A reaction has a rate constant of 1.26×10-4 s-1 at 29 °C and 0.231 s-1 at 79 °C. part a) Determine the activation barrier for the reaction. Part b)What is the value of the rate constant at 17 °C ?

A reaction has a rate constant of 1.26×10-4 s-1 at 29 °C and 0.231 s-1 at 79 °C. part a) Determine the activation barrier for the reaction. Part b)What is the value of the rate constant at 17 °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: Consider the reaction 2O3(g) ⟶3O2(g); Use the following data to calculate the activation energy for…

Q: A first-order reaction has rate constants of 4.6 x 10 2 s1 and 9.3 x 10 2 sl at 0°C and 20.°C,…

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

A: Arrhenius equation tells how rate of reaction depends on temperature. It is given as:

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

A: The given question can be solved as :

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 rate constant for the conversion of cyclopropane into propene was determined at several…

A: The integrated form of Arrhenius equation is lnk=-EaR1T+lnA The above equation is in the form of a…

Q: A first-order reaction has rate constants of 4.6 x 10-2 s-1 and 9.6 x 10-2 s1 at 0°C and 20.°C,…

A: The given data contains, k1=4.6×10-2/sk2=9.6×10-2/sT1=273 KT2=293 K

Q: Time(min) 0 5.83 17.8 25.6 35.6 Concentration(M) 0.120 0.0910 0.060 0.046 0.030 d)Would you…

A: Half-life of a reaction: It is the time required for the reactants concentration to decrease half…

Q: Part A) The activation energy of a certain reaction is 49.3 kJ/mol . At 22 ∘C , the rate constant is…

A: Activation Energy = 49.3 KJ/mol Part A Temperature at which rate = double ? Part B Rate constant at…

Q: A certain reaction, A → products, has a rate constant, k, of 5.8610-4 s-1 at 37 °C. When the…

Q: (D)What is the concentration of [A] at time t=64 s? 2.81 XM

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

Q: None

A: The best answer for the product of the reaction is (c) N-CO₂H / CO₂Et (H2N-CO₂Et)Here's…

Q: What is the activation energy of a reaction if it has the following rate constants?

Q: reaction has a rate constant of 1.24×10−4 s-1 at 28 °C and an activation energy of 137.0 kJ/mol. At…

Q: 5. The reaction, 2A + 2B C + D, has a rate constant of 6.0x10-3 L² mol-2 s¹ at 10°C. If its…

Q: What is the rate constant at 56°C?

Q: The rate constant for a first-order reaction is 4.60 x 10-4 s-1 at 350 oC. If the activation energy…

Q: The reaction between nitrogen dioxide and carbon monoxide is NO₂(g) + CO(g) → NO(g) + CO₂(g) The…

Q: A first-order reaction has rate constants of 4.6 x 10-² s¹ and 9.5 × 10-2 s¹ at 0°C and 20.°C,…

A: The given data contains,

Q: O + N2 → NO + N The activation energy for this reaction is 319.0 kJ/mol, and the reaction is…

Q: 17) A reaction has an activation energy of 85 kJ. What percentage increase would one get for & for…

Q: There is 60% reduction in the value of the rate constant of a reaction when the reaction temperature…

A: Given T1 = 60°C T2 = 40°C There is 60% reduction in the value of the rate constant standard value R…

Q: The activation energy of a certain reaction is 36.9 kJ·mol−1. At 35 °C, the rate constant is 0.0135…

A: We have to calculate a) temperature at which rate is twice as fast b) rate constant at 225°C

Q: The gas-phase reaction below has an overall enthalpy change of -45 kJ. The activation energy for the…

A: According to the question, The overall enthalpy change for the reaction is given by (∆H) = -45 kJ…

Q: Hydrogen peroxide decomposes spontaneously to yield water and oxygen gas according to the reaction…

A: The expression of Arrhenius equation is shown below: k = A e-Ea/RT Where; k = rate constant A =…

Q: A reaction is followed and found to have a rate constant of 3.36 × 104 M-1s-1 at 344 K and a rate…

A: Given data : Rate constant, K1 = 7.69 M-1 .s-1 At temperature, T1 = 219 K Rate constant, K2 =…

Q: A first-order reaction has rate constants of 4.6 x 10-2 s-1 and 9.8 x 10-2 s-1 at 0°C and 20.°C,…

Q: 11. A certain reaction has an activation energy of E₂ = 7.0 kJ/mol. The rate of this reaction at…

A: it lowers the activation energy required for the reaction to occur. This leads to an increase in the…

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

Q: The rate constant of a reaction exactly doubles when the temperature is changed from 25°C to 36°C.…

Q: The reaction between nitrogen dioxide and carbon monoxide is NO₂(g) + CO(g) → NO(g) + CO₂(g) The…

Q: 6. For a reaction at 25 °C, the activation energy of the forward reaction is 135 kJ and the…

A: Let us discuss the diagram and then answer the question.

