For the first-order reaction N2O5( g) → 2 NOX8) + 0x8) 2 NO2{g) + t/2= 20.5 h at 20°C and 3.5h at 40°C. (a) Calculate the activation energy of this reaction. (b) If the Arrhenius constant A = 2.5 x 1015 s', determine the value of k at 50°C.

For the first-order reaction N2O5( g) → 2 NOX8) + 0x8) 2 NO2{g) + t/2= 20.5 h at 20°C and 3.5h at 40°C. (a) Calculate the activation energy of this reaction. (b) If the Arrhenius constant A = 2.5 x 1015 s', determine the value of k at 50°C.

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter11: Rate Of Reaction

Section: Chapter Questions

Problem 103QAP

See similar textbooks

Related questions

Q: A certain first-order reaction (A→products) has a rate constant of 9.30x10-3 s-1 at 45 °C. How many…

Q: N205(g) – 2 NO2(g) + 1/2 O2(g) is measured at different temperatures, with the following rate…

A: The rate of the reaction N2O5(g) → 2 NO2(g) + 1/2 O2(g)

Q: A first-order reaction has rate constants of 4.6 x 10-2 s-1 and 5.6 x 10-2 s-1 at 0°C and 20.°C,…

Q: k (1/M s) t (°C) 1.87 X 10-3 600 0.0113 650 0.0569 700 0.244 750 Determine graphically the…

A: A numerical problem based on chemical kinetics, which is to be accomplished.

Q: (a) Define the following terms:(i) Collision frequency(ii) Rate constant (k)(b) The rate constant of…

A: Hi, since you have posted multiple questions and did not mention which question you want us to solve…

Q: 1) A reagent used in organic synthesis, decomposes in acidic solution by following a first-order…

A: Given first order reaction is : A (aq) ----------------> B (aq) + CO2 (g) Given half-life of the…

Q: What is the rate constant of a first-order reaction when 20.0% of a reactant remains after 60.0 s?

Q: The reactant concentration in a first-order reaction was 7.10×10−2 M after 30.0 s and 5.60×10−3 M…

A: The equation for first order reaction is, A - concentration at time t Ao – initial concentration k…

Q: Consider the decomposition of A to certain products, initially at 1.0 M. Determine the rate constant…

Q: A reaction of importance in the formation of smog is that between ozone and nitrogen monoxide…

A: The rate is given as Rate = K×[O3][NO] initially, we are given concentration of: [O3] = 4.40 × 10-6…

Q: 22.5 A first-order decomposition reaction is observed to have the following rate constants at the…

A: Given information:

Q: What is the half-life (in seconds) of a zero-order reaction which has an initial reactant…

A: The half-life for the zero-order reaction is calculated as shown in equation (1) where [R]o is…

Q: What is the best way to ascertain that a reaction is first order?

A: if it the reaction is a first-order reaction, plot the natural logarithm of a reactant concentration…

Q: Hydrogen peroxide decomposes spontaneously to yield water and oxygen gas according to the reaction…

A: The equation that describes the relationship between rate of a reaction and temperature is,…

Q: At 400 K, the half-life for the decomposition of a sample of a gaseous compound initially at a…

A: Given: Decomposition of a gaseous sample.

Q: In a study of the enzyme-catalysed oxidation of ethanol, the molar concentration of ethanol…

A: Given The reaction is a first order reaction Initial concentration = 220 mmol/dm3 Final…

Q: The enzyme urease catalyzes the reaction of urea,(NH2CONH2), with water to produce carbon dioxide…

A: a) The reaction taking place is as shown below NH2CONH2 + H2O ------catalyst--------> 2 NH3 +…

Q: The formation of NOCI from NO in the presence of a large excess of chlorine is pseudosecond-order in…

A: Given that the below reaction is of pseudo-second-order reaction in NO. 2NO(g) + Cl2(g) → 2NOCl(g)…

Q: A biochemist studying the breakdown of the insecticide DDT finds that it decomposes by a first-…

Q: The given first-order reaction A→B, has a rate constant of 1.60 x 10-2 s1 at 165°C and 6.54 x 10-'…

Q: The rate constant for the reaction PCl3 (g) + Cl2 (g) → PCl5 (g) is 1.3 x 103 M/min at 515 K, and…

A: Given, Reaction is, The rate constant for the reaction at 515 K…

Q: At 378.5oC, the half-life for the first order thermal decomposition of ethylene oxide is 363 min,…

A: The half-life of a reaction is the time taken for the reactant to reduce to half its initial value…

