The temperature dependence of the reaction rate constaot is given by theIn k- n A-Where:- rate conatantT= temperatureA = frequency factorE, - Energy of activationIn order to solve for the Energy of activation, B.. you must:Ste CnAdd the same expression to each side of the equation to leave the term that includes the variable by itself on the right-hand sideof the expression(Be sure that she anwer field changes from light jellow to dark yellow before releastng your answer)x + Ink+In A-RT- In AbStep TwoMultiply both sides of the equation by the same expression(Be sure that the answer field changes from light yellow to dark yellow before releasting your anver)x (la k - In A) =RTDrag and drop your selection from the following list to complete the anwer1.RTRTRTRT

The temperatare dependence of the reaction rate constact is givea by the lak-A- Where - rate conatant T-temperature A- frequency factor E- Energy of activation la order to solve for the Energy of activation, B.you must: S C Add the same expression to each side of the equation to leave the term that includes the variable by itself on the right-hand side of the expression (Be sure that she anwer fleid changes from light yellow to dark yellow before releastng your anwer) x +nk= / +In A- - In A Step Two Multiply both sudes of the equation by the same expressuon (Be sure that the anwer field changes from light yellow to dark yallow before releasing your antwer) x (la k- ln A)- Drag and drop your selection from the fellowing list to complete the answer 1. RT RT RT RT

The temperatare dependence of the reaction rate constact is givea by the lak-A- Where - rate conatant T-temperature A- frequency factor E- Energy of activation la order to solve for the Energy of activation, B.you must: S C Add the same expression to each side of the equation to leave the term that includes the variable by itself on the right-hand side of the expression (Be sure that she anwer fleid changes from light yellow to dark yellow before releastng your anwer) x +nk= / +In A- - In A Step Two Multiply both sudes of the equation by the same expressuon (Be sure that the anwer field changes from light yellow to dark yallow before releasing your antwer) x (la k- ln A)- Drag and drop your selection from the fellowing list to complete the answer 1. RT RT RT RT

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter8: Sampling, Standardization, And Calibration

Section: Chapter Questions

Problem 8.19QAP

See similar textbooks

Similar questions

(a) Most commercial heterogeneous catalysts are extremelyfinely divided solid materials. Why is particle sizeimportant? (b) What role does adsorption play in the actionof a heterogeneous catalyst?
The following data was obtained for the adsorption of an organic compound (S), on activated carbon from an aqueous solution of molar concentration Co, at 18 °C: Data: Molecular weight of S: 58 g/molWhich isotherm best represents the data: Langmuir, Freundlich, or BET?
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.
Assume that thermal decomposition of mercuric oxide, HgO, follows first-order kinetics. It can be followed by the production of oxygen gas as a product: 2HgO(s)2Hg(l)+O2(g) At a particular temperature, k=6.02104s1. If 1.00gram of HgO were present initially, how long would it take to produce a1.00mL of O2(g) at STP; b10.0mL of O2(g) at STP? STP = standard temperature and pressure for a gas.
An enzyme-catalyzed reaction is studied in the absence and presence of an inhibitor and the following data was obtained. [S] in mmoles/L Velocity in mmoles/L/min-1 No inhibitor With inhibitor 1.25 1.72 0.98 1.67 2.04 1.17 2.50 2.63 1.47 5.00 3.33 1.96 10.00 4.17 2.38 Calculate the Km of the enzyme in the reaction without inhibitor ________________________ Km’ of the enzyme in the reaction with inhibitor ________________________ Vmax of the uninhibited reaction ________________________ Vmax’ of the inhibited reaction ________________________
Collision theory depends on knowing the fraction of molecular collisions having at least the kinetic energy Ea along the line of flight. What is this fraction when (i) Ea = 20 kJ mol−1, (ii) Ea = 100 kJ mol−1 at (1) 350 K and (2) 900 K?
a particular reaction is proposed to be zero order. what plot would support this concclusion
Theoretically, it was concluded that the activation energy required to form one interatomic atom, (one void) of copper is approximately (4ev), assuming that this value is correct. Calculate the concentration of these defects (vacuum per cm^3) at the thermal equilibrium degree (1350k).
The compound α-tocopherol, a form of vitamin E, is a powerful antioxidant that may help to maintain the integrity of biological membranes. R.H. Bisby and A.W. Parker (J. Amer. Chem. Soc. 117, 5664 (1995)) studied the reaction of photochemically excited duroquinone with the antioxidant in ethanol. Once the duroquinone was photochemically excited, a bimolecular reaction took place at diffusion-limited rate. (a) Estimate the rate constant for a diffusion-limited reaction in ethanol. (b) The reported rate constant was 2.77 × 109 dm3 mol−1 s−1. Estimate the critical reaction distance if the sum of diffusion coefficients is 1 × 10−9 m2 s−1.
(a) Can an intermediate appear as a reactant in the firststep of a reaction mechanism? (b) On a reaction energyprofile diagram, is an intermediate represented asa peak or a valley? (c) If a molecule like Cl2 falls apart inan elementary reaction, what is the molecularity of thereaction?
The aqueous-phase decarboxylation of CH2NO2CO2H, CH2NO2CO2H CH3NO2(aq) + CO2(g), is studied at a certain temperature, giving the following data: Time (s) [CH2NO2CO2H] (M) 0.0e+00 0.100 1.0e-01 0.0466 2.0e-01 0.0217 3.0e-01 0.0101 4.0e-01 0.00473 Figure out whether this reaction is first-order or second-order with respect to the concentration of CH2NO2CO2H. Calculate the value of the rate constant. Pick the choice from below which gives the correct reaction order and value of the rate constant for this reaction.
Define the terms in. and limit the generality of. the expression In k, = In A- Ea /RT; why might there be deviations from the Arrhenius expression?