**Question 2: Determining Activation Energy**At 32.0°C, the rate constant of a reaction is 0.0550 s⁻¹. Given that the frequency factor is 1.20 x 10¹³ s⁻¹, calculate the activation energy.---To solve this problem, you can use the Arrhenius equation:\[ k = A e^{-E_a/(RT)} \]Where:- \( k \) is the rate constant,- \( A \) is the frequency factor,- \( E_a \) is the activation energy,- \( R \) is the universal gas constant (8.314 J/mol·K),- \( T \) is the temperature in Kelvin.**Steps to solve:**1. Convert the given temperature from Celsius to Kelvin by adding 273.15.2. Rearrange the Arrhenius equation to solve for the activation energy \( E_a \).3. Substitute the given values and constants into the equation.4. Solve for \( E_a \).Note: Pay careful attention to units throughout the calculation to ensure accuracy.

Answered: Image /qna-images/answer/1551e450-9c53-4d9f-8fa4-ad0dac9e6d6c.jpg

Answered: 2. The rate constant of a reaction at…

2. The rate constant of a reaction at 32.0°C is 0.0550 s¹. If the frequency factor is 1.20 x 10¹3 s¹, what is the activation energy?

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

Q: Given the same reactant concentrations, the reaction COg) + Cl,(8) → COC,(8) at 245°C is 136 times…

A: Recall the given reaction, CO (g) + Cl2 (g) -------> COCl2 (g) . The reaction at 245◦C is 136…

Q: The reaction C4H8(g)⟶2 C2H4(g) has an activation energy of 262 kJ/mol. At 600.0 K, the rate…

Q: A chemical reaction occurred for the hypothetical reaction A + B → C and the rate law was determined…

A: Given, rate law for the reaction: Rate = k [A][B] It is given that experiments were done to…

Q: Rate constants for decomposition of dinitrogen pentoxide are 3.7 x105 s¹ at 25.0 °C and 3.4 x10³ s¹…

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: A reaction has an activation energy of 225,0 kJ/mol. By what factor will the rate constant, k,…

A: Arrhenius equation: Arrhenius equation give the relationship between the activation energy and the…

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

Q: The rate constant of a chemical reaction is 8.04 s-1 at a temperature of 27.9 \deg C. If the…

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: Calculate the rate constant, ?, for a reaction at 50.0 °C that has an activation energy of 85.1…

Q: The rate constant for the reaction is 0.140 M−1⋅s−10.140⁢ M−1⋅s−1 at 200 ∘C.200⁢ ∘C. A⟶products…

Q: Suppose that a catalyst lowers the activation barrier of a reaction from 127 kJ/mol to 51 kJ/mol .…

A: Activation energy is the minimum energy required for a chemical reaction or reactants to go to…

Q: The rate constant for the reaction is 0.970 M−1⋅s−1 at 200 ∘C. A⟶products If the initial…

A: Given the rate constant is 0.970 M-1 s-1, from the unit of rate constant it is clear that reaction…

Q: The reaction C₂Hg (g) →2C₂H₂(g) has an activation energy of 262 kJ/mol. At 600.0 K, the rate…

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

A: The given rate constant (k)= 2.55×10^-8 s^-1 Given reaction is first order And we know for first…

Q: Given a reaction with an activation energy of 2.3 x 104 J/mol. The rate constant will increase by a…

A: Given that, activation energy Ea=2.3*104 J mol-1 T1=200 °C=(200+273) K =473 K T2=250 °C=(250+ 273)…

Q: The activation energy of a certain reaction is 33.6 kJ/mol . At 21 ∘C ∘C , the rate constant is…

Q: The activation energy for a particular reaction is 102 kJ/mol. If the rate constant is 1.35 x 104 s¹…

A: Answer:Here:k1 and k2 are the rate constants at temperatures T1 and T2 respectively

Q: Calculate the rate constant, k, for a reaction at 63.0 °C that has an activation energy of 76.9…