Q: The rate constant of a reaction at 32 °C is measured to be 0.055/s. If the frequency factor is 1.2 ×…

Q: . For the following consecutive first order reactions K =2.0s- K =2.0s →Y the time (in seconds)…

A: Here it is given a first order consecutive reaction.we will find the time required for Y to reach…

Q: A first-order reaction has a rate constant k = 0.0815 s-1 at a temperature of 65oC and a rate…

A: To calculate activation energy of the reaction in kJ/mole with the given rate constant at different…

Q: The rate constant for the reaction CH2=CH2(g) + H2(g) → CH3−CH3(g) was…

A: Activation energy can be calculated by the following equation. lnK2K1=EaR1T1-1T2T1=first…

Q: A certain second-order reaction (B→products) has a rate constant of 1.10×10−3 M−1⋅s−1 at 27 ∘C and…

Q: The rate constant of a reaction at 32 °C is 0.055/s. If the frequency factor is 1.2 * 10 13/s, what…

A: The below formula is used to determine the value of the activation barrier.

Q: The age of wine can be determined by measuring the trace amount of radioactive tritium, 3H, present…

A: N(t)=N0 exp[-k t]N(t) is the number of radioactive nuclei remaining at time t, N0 is the initial…

Q: The first-order decomposition of N,0 at 1000 K has a rate constant of 0.7 N20 after 9.6 s?

A: Ans. Option A is correct. Solution: Final concentration at time t can be calculated by applying…

Q: What is the rate constant of a first-order reaction when 20.0% of a reactant remains after 30.0 s?

A: Since we know that the relationship between the concentration of reactant i.e [A] and time for a…

Q: The age of wine can be determined by measuring the trace amount of radioactive tritium, ³H, present…

A: N(t)=N0 exp[-k t]N(t) is the number of radioactive nuclei remaining at time t, N0 is the initial…

Q: The first-order rate constant for reaction of a particular organic compound with water varies with…

A: We are given the following data for the first-order reaction: Temperature(K) 300 320 340 355…

Q: The reactant concentration in a first-order reaction was 9.00×10−2 MM after 15.0 ss and 9.20×10−3 MM…

A: The equation for first order reaction is:

Q: 6.17 The elimination of carbon dioxide from pyruvate ions by a decarboxylase enzyme was monitored by…

A: Given: Initial concentration of pyruvate ions in 100 mL is 3.23 mmol/L Pressure of carbon dioxide =…

Q: The age of wine can be determined by measuring the trace amount of radioactive tritium, 3H, present…

A: The half-life of a reaction is the time taken for the reactant to reduce to half its initial value…

Q: You are studying the rate of the reaction 2A → B and have obtained measurements of the concentration…

A: The order of the reaction with respect to a particular reactant is determined by observing their…

Q: A certain first-order reaction has a rate constant of 2.50×10−3 s^−1. How long will it take for the…

Q: The rate constant for a first-order reaction is 1.4 x 10-2s-1 at 646 K and 3.5 x10-2s-1 at 824 K.…

A: the relation between the rate constant and temperature is log(k2/k1) = Ea/2.303 R [(T2-T1)/T1T2]…

Q: Determine the activation energy for the reaction.

A: Arrhenius equation for the rate constant where, k = rate constant A = exponential factor Ea =…

Q: A certain second-order reaction (B→products) has a rate constant of 2.00×10−3 M^−1⋅s^−1 at 27∘C and…

Q: What is the effective rate constant [in units that combine M and min] for the reaction with rate law…

A: Given-> v = k[A][B]2 k = 0.54 M-2.min-1 Initial concentration of B = 3.7 M Initial concentration…

Q: A reaction having an activation energy of 55.1 kJ/mol has a rate constant of 4.2 x 10-8 s-1 when the…

Q: The age of wine can be determined by measuring the trace amount of radioactive tritium, 3H, present…

Q: Hydrogen peroxide decomposes spontaneously to yield water and oxygen gas according to the reaction…

A: The rate of a reaction is the speed at which the reaction proceeds. The rate of a reaction can be…

Q: A first-order reaction has a rate constant of 7.5 x 103 s. How many seconds does it take for the…

Q: The thermal decomposition of phosphine into phosphorus and hydrogen is a first order reaction with a…

A: Rate of reaction represents the change of concentration of a reactant or a product with respect to…

Q: A) The reactant concentration in a zero-order reaction was 0.100 mol L−1mol L−1 after 140 ss and…

A: Hello. Since the question contains multiple parts, the first part is solved (A & B). In case the…

