**Activation Energy and Rate Constants in Chemical Reactions**The activation energy for the following first-order reaction is **102 kJ/mol**.\[ 2 \text{N}_2\text{O}_5 (g) \rightarrow 4 \text{NO}_2 (g) + \text{O}_2 (g) \]The value of the rate constant, $ k $, is **1.35 × 10^-4 s^-1** at **35 °C**. What is the value of $ k $ at **0 °C**?Options:- A. $ 8.2 \times 10^{-7} \, \text{s}^{-1} $- B. $ 1.9 \times 10^{-5} \, \text{s}^{-1} $- C. $ 4.2 \times 10^{-5} \, \text{s}^{-1} $- D. $ 2.2 \times 10^{-2} \, \text{s}^{-1} $

Answered: Image /qna-images/answer/f5954f35-d0aa-44b3-9049-2985b777d4cf.jpg

The activation energy for the following first-order reaction is 102 kJ/mol. 2 N2O5 (g) →4 NO2 (g) + O2 (g) The value of the rate constant, k, is 1.35 x 104 s-' at 35 °C. What is the value of k at 0°C? A. 8.2 × 10-7s-! B. 1.9 x10-5 s- C. 4.2 ×10 s-1 D. 2.2 ×10-2 s-'

The activation energy for the following first-order reaction is 102 kJ/mol. 2 N2O5 (g) →4 NO2 (g) + O2 (g) The value of the rate constant, k, is 1.35 x 104 s-' at 35 °C. What is the value of k at 0°C? A. 8.2 × 10-7s-! B. 1.9 x10-5 s- C. 4.2 ×10 s-1 D. 2.2 ×10-2 s-'

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: Determine the order of reaction of B in this reaction. [A] (mol/L) [B] (mol/L) Initial rate (mol/Ls)…

A: The order of the reaction is given below

Q: What is the activation energy, Ea, for the reaction?

Q: reaction of a particular organic compound with water varies with temperature as follows:…

Q: 5. Rate constant of a reaction changes from 0.0125 s¹ to 0.320 s¹ when temperature changes from 411…

A: Given, Rate constant (k): k1 = 0.0125 s-1 k2 = 0.320 s-1 Temperature (T): T1 = 411 K T2 = 435 K…

Q: The rate constant for this second-order reaction is 0.150 M-1. s-1 at 300 °C A products How long, in…

A: The integrated rate law for a second order reaction is given by

Q: The reaction A →B is found to be first order.

A: formula is K = (2.303/t) log [a/(a-x) ] ------(1) where K = rate constant =? t = 80…

Q: A certain reaction is second order in N, and second order in H,. Use this information to complete…

Q: The following reaction is first order in respect to NO and second order in respect to O2. With this…

A: Given reaction is 2NO(g) + O2(g) ----> 2NO2 (g) Order with respect to NO = 1 Order with respect…

Q: The rate constant for this second-order reaction is 0.250M-1 ·s-l at 300 °C. A → products How long,…

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: A certain reaction is second order in N, and second order in H,. Use this information to complete…

A: Given : reaction order in reactant N2 = 2 and reaction order in reactant H2 = 2 Hence the rate of…

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

Q: A reaction was shown to follow second-order kinetics. How much time is required for [A] to change…

A: The integrated rate law for a second-order reaction:Where Given,

Q: For the first-order reaction: A(g) > B(g) the rate constant is k = 6x 10t s at -10°C, and the…

Q: 2 A P The rate coefficient for this elementary reaction isk = 8.63 x 10 M' min'. The initial…

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: How long, in seconds, would it take for the concentration of A to decrease from 0.750 M to 0.250 M?

A: Given:- reaction is 2nd order Rate constant = 0.890 M-1 s-1 Initial concentration = 0.750 M Final…

Q: What is the half-life of this reaction at 65 °C?

A: Given data is The decomposition of N2O5 is a first order reaction. The activation energy = 110…

Q: The mechanism shown here, along with their corresponding activation energies, is proposed for a gas…

A: The mechanism given is,Step 1: N2O5 NO2 + NO3 Ea = 25 kJ/molStep 2: NO2 + NO3 → NO2+ O2 + NO…

Q: A certain reaction has an activation energy of 66.90 kJ/mol. At what Kelvin temperature will the…

A: It is based on the concept of Arrhenius theory of rate constant. Here we are required to find the…

Q: The reaction C₂H₂ (g) →2 C₂H₂ (g) 8 has an activation energy of 262 kJ/mol. At 600.0 K, the rate…

A: The objective of this question is to find the rate constant, k, at a different temperature using the…

Q: M (mol/L) In M] 1/M (L/mol) 11- 0.9 104 0.8- -0. 0.1 0.64 -1- 6- 0.5 5- 04 -15- 4- 03 02 01- Time…

Q: digits. [N.] [4.] initial rate of reaction 2.06 M 2.30 M 6.00 x 10 M/s ) MIs 9.89 M 2.30 M O Mis…

A: We will divide rate law expression to get rate of reaction for 2nd and 3rd .

Q: The reaction A - B is found to be first order. At 650 K, 45 % of A has been converted to B in 75.0…

Q: A chemical reaction has the rate law R = K[A]²[B] The rate of the reaction is found to be 4.3 M/min…

A: Given, R = 4.3 M/min [A] = 0.20 M [B] = 0.10 M

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 following reaction was determined to be elemtary: A + 2B -> C What is the overall of the…

Q: Dinitrogen pentoxide, N2O5, decomposes by a first order reaction with an activation energy of 110…

A: We will use relation rate constant and activation energy

Q: the concentration of NOBr after 20 s.