A: The relation between rate constant, temperature and activation energy is given by Arrehenius…

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

A: Consider the given information is as follows; Order of the reaction = 1 (First order) Rate…

Q: The rate constant for the reaction is 0.770 M−1⋅s− at 200 ∘C. A⟶products If the initial…

A: Given the rate constant is 0.770 M-1 s-1, from the unit of rate constant it is clear that reaction…

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

A: For first order reaction : Half-life time, t1/2 = 0.693/k k = rate constant

Q: Suppose that a catalyst lowers the activation barrier of a reaction from 125 kJ/mol t o 55 kJ/mol.…

Q: Consider this reaction: →2N2O5g+2N2O4gO2g At a certain temperature it obeys this rate law.rate…

A: Since as per the given rate law we can see that the power of the concentration of N2O5 is 2 Hence…

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: 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: Suppose that a catalyst lowers the activation barrier of a reaction from 124 kJ mol−1kJ mol−1 to 53…

A: The question is based on the concept of chemical kinetics. we need to calculate the rate factor…

Q: A reaction has a rate constant of 8.52 x 102s1 at 12 C and 2.61 x 101l at 45 °C. Determine the…

A: Given that: Rate constant (k1) = 8.52 × 10-2 s-1 Temperature (T1) =…

Q: Ethylene oxide, C₂H4O, decomposes when heated to give methane and carbon monoxide. C₂H4O(g) → CH4…

A: We have to select the rate law expression for the given reaction and calculate the value of rate…

Q: 2 NOBr(g) k= - 2 NO(g) + Br₂(g) Determine the value and units of the rate constant, k. [NOBr], (M)…

A: Rate law expression: Let us understand the rate law expression by taking an example, X + Y ➝ Z The…

Q: Rates of Reactions Consider reactions of the type: Reactant 1 + Reactant 2 Products The activation…

A: Answer: On increasing the temperature, rate of reaction increases because increase in temperature…

Q: The activation energy of a particular reaction is 65.7 kJ/mol. How much faster does the reaction…

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

Q: Calculate the rate constant, k, for a reaction at 60.0 °C that has an activation energy of 77.7…

A: Rate constant is the ratio of product to the reactant where each concentration term is raised to the…

Q: The rate constant for the reaction is 0.130 M−1⋅s−1 at 200 ∘C A⟶products If the initial…

A: Rate is the speed at which a reaction takes place. The rate of appearance of the product equals to…

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

A: Arrhenius equation: Arrhenius equation give the relationship between the activation energy and the…

Q: The hydrolysis of sucrose (C12H22O11)(C12H22O11) into glucose and fructose in acidic water has a…

A: GIVEN: rate constant = 1.8 * 10 - 4 s-1 Volume of sucrose= 2.65L Molarity of sucrose = 0.150 M Time…

Q: The rate constant for a reaction at 23.0°C is 0.010 s1 and its activation energy is 35.8 kJ.…

Q: 4. A slightly bruised apple will rot extensively in about 4.00 days at room temperature, 25.0°C. If…

Q: Given the same reactant concentrations, the below reaction at 257. °C is 94.6 times as fast as the…

A: Answer:Here:k1 and k2 are rate constants at temperatures T1 and T2 respectively.

Q: Thermal decomposition of substance A in the gas phase at a constant volume proceeds according to the…

A: see attachmentExplanation:Step 1: Step 2: Step 3: Step 4:

Q: The rates of most reactions double when their temperature is raised from 298 K to 308 K. Calculate…

A: Arrhenius equation gives the relation between rate constant and temperature. lnk2k1=-EaR1T2-1T1…

Q: The rate constant for a certain reaction is k = 7.60×10−3 s^-1 . If the initial reactant…