Question

For the first-order reaction
N2O5( g) →
2 NOX8) + 0x8)
t/2= 20.5 h at 20°C and 3.5h at 40°C.
(a) Calculate the activation energy of this reaction.
(b) If the Arrhenius constant A= 2.5 x 10'3 s',
determine the value of k at 50°C.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Step by step

Solved in 4 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

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 frequency factor A is 6.31 108 L mol1 s1 and the activation energy is 10. kJ/mol for the gas-phase reaction NO(g)+O3(g)NO2(g)+O2(g) which is important in the chemistry of stratospheric ozone depletion. (a) Calculate the rate constant for this reaction at 370. K. (b) Assuming that this is an elementary reaction, calculate the rate of the reaction at 370. K if [NO] = 0.0010 M and [O3] = 0.00050 M.
The initial concentration of the reactant in a tirst-order reaction A —» products is 0.64 rnol/L and the half-life is 30.0 s. Calculate the concentration of the reactant exactly 60 s after initiation of the reaction. How long would it take for the concentration of the reactant to drop to one-eighth its initial value? How long would it take for the concentration of the reactant to drop to 0.040 mol/L?
The decomposition of azomethane, (CH3)2N2, to nitrogen and ethane gases is a first-order reaction, (CH3)2N2(g)N2(g)+C2H6(g). At a certain temperature, a 29-mg sample of azomethane is reduced to 12 mg in 1.4 s. (a) What is the rate constant k for the decomposition at that temperature? (b) What is the half-life of the decomposition? (c) How long will it take to decompose 78% of the azomethane?
Define stability from both a kinetic and thermodynamic perspective. Give examples to show the differences in these concepts.
Experiments have shown that the average frequency of chirping by a snowy tree cricket (Oecanthus fultoni) depends on temperature as shown in the table. Chirping Rate (per min) Temperature (C) 178 25.0 126 20.3 100. 17.3 What is the apparent activation energy of the process that controls the chirping? What is the rate of chirping expected at a temperature of 7.5C?
The thermal decomposition of diacetylene, C4H2, was studied at 950 C. Use the following data (K. C. Hou and H. B. Palmer, Journal of Physical Chemistry. Vol. 60, p. 858, 1965) to determine the order of the reaction.
The decomposition of NO2(g) occurs by the following bimolecular elementary reaction: 2NO2(g)2NO(g)+O2(g) The rate constant at 273 K is 2.3 1012 L/mol s, and the activation energy is 111 kJ/mol. How long will it take for the concentration of NO2(g) to decrease from an initial partial pressure of 2.5 atm to 1.5 atm at 500. K? Assume ideal gas behavior.
(Section 11-5) A rule of thumb is that for a typical reaction, if concentrations are unchanged, a 10-K rise in temperature increases the reaction rate by two to four times. Use an average increase of three times to answer the questions below. (a) What is the approximate activation energy of a typical chemical reaction at 298 K? (b) If a catalyst increases a chemical reactions rate by providing a mechanism that has a lower activation energy, then what change do you expect a 10-K increase in temperature to make in the rate of a reaction whose uncatalyzed activation energy of 75 kJ/mol has been lowered to one half this value (at 298 K) by addition of a catalyst?
The acid-catalyzed iodination of acetone CH3COCH3(aq) + I2(aq) CH3COCH2I(aq) + HI(aq) is a common laboratory experiment used in general chemistry courses to teach the method of initial rates. The reaction is followed spectrophotometrically by the disappearance of the color of iodine in the solution. The following data (J. P. Birk and D. L Walters, Journal of Chemical Education, Vol. 69, p. 585, 1992) were collected at 23 C for this reaction. Determine the rate law for this reaction.
The hydrolysis of the sugar sucrose to the sugars glucose and fructose, C12H22O11+H2OC6H12O6+C6H12O6 follows a first-order rate equation for the disappearance of sucrose: Rate =k[C12H22O11] (The products of the reaction, glucose and fructose, have the same molecular formulas but differ in the arrangement of the atoms in their molecules.) (a) In neutral solution, k=2.11011s1 at 27 C and 8.51011s1 at 37 C. Determine the activation energy, the frequency factor, and the rate constant for this equation at 47 C (assuming the kinetics remain consistent with the Arrhenius equation at this temperature). (b) When a solution of sucrose with an initial concentration of 0.150 M reaches equilibrium, the concentration of sucrose is 1.65107M . How long will it take the solution to reach equilibrium at 27 C in the absence of a catalyst? Because the concentration of sucrose at equilibrium is so low, assume that the reaction is irreversible. (c) Why does assuming that the reaction is irreversible simplify the calculation in pan (b)?