Q: The initial rates of a reaction at different initial concentrations of the reactants were determined…

A: Given that, A + B ----> product rate, r= k [A]m[B]n where, m is the order of A with respect to B…

Q: Consider the reaction below at 100oC T2U (g) ⟶⟶ 2 T (g) + U (g) When [T2U] = 0.250 M, the…

A: The rate of the reaction is written in terms of the concentration of the reactant as: Rate = kT2Ux…

Q: The reaction rate constants of a reaction at 298 K and 373 K are 0.0450 s-1 and 20.1 s-1,…

A: The activation energy of a reaction at different temperatures can be determined from its rate…

Q: Calculate the activation energy for the reaction (in kJ/mol) when at 675 K the rate constant for the…

Q: 2 ClO (g) Cl2 (g) + O2 (g) Determine the activation energy (Ea) and frequency factor (A) for this…

A: Here i have determined values of both Ea and A

Q: For a certain reaction, the activation energy is found to be (1.77x10^1) kJ/mol. If the rate…

Q: The rate constant for a certain reaction is 2.5 x 10-° M min at 481 K. The activation energy for the…

A: The given question is based on the knowledge of the Arrhenius concept which relates the activation…

Q: 5. The measurement of reaction rates as a function of temperature provides information on the…

A: Rate of reaction is the change in the concentration of the reactants and products with respect to…

Q: The activation energy of an uncatalyzed reaction is 86 kJ/mol. The addition of a catalyst lowers the…

A: We will solve this question using arrhenius equation.

Q: The rate constant k for the reaction shown below is 2.6 × 10–8 L/mol⋅s when the reaction proceeds at…

A: k = Ae-Ea/RT where, k = Rate constant = 2.6 x 10-8 L/mol.s A = Frequency factor = ? Ea = Activation…

Question

A reaction
has a rate constant of
1.26×10-4 s-1 at 29 °C and 0.231 s-1
at 79 °C. part a) Determine the
activation barrier for the reaction. Part
b)What is the value of the rate
constant at 17 °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: Data given

VIEW

Step 2: Calculation of activation barrier

VIEW

Step 3: Rate constant at 17°C

VIEW

Solution

VIEW

Step by step

Solved in 4 steps with 3 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 student collected conducted 6 kinetics experiments for one reaction by holding the concentrations of ALL the reactants and catalyst constant and varying the temperature. After determining the rate constant for this reaction at the 6 different temperatures, an Arrhenius Plot was made. The graph resulted in a straight line. The equation for the straight line was: y= -4,257.15 x + 14.326 What is the Activation Energy (in Joules/mol) for this reaction at 30 oC? Do not include the units in your answer.
12.) The first-order rate constant for the reaction of methyl chloride (CH3Cl) with water to produce methanol (CH3OH) and hydrochloric acid (HCl) is 0.332 S-¹ at 25°C. Calculate the rate constant at 40°C if the activation energy is 116 kJ/mol.
100 80 A 60 PE (kJ) A+B 40 20 Progress of the reaction The activation energy is C+D The reaction is 3 KJ (endothermic or exothermic).
(6) : The rate of a particular reaction increases by a factor of 1.97 when the temperature is increased from 20°C to 30°C. Calculate the activation energy for this reaction.
Consider a hypothetical chemical reaction A + B → C, where A and B are reactants and C is the product. The reaction is known to have a high activation energy barrier. However, upon adding a catalyst, the reaction proceeds at a significantly faster rate. Explain the role of the catalyst in reducing the activation energy barrier and increasing the reaction rate.
Be sure to answer all parts. Use the data in the following table to determine the activation energy of the reaction: T(K) k (s−1) 625 1.1 × 10−4 635 1.5 × 10−4 645 2.0 × 10−4
A reaction having an activation energy of 55.1 kJ/mol has a rate constant of 4.2 x 10-8 s-1 when the temperature is 427. K. What is the rate constant (in s=1) when the temperature is 613. K?
Part A) The activation energy of a certain reaction is 30.5 kJ/molkJ/mol . At 20 ∘C∘C, the rate constant is 0.0130 s−10.0130 s−1. At what temperature would this reaction go twice as fast? Express your answer numerically in degrees Celsius Part B) Given that the initial rate constant is 0.0130 s−10.0130 s−1 at an initial temperature of 20 ∘C∘C, what would the rate constant be at a temperature of 100 ∘C∘C? Express your answer numerically in inverse seconds.
What is the activation energy of a reaction if it has the following rate constants? Rate Constant Temperature 6.20 x 10-4 s-1 700 K 2.39 x 10-2 s-1 760 K
Given the same reactant concentrations, the reaction CO(g) + Cl2(g) → COCl2(g) at 249°C is 48.4 times as fast as the same reaction at 169°C. Calculate the activation energy for this reaction. Assume that the frequency factor is constant.
1a) A(g) + B(g) C(g) The rate law for the above reaction is: -d[A]/dt = k[A][B] The rate constant is 1.13×102 L mol-1 s-1 at 346.0°C and 3.55×103 L mol-1 s-1 at 548.0°C. Use the Arrhenius equation k = Ae-Ea/RT to: Calculate Ea for this reaction. 1b) Calculate the rate constant k at 416.0°C for this reaction. 1c) Calculate the pre-exponential factor A for this reaction.
For a certain reaction, the activation energy is found to be (1.77x10^1) kJ/mol. If the rate constant is (3.6x10^-5) at (3.78x10^2) K, what is the rate constant at (6.290x10^2) K? R = 8.314 J/Kmol; T(K) = T(°C) + 273