A: According to the question, the reaction is given below – 2NOBr(g) → 2NO(g) + Br2(g) We have, The…

Q: A certain reaction is first order in N, and second order in H,. Use this information to complete the…

A: Consider the general reaction. A+B→C+D Write the expression of rate law of this reaction. Rate of…

Q: The rate constants for a reaction are found to be k(315 C) = 8.5 x 10 -8 s-1 k(506 C) = 27.0 x 10…

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 activation energy of a first order reaction is 2.03 × 105 J/mol. At 40 oC, the rate constant is…

Q: a. R = k[A][B] b. R = k[A]³[B] c. R = k[A][B]² d. R = k[A]³[B]?

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

A: we have to complete the given table.

Q: Consider the elementary reaction equation K(g) + HCl(g) KCI(g) + H(g) What is the order with respect…

A: The given elementary reaction is recorded as followsK(g) + HCl(g) ⟶ KCl (g) + H(g)

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: Use the following information to determine the activation energy for the reaction shown here:…

Q: Decomposition of hydrogen peroxide (H2O2) is a first order reaction. The initial concentration of…

A: Given : initial concentration of hydrogen peroxide, [ A ]o = 0.350 M concentration of hydrogen…

Q: Consider a reaction that has the following mechanism: A2 2 A (fast, equilibrium) A+B AB (slow) A +…

A: The rate of a reaction is directly related to the concentration of reactant species. A reaction…

Q: 6. The rate constants for the decomposition of a compound are 6.2 x 10 s at 45°C and 2.1 x 10 s' at…

Q: A certain reaction is second order in N, and first order in H,. Use this information to complete the…

A: First we will calculate the rate constant using the rate law expression. Than we will use the rate…

Q: consider the following reaction with an activation energy of 12.10 kJ/mol and a rate constant of 9.0…

Q: The given first-order reaction A - B, has a rate constant of 1.60 x 102 s1 at 165°C and 6.54 x 10 at…

A: Activation energy can be calculated as follows

Q: A first order reaction (A --> B) has an initial concentration, [A]= 0.600M and after 100.0 seconds…

A: We have given that for first order reaction A → B Initial concentration of [A]0 = 0.600M…

Question

**Activation Energy and Rate Constants in Chemical Reactions**

The activation energy for the following first-order reaction is **102 kJ/mol**.

\[ 2 \text{N}_2\text{O}_5 (g) \rightarrow 4 \text{NO}_2 (g) + \text{O}_2 (g) \]

The value of the rate constant, $ k $, is **1.35 × 10^-4 s^-1** at **35 °C**. What is the value of $ k $ at **0 °C**?

Options:
- A. $ 8.2 \times 10^{-7} \, \text{s}^{-1} $
- B. $ 1.9 \times 10^{-5} \, \text{s}^{-1} $
- C. $ 4.2 \times 10^{-5} \, \text{s}^{-1} $
- D. $ 2.2 \times 10^{-2} \, \text{s}^{-1} $

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

18. * Determine the activation energy for the first-order reaction 2NOCI2NO + Cl2 given the following rate constants at different temperatures. Temperature (K) k (L/mol-s) 500 2.9 x 10-1 600 16.3 O 1.21 x 10* J/mol O 1.00 x 10s J/mol O 8.27 x 10 $ J/mol O 6.88 x 10-4 J/mol
q11 What is the value of k for a reaction that follows first-order kinetics, given that its half-life is 28 seconds? A. 38 S-1 B.0.039 S-1 C.0.025 s-1 D.0.0086 S-1
5. The reaction A →B+C is known to be first order in A. Below are data showing the concentration of A as a function of reaction time. Time, min [A], M 5.00 x 10-2 4.30 x 10-2 5 10 3.70 x 10-2 2.74 x 10-2 1.51 x 10-2 20 40 1.12 x 10-2 8.26 x 10-3 50 60 (a) What is the average rate of reaction between 5 and 20 min? Report the units as well as the numbers. (b) Plot the data above, showing the concentration of A as a function of the time. From your graph, determine the instantaneous rate of reaction at 40 min. Report the units as well as the numbers. (c) Plot In [A] versus time. Estimate the rate constant for this first-order reaction from your graph. Report the units as well as the numbers.
If the half-life of a 1st order reaction is 67 minutes, k= a. 1.0x10-2s-1 b. 97 s-1 c. 5800 s-1 d. 1.7x10-4s-1
9.
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 =
4. Determine the order of the following reactions from the rate constant. a. k= 1.3 x 104 s-1 b. k = 4.7 x 10-² mol L-'s'
The half-life of a first order reaction is constant and equal to 0.693/k. CA first order reaction with k= 3.465 x 10-2 s-1 is started with [A]o=0.800 M. What is the concentration of A after 60 seconds? Oa. 0.100 M Ob. 0.400 M Oc. c. 0.200 M Od. 0.0800 M
The following reaction has rate law r = k[C4H6] 2 , where k = 0.014 M-1 s -1 What is the concentration of C4H6 (in M) after 3.0 hours, if [C4H6]o = 0.025 M? A. 0.0052 M B. 0.024 M C. 0.012 M D. 0.0060 M
6. The rate constants for the decomposition of a compound are 6.2 x 10* s' at 45°C and 2.1 x 103 s1 at 55°C. What is the value of the activation energy for this reaction in kJ/mol? А. 1.7 х 10% В. 1.1 x 105 C. 2.5 x 103 D. 2.5 x 104 E. 1.1x 106
Q6. Answer the following questions based on the data provided: N203(g) - NO,(g) + NO,(g) Time (s) (N,O.] (M) 1.000 25 0.822 50 0.677 75 0.557 100 0.458 0.377 125 150 0.310 0.255 0.210 175 200 a. What is the overall order of the reaction? b. Calculate the value of the rate constant. c. What is the concentration of dinitrogen monoxide at 250s?
7