The reactant concentration in a second-order reaction was 0.590 M after 140 s and 2.70×10-2 M after 790 s. What is the rateconstant for this reaction?Express your answer with the appropriate units. Indicate the multiplication of units, as necessary, explicitly either with amultiplication dot or a dash.

Answered: Image /qna-images/answer/8d049cce-f489-4b81-8902-bea7185ae4a8.jpg

Answered: The reactant concentration in a…

The reactant concentration in a second-order reaction was 0.590 M after 140 s and 2.70×10-2 M after 790 s . What is the rate constant for this reaction?

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter12: Kinetics

Section: Chapter Questions

Problem 20E: The decomposition of acetaldehyde is a second order reaction with a rate constant of 4.71108...

See similar textbooks

Related questions

Q: 8. A first order reaction has a rate constant of 7.65 x 10² s'. If the initial concentration of…

A: The rate constant for the given first order reaction is = 7.65x10-2 s-1 The initial concentration of…

Q: At a given temperature, a first-order reaction has a rate constant of 2.1 × 10–3 s–1. How long will…

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

Q: What is the half-life for the decomposition of NOCl when the concentration of NOCl is 0.15 M? The…

A: Given information: The initial concentration of NOCl is 0.15 M The rate constant for second order…

Q: The rate constant for a first-order reaction is 3.18 y-1 . If the initial concentration of the…

A: Given: The rate constant for the reaction, (K)=3.18 y-1. The initial concentration, C0=0.54 M. The…

Q: A first-order reaction has a half-life of 11.0 seconds. What is the value of the rate constant? k…

A: A first-order reaction means that the rate of the reaction is directly proportional to the…

Q: Calculate the initial concentration for a first order reaction with a final concentration of 0.403…

A: GivenOrder of reaction = 1Final concentration = 0.403 Mk = 0.00721 min-1t = 43.2 minInitial…

Q: The reactant concentration in a second-order reaction was 0.520 M after 190 s and 4.00×10−2 M after…

A: For a 2nd order reaction, we know that the concentration and time are related as 1/[A] = 1/[A]0 +…

Q: The rate constant for a particular second-order reaction is 0.47 /(M×s). If the initial…

A: The speed, via which dissociation of reactants and formation of products occurs, is known as the…

Q: The reactant concentration in a first-order reaction was 6.80×10-2 M after 25.0 s and 2.10×10-3…

A: First order kinetic reaction are those in which the rate is direcdirectly proportional to the…

Q: After experimentally determining the order of this reaction, it was indeed found out to be 2nd order…

A: “Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: What is the rate constant of a first-order reaction when 20.0% of a reactant remains after 38.5 s?

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

Q: The rate constant for a first order reaction is 0.0640 1/s. What is the half-life for this reaction?

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: What are the units for the rate constant of a second order reaction? (s stands for seconds and M for…

A: Which one of the following is correct

Q: A second-order reaction has a half-life of 12 s when the initial concentration of reactant is 0.98…

Q: The reaction C2H5Cl →C2H4 + HCl is first order in C2H5Cl. The rate constant is 1.60 x 10-6/s. In an…

A: We have to predict the concentration after given time.

Q: The rate constant for a first-order reaction is 0.54 s¬1. What is the half-life of this reaction if…

A: • The values provided in the question are:- i) Rate constant of a first order reaction, k1 =…

Q: After a certain pesticide compound is applied to crops, its decomposition is a first-order reaction…

A: Half life :- The time required for half of reactants to convert into products is called half life…

Q: A particular first-order reaction has a rate constant of 0.0167 hr What is the half-life for this…

A: Given rate constant for first order reaction = 0.0167 hr-1 To find half life for this reaction.

Q: Consider the first-order reaction: ½ A2 → B+ C. The rate constant is found to be 3.15 x 10-³ min¹¹.…

A: In the given question we have to calculate the time required to convert 30% reactant A2 given data:…

Q: The isomerization of methyl isocyanide, CH3NC → CH3CN, follows first-order kinetics. The half-lives…

A: Given that, t1/2 at 199°C = 161 min t1/2 at 230°C = 12.5 min T1 = 199°C T2 = 230°C To calculate:…

Q: A second-order reaction has a half-life of 10 s when the initial concentration of reactant is 0.99…

Q: What is the rate constant of a first-order reaction if the half-life is 6.28 min?

