The dimerization of butadiene2C,H.(g) C3H12(g)was studied at 500. K, and the following data were obtained:[C.H] (mol/L)1.6 x 101.5 x 101.3 x 101.1 x 100.68 x 10Time (s)195604124621806210What is the rate law and rate constant ?Rate = k[C4H6]^2 k= 0.028%3DRate = k[C4H6]^2 k= 0.007%3DRate = k[C4H6] k= 0.014%3!Rate = k[C4H6] k= 0.007%3!Rate k[C4H6]^2 k= 0.014Rate k[C4H6] k= 0.028%3D

For second order reaction, Rate = k[A]2 -d[A]/dt = k[A]2 On solving, we get 1/[A]t = 1/[A]o +kt When…

The dimerization of butadiene 2C,H(g) C3H12(g) was studied at 500. K, and the following data were obtained: Time (s) [C.H] (mol/L) 1.6 x 10 1.5 x 10 1.3 x 10 1.1 x 10 0.68 x 10 195 604 1246 2180 6210 What is the rate law and rate constant ?

The dimerization of butadiene 2C,H(g) C3H12(g) was studied at 500. K, and the following data were obtained: Time (s) [C.H] (mol/L) 1.6 x 10 1.5 x 10 1.3 x 10 1.1 x 10 0.68 x 10 195 604 1246 2180 6210 What is the rate law and rate constant ?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: Express the rate of the following chemical reactions in terms of the change in concentration of the…

A: The rate of reaction is defined as the change in the concentration of reactant per unit time per…

Q: Consider the reaction A → B, which has the following complex rate equation d[B]/dt =…

Q: Consider the following reaction: 2 NO(g) + 2 H2(g) N2(g) + 2 H2O(g) (a) The rate law for this…

A: The reaction taking place is given as, => 2 NO (g )+ 2 H2 (g) ↔ N2 (g) + 2 H2O (g) Given: Order…

Q: Consider the reaction and its rate law. 4 A + 3 B –→ products = k[A}°[B]* What is the order with…

A: Chemical kinetics is branch of chemistry in which we deal with speed at which rate of reaction…

Q: Writing the rate law implied by a simple mechanism with an initial slow... Suppose the formation of…

A: Overall reaction can be determined by adding all the steps of the reaction mechanism.Rate of…

Q: In the presence of O2, NO reacts with sulfur-containing proteins to form S-nitrosothiols, such as…

A: Chemical kinetics is the branch of chemistry that mainly deals with the rate of reaction and change…

Q: Ozone decomposes to form oxygen molecules and oxygen atoms, O3(g)→O2(g) + O(g), in the upper…

Q: Suppose the formation of nitryl fluoride proceeds by the following mechanism: rate constant step 1…

A: For any reaction: aA+bB→cC The rate law is given by: rate=kAxBy Here x and y are the partial…

Q: VII. A possible reaction for the degradation of the pesticide DDT to a less harmful compound was…

Q: The rate law for the reaction A + B - 3C was determined to be v = k[AJ°[B]° at 20°C. If the reaction…

Q: You dissolve an Al determine that 0.81 relevant calculation. Recall from the intr dissociate to give…

A: The main chemical component present in Alka Seltzer is sodium bicarbonate.

Q: Data in the table below were collected at 540 K for the following reaction: CO (g) + NO2(g) → CO2(g)…

Q: Consider the reaction described by the equation C,H,Br, (aq) + 3I¯(aq) → C,H,(g) + 2 Br¯(aq) + I5…

A: Given C2H4Br2 + 3I- → C2H4 + 2 Br- + I3-( aq ) Rate( R ) = K [ C2H4Br2 ] [ I- ] Rate…

Q: Consider the following reaction. aA +bB →→ cC whose first and second half-lives are 49.8 and…

A: Given: The half life of the reaction, (t1/2)=49.8 min. The rate constant, (K) = 0.01392. The initial…

Q: The rate coefficient for the reaction CH₂O(g) + O(g) → HCO(g) + OH(g) was measured as a function of…

A: The objective of this question is to determine the Arrhenius expression for the rate coefficient of…

Q: The reaction N,0 (g) + 0 (g) → N2 (g) + O2 (g) has a frequency factor of 3.69 x 10° M-1 s-l and an…

A: If the temperature is changed or a catalyst is added, for example, the constant changes. This is…

Q: 3A+B+C → D+Ewhere the rate law is defined as_ Δ|A|/Δr = k[A]2 [B] [C]An experiment is carried out…