Question

Expert Solution

Step 1

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

Consider the hypothetical reaction A(g) + B(g) ----> C(g) The four containers below represent this reaction being run with different initial amounts of A and B. Assume that the volume of each container is 1.0L. The reaction is second order with respect to A and first order in respect to B. If the temperature in container W were increased, what impact would this probably have on the reaction rate? Why?
The reaction described by the equation 0,(g) + NO(g) 0,(g) + NO, (g) has, at 310 K, the rate law rate of reaction = k[O,][NO] k = 3.0 × 106 M-1-s-1 Given that [O,] = 4.0 x 10-4 M and [NO] : 5.0 x 10- M at t = 0, calculate the rate of the reaction at t = 0. rate: M/s What is the overall order of this reaction? 3 1 2
Calculate the rate constant, k, for a reaction at 61.0 °C that has an activation energy of 78.9 kJ/mol and a frequency factor of 2.66 x 101 s-1. k =
The rate equation for the hydrolysis of sucrose to fructose and glucose C₁2H₂O(aq) + H₂O()→ CsH₁2Os(aq) + CH₂Os (aq) is-A[sucrose]/At=k[C₁₂H₂O₂). After 28 minutes at 27 °C, the sucrose concentration decreased from 0.0112 M to 0.0090 M. Find the rate constant k. k= min-1 Submit Answer Try Another Version 4 item attempts remaining
The reaction described by the equation 0,(g) + NO(g) → 0,(g) + NO,(g) has, at 310 K, the rate law rate of reaction = k[O,][NO] k = 3.0 × 106 M-!·s-! Given that [O,] = 4.0 × 10-4 M and [NO] = 2.0 × 10-³ M at t = 0, calculate the rate of the reaction at t = 0. %3D rate: M/s What is the overall order of this reaction? 3
The activation energy of an uncatalyzed reaction is 94 kJ/molk. The addition of a catalyst lowers the activation energy to 54 kJ/molk . Assuming that the collision factor remains the same, by what factor will the catalyst increase the rate of the reaction at 25 ∘C? Express the ratio to two significant digits. Assuming that the collision factor remains the same, by what factor will the catalyst increase the rate of the reaction at 120 ∘C? Express the ratio to two significant digits.
8. Dinitrogen tetraoxide (N2O4) decomposes spontaneously at room temperature in the gas phase: N2O4 (g) → 2 NO2(g) The rate law governing the disappearance of N2O4 with time is A[N,O4] = k N2O4]. At At 30°C, k = 5.1 x 106 s-1 and the activation energy for the reaction is 54.0 kJ/mol. Calculate the time (in seconds) required for the partial pressure of N2O4(g) to decrease from а. 0.10 atm to 0.010 atm at 30°C. b. Calculate the value of the rate constant at 300K. Repeat the calculation for the reaction in a) at the new temperature (300K). С. d. Write an observation about how the rate of reaction changed upon increasing the temperature.
The reaction described by the equation 0,(g) + NO(g) - O2(g) + NO, (g) > has, at 310 K, the rate law rate of reaction k[O,][NO] k = 3.0 x 106 M-1.s-1 Given that [O,] = 2.0 × 10-4 M and [NO] = 4.0 × 10-³ M at t = 0, calculate the rate of the reaction at t = 0. rate: M/s What is the overall order of this reaction? 2 3 1
If the rate constant for a reaction is 2.86 s1 at 20\deg C and the activation energy is 36.2 kJ/mol, then at what temperature will the rate constant have doubled?
The rate constant for the reaction is 0.450 M−1⋅s−1 at 200 ∘C. A⟶products If the initial concentration of A is 0.00610 M, what will be the concentration after 405 s?
A possible reaction for the degradation of the pesticide DDT to a less harmful compound was simulated in the laboratory. The reaction was found to be first order, with k = 2.47 x 10-8 s-1 at 25°C. What is the half-life for the degradation of DDT in this experiment, in years? (1 year = 365 days)
-1 For a certain reaction, the frequency factor A is 7.5 × 10⁹ s1 and the activation energy is 21.4 What is the rate constant for the reaction at 95. °C? Round your answer to 2 significant digits. Note: Reference the Fundamental constants table for additional information. k = -1 S X kJ mol S