The rate constant of a first-order reaction is 4.60 x 104/s at 350°C. If the activation energy is 104 kJ/mol, at what temperature will the rate constant be 8.80 x 104/s? A. 669 °C В. 402 °C С. 371 °C D. 350 °C

The rate constant of a first-order reaction is 4.60 x 104/s at 350°C. If the activation energy is 104 kJ/mol, at what temperature will the rate constant be 8.80 x 104/s? A. 669 °C В. 402 °C С. 371 °C D. 350 °C

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: The first-order reaction AB has a rate constant of 6.43 x 10-251. How many seconds will it take for…

Q: 2. The rate constant of a reaction at 32.0°C is 0.0550 s¹. If the frequency factor is 1.20 x 10¹3…

Q: - The activation energy for the following 1st-order reaction is 114 kJ/mol. N₂0s (g) → 2 NO₂ (g) +…

A: K2 at temperatureT2(-5°C) = 2.14×10-7 s-1 Explanation:Step 1:.

Q: The reaction: A+B → C + D is second order in [A] and zero order in [B]. The value of k is 0.012 M-¹…

A: The order of the reaction is the total power coefficient of the reactants in the rate law equation.…

Q: In the reaction, N2O4(g) 2 2 NO2(g) the concentration of N,04 was measured as a function of time…

A: The rate of the reaction is the change of the concentration of the reactant or the product per unit…

Q: A chemistry graduate student is studying the rate of this reaction: 2SO3 (g) →2SO₂(g) + O₂(g) He…

A: The objective is to determine the rate law and rate constant of the given reaction.Given…

Q: Consider the following data for the reaction: A+B → C+D [A] (M) [B] (M) 0.0100 0.0200 0.0200 0.0100…

Q: Consider the following reaction mechanism: Step 1: A(g) + B(g) X(g) fast step Step 2: X(g) + C(g)…

A: Chemical kinetics is the study of the reaction that how fast or slow a reaction is taking place. The…

Q: Nitrogen pentoOxide decomposes by a first-order process yielding N,0, and oxygen. 2N,0, → 2N,0, + 0,…

A: given, 2 N2O5 ----> 2 N2O4 + O2 HALF LIFE = 0.85 Hr rate constant = ?

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: The rate constant for this zero-order reaction is 0.0200 M· S at 300 A → products How long (in…

A: We have given that A → Products K0 = 0.0200M S-1 [A]0 = 0.830M [A]t = 0.280M t = ?

Q: 8. The rate constant for a first order reaction is 4.60 x 10* s' at 350°C. If the activation energy,…

A: Arrhenius equation that relates the rate constants k1 and k2 at respective temperatures T1 and T2…

Q: er reaction has a rate constant of 1.

A: First order reaction is that which depend only on one reactant concentration. To calculate…

Q: 12.

A: Correct option is D L mol-1s-1 The unit for the rate constant of a second order reaction…

Q: A zero-order reaction has a first half-life of 964 s. What will be the value of the seventh…

A: The half-life of the reaction is the time in which the concentration of the reacting species is…

Q: The first-order reaction, SO2C12 → SO2 + Cl2, has a rate constant equal to 2.20 x 10 s' at 593 K…

A: Chemical kinetics is the study of the reaction that how fast or slow a reaction is taking place. The…

Q: rate

Q: 21. For the decomposition of N₂Os(g), 2 N₂Os(g) →4 NO₂(g) + O2(g), the following data were obtained…

Q: If the initial mass of A is 18.03 g. calculate the mass of A remaining after 2.00 min. mass of A:

A: k = 0.0177s-¹ Ao = 18.03g t = 2×60 = 120sec ln[At] = ln[A] - kt = ln[18.03] -…

Q: Expt Initial [NO] Initial [Cl2] 0.0125 M initial Rate M1 0.0510 M 2 0.0250 M 4.54 0.0255 M 0.0255 M…

A: Welcome to bartleby ! We have to tell the rate law

Q: Consider this reaction: →2Cl2O5g+2Cl2g5O2g At a certain temperature it obeys this rate law.rate…

A: The reaction given is 2 Cl2O5 ----> 2 Cl2 + 5 O2 And the rate law given is Rate = 0.00711 X…

Q: For the reaction X — Ү identify what the graphs of [X] versus time and [Y] versus time would look…

Q: The rate constant for this second-order reaction is 0.560 M-1 •s-1 at 300 °C. A → products How long,…

Q: The reaction: 2NO + Cl2 → 2NOCl is second order in NO, first order in Cl2 and third order overall.…

Q: Consider the reaction A⟶ Products. The rate law for this reaction is rate = k[A] where k= 3.00×10-3…

A: The rate law of the reaction indicates that the reaction is of first order.

Q: The reaction C,H,(g)2C,H, () has an activation energy of 262 kJ/mol. At 600.0 K, the rate constant,…

A: The activation energy is 262kJ/mol At 600K, rate constant = 6.1 x 10-8s-1 at 850K, rate constant =…

Q: Which of the following statements are true about a first-order reaction? X. Units of the rate…

A: Use the concept first order reaction's chemical kinetics.

