The rate constant, k, for a first-order reactionN2O5 → NO2 + NO3is ,16 x 10s at 0°C. The activation energy of this reaction is88.0 kJ/mol. Determine the value of k at 2°C !

Answered: Image /qna-images/answer/05fc1964-4871-45c7-b90a-a007c04ddfe6.jpg

Answered: The rate constant, k, for a first-order…

The rate constant, k, for a first-order reaction N2O5 → NO2 + NO3 is ,16 x 103s at 0°C. The activation energy of this reaction is 88.0 kJ/mol. Determine the value of k at 2°C !

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter11: Chemical Kinetics: Rates Of Reactions

Section: Chapter Questions

Problem 31QRT

See similar textbooks

Related questions

Q: Consider the mechanism. Step 1: 2A B+C slow Step 2: B +C → E fast Overall: 2 A → E Determine the…

A: Given Step 1 2A -------> B + C ( Slow step ) step 2 B + C -----> E…

Q: The rate constant for this first-order reaction is 0.640 s at 400 °C. A products How long, in…

Q: The reactant concentration in a zero-order reaction was 6.00×10−2 M after 115 s and 4.00×10−2 M…

Q: A first order process has an experimentally determined rate constant of 6.0 x104s! at 500°C. If the…

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

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 decomposition of sulfuryl chloride (SO2Cl2) is a first-order process. The rate constant for the…

A: The integrated equation for first order reaction is expressed as :

Q: The rate constant for this first-order reaction is 0.770 s- at 400 °C. A → products How long, in…

Q: The rate constant for this second‑order reaction is 0.540 M−1⋅s−1 at 300 ∘C. A⟶products How…

A: Given: Reaction is second order. Rate constant of the reaction = 0.540 M-1s-1. And the concentration…

Q: The rate constant for this first-order reaction is 0.300 s- at 400 °C. products How long, in…

Q: Dinitrogen tetraoxide, N2O4, decomposes to nitrogen dioxide, NO2, in a first-order process. If k=…

Q: Molecular iodine, I2(g), dissociates into iodine atoms at 625 K with a first-order rate constant of…

A: The integrated rate law for first-order reaction can be given as,

Q: The rate constant for this zero-order reaction is 0.0320 M s- at 300 C. A products How long (in…

A: Zero order reaction :- Reaction in which rate is independent of concentration of reactants is called…

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

Q: What is the rate constant?

A: The required relation is given below.

Q: A reaction has a rate constant of k = 2.55 s¹. What is the overall reaction order? S

A: Given : for a reaction the value of rate constant (K) = 2.55 s-1 To determine : overall reaction…

Q: Hydrogen peroxide decomposes spontancously to yield water and oxygen gas-tecording to the reaction e…

A: T = 2792.86K or = 2793K

Q: For the reaction of BF, (g) + NH, (g) F,BNH, (g) the second-order rate constant k at 100° C is 3.41…

A: Given chemical Reaction is of 2nd order reaction. Rate constant (k) = 3.41 M-1S-1 Initial…

Q: 2- Methyl isocyanide, CH3NC, isomerizes, when heated, to give acetonitrile (methyl cyanide), CH3CN.…

A: Half life is the time required to reduce the original concentration into it's half. Half life of…

Q: 1.) Write the FULL reaction rate for the following chemical formula: 5H;C,0,(ag) + 2KMNO,(aq) +…

A: The given reaction is represented as follows:

Q: The rate constant of a first-order reaction is 4.60 x 104/s at 350°C. If the activation energy is…

A: Given that: Rate constant (k1) = 4.60×10-4 s-1 Temperature (T1) = 350°C = 623K Activation energy…

Q: The decomposition of ethyl iodide in the gas phase to produce ethylene and hydrogen iodide is a…

Q: The rate constant for this first-order reaction is 0.0330 s at 400 C. A products After how many…

A: Given reaction: A → products The rate constant of this reaction = 0.0330 s-1 We have to calculate…

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

A: The first order reaction is kinetic reaction are those reaction where the rate of the reaction is…

Q: Methyl isocyanide, CH3NC, isomerizes, when heated, to give acetonitrile (methyl cyanide), CH3CN.…

A: First-order reaction:The rate of the first-order reaction depends on the concentration of one…

Q: The decomposition of sulfuryl chloride (SO₂Cl₂) is a first-order process. The rate constant for the…

A: Given: Rate constant (k) is 4.5×10-2 s-1. Initial pressure is 335 torr. Time is 62 s.

Q: rate constant

Q: Consider the mechanism. Step 1: 2 A B+ C slow Step 2: B +C E fast Overall: 2A E Determine the rate…

A: STEP 1 : 2A ------> B + C ....................SLOW STEP 2 : B + C ------->…

Q: The rate constant for this first‑order reaction is 0.0130 s−1 at 400 ∘C. A⟶products After how…

Q: The rate constant for this first-order reaction is 0.0870 s- at 400 °C. A - products After how many…

A: Given data Order of reaction = 1 Rate constant value : k = 0.0870 s-1 Final concentration [A] =…

Q: The concentration of a particular reactant is doubled (all other concentrations are constant) and…

Q: A reaction has a rate constant of k = 2.55 s¹. What is the overall reaction order?

A: Given :- rate constant (K) = 2.55 s-1 To determine :- overall reaction order

Q: Cyclobutane, C4H8, decomposes when heated to ethylene, C2H4. The reaction is first order. In an…

A: Cyclobutane, C4H8, decomposes when heated to ethylene, C2H4.The reaction is first order.

