. rate equationPAPBRate = K[A] [B] [C]PB. Calculate[A]1. .72. 1.43..74. .7K[B]1.31.31.32.6+3CP (net[C].44Consider [A] : 142·003.Rate factor = (012) 44=(2) PA;Consider [C] : 143.006Rate factor =.00 32 = (2) Pc.8ЧConsider [B]: 14Rate factor = (-00) = 11 = (2) PBPA = 2Rate.00 3.012.006.003: PB = 0= 2: P₁ = 1Rate KLA] [B] [Rate= K[A] [4]

Here we are required to find the rate constant for the given reaction.

7A + 413 A. rate equation PA Rate = K[A] [B] [4] P B. Calculate [A] 1.7 2. 1.4 3..7 4. .7 [B] 1.3 1.3 1.3 2.6 K Rate factor= +3CP (net Consider [A] : 142 4=(2) PA [C] .4 4 8 Ч (1013) = 4 : PA = 2 Consider [B]: 154 Rate factor = (1003) = 1 1 = (2) PB Consider [C] : 143 Rate factor = (-005) = 2 2 = (2) Pc Rate .00 3 -012 .006 .003 : PB = 0 : P₂ = 1 Rate = K[A] [B] [C]' Rate = K[A]²[<]

7A + 413 A. rate equation PA Rate = K[A] [B] [4] P B. Calculate [A] 1.7 2. 1.4 3..7 4. .7 [B] 1.3 1.3 1.3 2.6 K Rate factor= +3CP (net Consider [A] : 142 4=(2) PA [C] .4 4 8 Ч (1013) = 4 : PA = 2 Consider [B]: 154 Rate factor = (1003) = 1 1 = (2) PB Consider [C] : 143 Rate factor = (-005) = 2 2 = (2) Pc Rate .00 3 -012 .006 .003 : PB = 0 : P₂ = 1 Rate = K[A] [B] [C]' Rate = K[A]²[<]

Principles of Instrumental Analysis

7th Edition

ISBN:9781305577213

Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Chapter32: Radiochemical Methods

Section: Chapter Questions

Problem 32.12QAP

See similar textbooks

Similar questions

Define stability from both a kinetic and thermodynamic perspective. Give examples to show the differences in these concepts.
The rate of photodecomposition of the herbicide piclo- ram in aqueous systems was determined by exposure to sunlight for a number of days. One such experiment produced the following results. (Data from R.T. Hedlun and C.R. Youngson, “The Rates of Photodecomposition of Picloram in Aqueous Systems," Fate of Organic Pesticides in tbe Aquatic Environment, Advances in Chemistry Series, #111, American Chemical Society (1972), 159—172.) Exposure Time, t (days) [Pidoram] (mol L_1) 0 4.14 X 10-6 7 3.70 X 10-6 14 3.31 X 10-6 21 2.94 X 10~6 28 2.61 X 10~6 35 2.30 X 10-6 42 2.05 X 10-6 49 1.82 X 10"6 56 1.65 X 10-6 Determine the order of reaction, the rate constant, and the half-life for the photodecomposition of picloram.
List at least four experimentally determined parameters that you, an experimenter, can define when exploring the hydrolysis of ethyl benzoate by aqueous sodium hydroxide.
A drug decomposes in the blood by a first-order process. A pill containing 0.500 g of the active ingredient reaches its maximum concentration of 2.5 mg/ 100 mL of blood. If the half-life of the active ingredient is 75 min, what is its concentration in the blood 2.0 h after the maximum concentration has been reached?
The plot below shows the number of collisions with a particular energy for two different temperatures. a. Which is greater, T2 or T1? How can you tell? b. What does this plot tell us about the temperature of the rate of a chemical reaction? Explain your answer.
The following experimental data were obtained for the reaction of \'I14* and NOf in acidic solution. NH/(aq) + NO2-(aq) — N;(g) + 2 H,O(f) INH/I (mol L1) [NO21 (mol L-1, Rate = A[NJ/At (mol L-1 s’) 0.0092 0.098 3.33 X IO"7 0.0092 0.049 1.66 X 10‘7 0.0488 0.196 3.51 X 10"6 0.0249 0.196 1.80 X 10-6 Determine the rate law for this reaction and calculate the rate constant.
Regular ?ights of supersonic aircraft in the stratosphere ale of concern because such aircraft produce nitric oxide, NO, as a byproduct in the exhaust of their engines. Nitric oxide reacts with ozone, and it has been suggested that this could contribute to depletion of the ozone layer. The reaction NO+O3NO2+O2 is first order with respect to both NO and O3 with a rate constant of 2.20107 L/mol/s. What is the instantaneous rate of disappearance of NO when [NO]=3.3106 M and [O3]=5.9107M?
Determine the average rate of change of BB from ?=0 st=0 s to ?=272 s.t=272 s. A⟶2BA⟶2B Time (s) Concentration of A (M) 0 0.7300.730 136136 0.4450.445 272272 0.1600.160 rateB= __________M/s
a. Express the rate in terms of change of concentration of A with respect to time where 2A + B -> products, rate = k[A]-1. b. Give the derived integrated rate law.
Use this data to determine the value of the rate constant. Ex # [A] (M) [B] (M) Rate (M/hr) 1 .240 .120 2.00 2 .120 .120 .500 3 .240 .0600 1.00 Question 4 options: 289 per hour 579 per hour 8.3 per hour 0.0144 per hour 69.4 per hour .00346 per hour 0.060 per hour 0.0173 per hour 17 per hour 0.12 per hour
Derive the integrated form of a third-order rate law v = kr[A]2[B] in which the stoichiometry is 2 A + B → P and the reactants are initially present in (a) their stoichiometric proportions ([B]0 = 12[A]0); (b) with B present initially in twice that amount ([B]0 = [A]0). Express your rate law in terms of [A]0, [B]0, and x, where [A] = [A]0 − 2x.
EXP [NO]-1/m [H2] .1M initial rate/ ms-1 1 0.10 0.10 1.23x10-3 2 0.10 0.20 1.23 x 10-3 3 0.20 0.10 4.92 x 10-3 calculate the rate when [NO] = 0.050M and [H2]=0.150M