Q: The rate constant of a second-order reaction is 2.94 x 10-2 M-1 s-1 and initial concentration is…

A: Given K = 2.94 x 10-2 M-1 s-1 initial Concentration = 0.300 M time = 81 s

Q: he half-life, t2, of a chemical reaction is proportional to the initial concentration of the…

A: Half Life (t1/2):

Q: What is the rate constant of a first-order reaction that takes 318 seconds for the reactant…

Q: How long would it take for the reactant of a first-order reaction todecrease to one-half its initial…

A: This problem can be solved by using the rate law for the first order reaction which is given as…

Q: What is the half-life for a particular reaction if the rate law is rate = (1001 M⁻¹*min⁻¹)[A]² and…

A: For zero order reaction, the units for rate constant = M.s–1. For first order reaction, the units…

Q: A chemical reaction that is first order in X is observed to have a rate constant of 2.1 x 10^-2s^-1.…

A: Integrated rate law for the first order reaction is, ln[A] = −kt + ln[A]0Where,k is the rate…

Q: . A reaction that is second-order in one reactant has a rate constant of 2.2 x 10-2 L/(mol • ). If…

A: Given : Rate constant of reaction = 2.2 X 10-2 M-1s-1. Initial concentration of reactant = 0.360 M…

Q: What is the half-life for a particular reaction if the rate law is rate = (1141 M⁻¹*min⁻¹)[A]² and…

A: Rate determining step is a step which is the slowest step of the reaction and the reactant involving…

Q: A particular reaction is found to be first order. The reactant has an initial concentration of 1.71…

A: For first-order reaction, the equation ln[A] = -kt + ln[A]0 depicts a straight line (y = mx + c)…

Q: The rate constant for this second‑order reaction is 0.570 M−1⋅s−1 at 300 ∘C. A⟶products How long, in…

A: Given, The rate constant, K = 0.570 M-1S-1 Initial concentration, [A]0 = 0.820 M Final…

Q: At a given temperature, a first-order reaction has a rate constant of 3.5 x 10-3s How long will it…

A: Here given, Rate constant for the first order reaction (k) = 3.5×10-3 s-1 We have to calculate the…

Q: What is the rate constant of a first-order reaction when 20.0% of a reactant remains after 48.0 s?

Q: The decomposition of N2O5 in solution in carbon tetrachloride is a first-order reaction. 2N2O5 →…

A: Given the first-order reaction: 2N2O5 → 4NO2 + O2 The integrated-rate law equation for studying…

Q: What is the half-life for a particular reaction if the rate law is rate = (1231 M*min⁻¹)[A]⁰ and the…

Q: 2. The rate constant for a first order reaction, SO₂Cl₂ → SO₂ + Cl₂ at 600 K is 2.2 x 10-5 s-¹. What…

Q: concentration

Q: The reactant concentration in a second-order reaction was 0.230 MM after 230 s and 4.20×10−2 MM…

Q: A first-order reaction has a half-life of 1.34 x 103 hours. If the initial concentration of reactant…

A: Half life of the reaction is the time at which half of the reactant get reduced.

Q: One example of a first-order reaction is the isomerization of hydrogen isocyanide to hydrogen…

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: The decomposition of N2O5 in solution in carbon tetrachloride is a first-order reaction. 2N2O5 →…

Q: The rate constant for this second‑order reaction is 0.640 M−1⋅s−1 at 300 ∘C. A⟶products How long, in…

Q: The reactant concentration in a second-order reaction was 0.230 M after 230 s and 4.20×10−2 M after…

A: The rate law for a second order reaction is given below,

Q: What is the rate constant of a first-order reaction that takes 459 seconds for the reactant…

A: The time taken during a reaction to reduce the concentration of a reactant to half of its initial…

Q: The rate constant for a first-order reaction is 0.77 s^-1. What is the half-life of this reaction if…

A: The following equation can be used to calculate the half-life of a first-order reaction. t12=ln…

Question

The reactant concentration in a second-order reaction was 0.590 M after 140 s and 2.70×10-2 M after 790 s. What is the rate
constant for this reaction?
Express your answer with the appropriate units. Indicate the multiplication of units, as necessary, explicitly either with a
multiplication dot or a dash.

Expert Solution

This question has been solved!

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

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

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?
Explain why half-lives are not normally used to describe reactions other than first order.
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)?
The decomposition of N2O5 in CCl4 is a first-order reaction. If 2.56 mg of N2O5 is present initially and 2.50 mg is present after 4.26 minutes at 55 C, what is the value of the rate constant, k?
The decomposition of acetaldehyde is a second order reaction with a rate constant of 4.71108 L/mol/s. What is the instantaneous rate of decomposition of acetaldehyde in a solution with a concentration of 5.55104M?
From the given data, use a graphical method to determine the order and rate constant of the following reaction: 2XY+Z Time (s) 5.0 10.0 15.0 20.0 25.0 30.0 35.0 40.0 [X](M) 0.0990 0.0497 0.0332 0.0249 0.0200 0.0166 0.0143 0.0125
What is the difference between average rate, initial rate, and instantaneous rate?
If you know some calculus, derive the integrated first-order rate law for the reaction by following these steps: Define the reaction rate in terms of [A]. Write the rate law in terms of [A], k, and t. Separate variables in the rate law. Integrate the rate law. Write the integrated equation in the form . Derive the half-life as was done in Section 11-3c.
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.