Q: Consider the following reaction. aA +bB →→ cC whose first and second half-lives are 24.1 and 12.05…

A: Given:Rate constant (k) = 0.3251[A]0 = 15.67First half-life (t1/2 ) = 24.1 minutesNow, we can…

Q: write the rate law for the following reaction: H2S(g)+Cl2(g)-->S(s)+2HCl(g) represent the order as…

A: Order of the reaction tells about the rate of the reaction and the concentration of all the species…

Q: For the gas phase decomposition of trichloromethyl chloroformate, CICOOCC13 → 2 COC1₂ -1 the rate…

Q: The reaction C4H8(g)→2C2H4(g) Ea = 262 kJ/mol, T = 600K, k = 6.1\times 10-8 s-1. What is the value…

A: The activation energy is .The initial temperature is .The initial rate constant is .The final…

Q: A kinetics study of a reaction, A +B -C, is found to be zeroth order with respect to A and second…

A: Rate of the reaction depends on order of the reaction

Q: A proposed mechanism for a reaction is: NO + NO -> N2O2 N2O2 + O2 -> 2NO2 a) What is the overall…

A: a) Overall reaction can be obtained by adding both the steps: 2 NO + N2O2 + O2 —> N2O2 + 2 NO2…

Q: The reaction A (g) + (B) g → C(g) has a rate law that is rate = 5.43 x 10-2 (A][B]. The reaction…

A: Order of the reaction is defined as the sum of the exponential power of all the concentration terms…

Q: 5. The reaction 2NO(g) + Cl2(g) → 2NOCI(g) was performed and the following data obtained: (under…

A: Answer: For every reaction, in respect to its order, there is always a certain type of…

Q: The rate of the reaction 2 CIO2(aq) + 2 OH" (aq) → ClO, (aq) + ClO (aq) + H2O(€) is given by rate =…

A: The rate law of the reaction is given as, => Rate = K [ClO2]2 [OH- ] Given: Initial concentration…

Q: How to use calculus to integrate the differential rate law and obtain the first-order integrated…

A: The given first-order integrated rate law is,

Q: For the following reaction: H2(g) + ICl(g) ----> HI(g) + HCl(g) slow HI(g) + ICl(g) ---> I2(g) +…

A: Rate law equation

Q: Suppose the reduction of nitric oxide proceeds by the following mechanism: step elementary reaction…

Q: d. The activation energy of the reaction is 85 kJ/mol. Calculate the time required for [A₂] to go…

A: Answer :

Q: The rate equation for the hydrolysis of sucrose to fructose and glucose C12H22 O11 (aq) + H₂O(l) →…

A: Hydrolysis of sucrose follow first order kinetics

Q: The rate constant for this second‑order reaction is 0.630 M−1⋅s−1at 300 ∘C. A⟶products How…

Q: A possible mechanism for the next decomposition reaction is A(g) ⇄ 2B(g) + C…

A: These reactions are complex reactions, therefore the reactions which are completed in more than one…

Q: The formation of nitrosyl chloride is described by the following chemical equation: 2NO(g) + Cl₂ (g)…

A: For a multi-step reaction, the sum of all the steps of a mechanism gives the overall balanced…

Q: The rate constant for decomposition of azomethane at 425°C is 0.68s CH,N=NCH,(g)N(g) + C,H,(g) a)…

A: Since you have posted a question with multiple sub-parts,we will solve first three sub-parts for you…

Q: The rate constant for the following second-order reaction is S 2NOBr(g) 2NO(g) + Br₂ (g) Calculate…

A: The reaction given : 2 NOBr (g) ==> 2 NO(g) + Br2(g) rate constant , k = 0.80 M-.s- [NOBr]0=…

Q: Consider the following reaction. aA +bB →→ cC whose first and second half-lives are 18.4 and 36.8…

A: Given, First Half life = 18.4 mins Rate constant (k) = 0.005408 [Ao] = 10.05 Find, [A] at 23.12…

Q: A: Consider the following reaction: N2H5+ + 4 Fe(CN)63- --> N2(g) + 5 H+ + 4 Fe(CN)64-…

A: The rate law is an expression showing the relationship of the reaction rate to the concentrations of…

Q: Determine the rate law for the reaction, 2IC1 + H2 = I, + 2HCi, from the following initial rate…

Q: The combustion of ammonia is shown below: 4NH:(g) + 50:(g) → 4NO(g) + 6H;O(g) Write an equation that…

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

A: A question based on kinetics of reactions in solution that is to be accomplished.