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: The initial concentration of a reactant is 1.58 M for a second-order reaction. It takes 12.3 minutes…

A: The integrated rate law for second order reaction is as follows,

Q: Chloroethane decomposes at elevated temperatures accord- ing to the reaction C:HSCI(g) → C2H4 (g) +…

A: The integrated rate law for first order reaction is given by, k=1tln[A]0[A] where t is the time in…

Q: Consider the mechanism. Step 1: Step 2: 2A B slow B +C D fast Overall: 2 A +C D Determine the rate…

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

Q: For a certain reaction, the frequency factor A is 3.4 x 10° s and the activation energy is 15.9…

Q: 2. The reaction H2 (g) + 2 NO (g) + H,O (g) is studied at a certain temperature N,0 (g) by…

A: Introduction : Rate law can be defined as the representation of rate of reaction in terms of…

Q: The rate law for the reaction: H2(g) + 2NO(g) ⟶ N2 O(g)…

A: Given information, The balanced chemical equation is given below, H2(g) + 2NO(g) ⟶ N2 O(g) + H2O(g)…

Q: Methyl isocyanide, CH3NC, isomerizes, when heated, to give acetonitrile (methyl cyanide), CH3CN.…

A: The reaction follows the first-order reaction kinetics. For the first-order reaction, the rate of…

Q: The first order reaction SO,CI, (g) --> SO2 (g) + Cl2 (g) has a rate constant of 2.90 X 104 s at a…

A: Ans

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: The rate law for the chemical reaction H2(g)+2NO(g) ⟶ N2O(g)+H2O(g) has…

A: The rate law (also known as the rate equation) for a chemical reaction is an expression that…

Q: The rate constant for this zero-order reaction is 0.0240 M · s-l at 300 °C. A → products How long…

Q: The rate constant for this zero-order reaction is 0.0170 M · s-l at 300 °C. A → products How long…

A: Consider the given zero-order reaction as; A → products Given information is as follows: Initial…

Q: A chemistry graduate student is studying the rate of this reaction: 2H,РО, (аg) — Р,0, (ag) +зн,о…

A: Since the rate of reaction depends only on the reactant Hence for the above reaction we can write…

Question

The rate constant, k, for a first-order reaction
N2O5 → NO2 + NO3
is ,16 x 10s at 0°C. The activation energy of this reaction is
88.0 kJ/mol. Determine the value of k at 2°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

VIEW

Step 2

VIEW

Step by step

Solved in 2 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

At 573 K, gaseous NO2(g) decomposes, forming NO(g) and O2(g). If a vessel containing NO2(g) has an initial concentration of 1.9 102 mol/L, how long will it take for 75% of the NO2(g) to decompose? The decomposition of NO2(g) is second-order in the reactant and the rate constant for this reaction, at 573 K, is 1.1 L/mol s.
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?
11.32 The following experimental data were obtained for the reaction 2A + 3 B—C + 2D [A](mol L 1) [B](mol L ’) Rate = A(C]/Af (mol L-1 s-1) 0.127 0.15 0.033 0.127 0.30 0.132 0.255 0.15 0.066 Determine the reaction order for each reactant and the value of the rate constant.
For a reaction involving the decomposition of a hypothetical substance Y, these data are obtained: Determine the order of the reaction. Write the rate law for the decomposition of Y. Calculate k for the experiment above.
Hydrogen iodide, HI, decomposes in the gas phase to produce hydrogen, H2, and iodine, I2. The value of the rate constant, k, fur the reaction was measured at several different temperatures and the data are shown here: Temperature (K) k (M -1 5-1) 555 6.23107 575 2.42106 645 1.44104 700 2.01103 What is the value of the activation energy (in kJ/mol) for this reaction?
At 620. K butadiene dimerizes at a moderate rate. The following data were obtained in an experiment involving this reaction: t(s) [C4H6] (mol/L) 0 0.01000 1000.. 0.00629 2000. 0.00459 3000. 0.00361 a. Determine the order of the reaction in butadiene. b. In how many seconds is the dimerization 1.0% complete? c. In how many seconds is the dimerization 10.0% complete? d. What is the half-life for the reaction if the initial concentration of butadiene is 0.0200 M? e. Use the results from this problem and Exercise 45 to calculate the activation energy for the dimerization of butadiene.
Hydrogen peroxide, H2O2(aq), decomposes to H2O() and O2(g) in a reaction that is first-order in H2O2 and has a rate constant k = 1.06 103 min1 at a given temperature. (a) How long will it take for 15% of a sample of H2O2 to decompose? (b) How long will it take for 85% of the sample to decompose?
Gaseous azomethane (CH3N2CH3) decomposes to ethane and nitrogen when heated: CH3N2CH3(g) CH3CH3(g) + N2(g) The decomposition of azomethane is a first-order reaction with k = 3.6 104 s1 at 600 K. (a) A sample of gaseous CH3N2CH3 is placed in a flask and heated at 600 K for 150 seconds. What fraction of the initial sample remains after this time? (b) How long must a sample be heated so that 99% of the sample has decomposed?
The rate constant for the decomposition of acetaldehyde, CH3CHO, t0 methane, CH4, and carbon monoxide, CO, in the gas phase is 1.1102 L/mol/s at 703 K and 4.95 L/moI/s at 865 K. Determine the activation energy for this decomposition.