Q: , the half-life of a first-order reaction

A: The half-life of a reaction is the time required for the reactant concentration to decrease to…

Q: A reactant decomposes with a half-life of 107 s when its initial concentration is 0.171 M. When the…

Q: Consider the following reaction that follows a second order rate law. 2 NO2 (g) → 2 NO (g) + 02 (9)…

Q: A certain reaction is second order in N₂ and second order in H₂. Use this information to complete…

A: The objective of the question is to find the missing rate of the reaction at the given concentration…

Q: The reaction C,H, (g) → 2C,H,(g) has an activation energy of 262 kJ/mol. At 600.0 K, the rate…

A: Two point Arrhenius equation is given by, Where, Ea is the…

Q: The reaction 4 HBr(g) + O2(g) 2 H2O(g) + 2 Br2(g) was studied at a certain temperature with the…

Q: 40. In zero-order reactions, for every rise of 10 °C of the temperature, the rate of the reaction is…

A: For every rise of 10°c of the temperature the rate of the reaction is double.

Q: 5. The reaction H2 (g) + 12 (g) → 2 HI (g) has the following mechanism proposed: Fast 12 (g) = 21…

Q: A particular reactant decomposes with a half-life of 129 s when its initial concentration is 0.282…

A: The half-life of the reaction when the initial concentration of the reactants is 0.282 M is = 129 s…

Question

The rate constant of a first-order reaction is 4.60 x 104/s at 350°C. If the activation energy is
104 kJ/mol, at what temperature will the rate constant be 8.80 x 104/s?
A. 669 °C
B. 402 °C
C. 371 °C
D. 350 °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

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

For the reaction: NO2(g) → 1/2 O2(g) + NO (g) The following data were obtained: Time (s) 0 50 100 [NO₂] (M) 0.01 Concentration NO2 0.00787 -4.844697217 127.064803 200 0.00481 -5.337058195 0.00649 -5.037492748 154.0832049 300 0.0038 -5.572754212 0.012 0.01 0.008 Natural Log [NO2] (M) Determine the rate law of this reaction and the value of k, the rate constant. The graphs of the data appear below. 0.006 0.004 -4.605170186 100 0.002 0 0 1/[NO2] 100 200 Time (s) 207.9002079 1/[NO2] 263.1578947 y = -1.97E-05x + 9.15E-03 R² = 9.27E-01 300 250 200 150 100 50 0 300 0 50 400 100 Natural Log [NO2] 150 -4.5 -4.7 -4.9 -5.1 -5.3 -5.5 -5.7 0 200 Time (s) y = 0.5431x + 99.833 R² = 1 100 250 300 200 Time (s) 350 y = -0.0032x - 4.6679 R² = 0.9824 300 400
Consider the reaction A⟶ Products. The rate law for this reaction is rate = k[A] where k= 3.00×10-3 s-1 at a particular temperature. If the initial [A] = 0.500 M, what will be the concentration of A after 2.00 minutes? 0.497 M 0.349 M 0.424 M 0.499 M
General Chemistry 4th Edition McQuarrie • Rock • Gallogly dUniversity Science Books presented by Macmillan Learning The reaction C,H¿ (g) → 2 C,H¿(g) has an activation energy of 262 kJ/mol. At 600.0 K, the rate constant, k, is 6.1 × 10-8 s-!. What is the value of the rate constant at 840.0 K? k =
For the reaction:A(g) + B(g) →AB(g) the rate is 0.30 mol/L.s, when [A]0 = [B]0 = 1.0 mol/L. If the reaction is first order in B and second order in A, what is the rate when [A]0 = 1.9 mol/L and [B]0 = 4.3 mol/L?
A certain reaction is second order in N₂ and second order in H₂. Use this information to complete the table below. Round each of your answers to 3 significant digits. 0.460 M 0.460 M 1.43 M [¹2₂] 1.66 M 2.94 M 0.534 M initial rate of reaction 56.0 M/s M/S M/S 0 x10 X
A certain reaction is second order in N, and first order in H₂. Use this information to complete the table below. Round each of your answers to 3 significant digits. [₂] 1.94 M 1.94 M 3.73 M 1.34 M 6.33 M 0.697 M initial rate of reaction 0.349 M/s M/S M/S X
A particular first-order reaction has a rate constant of 1.35 x 102 s at 25.0 ° C. What is the magnitude of k at 55.0°C if Ea = 55.5 kJ/mol. 1.05 103 2.67 1065 277 1.35 102 1.65 104
The rate constant for this first-order reaction is 0.0125 s−10.0125⁢ s−1 at 300 °C. A⟶productsA⟶products If the initial mass of A is 18.99 g,18.99 g, calculate the mass of A remaining after 2.53 min.
17
The decomposition of hydrogen iodide on a gold surface at 150 °C HI(g) → ½ H2 (g) + ½ I2 (g) is zero order in HI with a rate constant of 1.20×10-4 M/s How much time is required for the concentration of HI to drop to 9.40×10-2 M if its initial concentration is 0.525 M?