Q: 2. At low temperatures the rate law for the reaction (½ A+ ½ B → C) is - r₁ =k₁ C₁ CB. If the…

A: The given rate law for the reaction at low temperatures is - r1 = k1 C1 CB. Here, r1 is the rate of…

Question

The dimerization of butadiene
2C,H.(g) C3H12(g)
was studied at 500. K, and the following data were obtained:
[C.H] (mol/L)
1.6 x 10
1.5 x 10
1.3 x 10
1.1 x 10
0.68 x 10
Time (s)
195
604
1246
2180
6210
What is the rate law and rate constant ?
Rate = k[C4H6]^2 k= 0.028
%3D
Rate = k[C4H6]^2 k= 0.007
%3D
Rate = k[C4H6] k= 0.014
%3!
Rate = k[C4H6] k= 0.007
%3!
Rate k[C4H6]^2 k= 0.014
Rate k[C4H6] k= 0.028
%3D

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 Calculating Rate law

VIEW

Step 2 second order reaction

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 1 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 certain reaction has an activation energy of 63.0 kJ mol−1kJ mol−1 and a frequency factor of A1�1 = 5.20×1012 L mol−1 s−1L mol−1 s−1 . What is the rate constant, k�, of this reaction at 29.0 ∘C∘C ? Express your answer with the appropriate units. Indicate the multiplication of units explicitly either with a multiplication dot (asterisk) or a dash.
Rate constants for the decomposition of gaseous dinitrogen pentoxide are 3.7×10−53.7×10−5 s−1s−1 at 25 ∘C∘C and 1.7×10−31.7×10−3 s−1s−1 at 55 ∘C∘C.2N2O5(g)→4NO2(g)+O2(g What is the activation energy for this reaction in kJ/molkJ/mol? What is the rate constant at 35 ∘C∘C?
24.) At 700 °C, hydrogen gas reduces nitric oxide according to the equation 2H2(g) + 2NO(g)  2H2O(g) + N2(g) whichobeys the rate law, Rate = k [H2][NO]2. What is the value of the rate constant, in 1M2⋅h , if the initial rate of thereaction is 0.183 M/h when the initial [H2] = 0.220 M and the initial [NO] = 0.250 M.a. 3.33 b. 0.075 c. 0.003 d. 13.33 e. 15.15
How Rate laws for new reactions with unknown mechanisms are determined ?
The rearrangement of ammonium cyanate to urea in aqueous solution at 50 °C NHẠNCO(aq)–→(NH2)½CO(aq) is second order in NH NCO with a rate constant of 1.10x10² M' min! If the initial concentration of NH,NCO is 0.945 M, the concentration of NH NCO will be 0.160 M after minutes have passed.
24
Define rate constant (K).
18. Which of these reactions appear to involve a catalyst? In those cases where a catalyst is present, tell whether it is homogeneous or heterogeneous. a) CH,COOCH,(aq) + H,O(() CH,COOH(aq) + CH,OH(aq) Rate = k[CH,COOCH,[H,O"] b) H;(g) +1(g) - Rate = k[H,][I,] +2 HI(g) %3D
Consider the reaction described by the equation С,Н, Вr, (aq) + 3Г (аq) — С,н,(8) + 2 Br (aq) + I5 (aq) The rate law is rate = k[C,H,Br,][I¯] where k = 0.00594 M-1. s-!. What are the missing entries in the table? Run [C,H,Br, lo (M) [I-], (M) Initial rate of formation of C,H, (M-s -) 1 0.245 0.00143 0.245 y 0.000713 3 0.245 0.245
Please help with this
Writing the rate law implied by a simple mechanism with an initial slow... Suppose the formation of nitryl fluoride proceeds by the following mechanism: elementary reaction step 1 NO₂ (g) +F₂ (g) 2 k₁ k₂ 2 F (g) + NO₂(g) → NO₂F (g) Suppose also k₁ « k₂. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction. Write the experimentally- observable rate law for the overall chemical reaction. NO₂F (g) +F (g) Note: your answer should not contain the concentrations of any intermediates. rate constant rate = k 0+ 00 X Ś
Consider the following reaction. aA +bB →→ cC whose first and second half-lives are 15.9 and 15.9 minutes respectively. If the rate constant is equal to 0.04358 and [A]0 = 11.98, calculate the [A] at t = 30.83 minutes.