Help A reaction is found to have an activation energy of 108 kJ/mol. If the rate constant for this reaction is 4.60 × 10¯65-1at 275 K, what is the rate constant at 366 K?O 0.58 s1O 1.9 × 10-4 s-1O 1.7 s1O 12 s1O 5.4 x 10-5 s-1

Answered: Image /qna-images/answer/33773e0f-9e56-42dc-8dab-e0631e258584.jpg

Answered: A reaction is found to have an…

A reaction is found to have an activation energy of 108 kJ/mol. If the rate constant for this reaction is 4.60 x 10°6 s-1 at 275 K, what is the rate constant at 366 K?

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

Chapter12: Chemical Kinetics

Section: Chapter Questions

Problem 108CWP: Consider the hypothetical reaction A2(g) + B2(g) 2AB(g), where the rate law is: [A2]t=k[A2][B2] The...

See similar textbooks

Related questions

Q: The activation energy, Ea, for a particular reaction is 19.4 kJ/mol. If the rate constant at 80 °C…

Q: What is the activation energy of the reverse reaction if the forward reaction has an activation…

A: The activation energy of reversible reaction can be calculated by subtracting the enthalpy from the…

Q: A first-order reaction has rate constants of 4.6 x 10-2 s-1 and 5.6 x 10-2 s-1 at 0°C and 20.°C,…

Q: A certain reaction has an activation energy of 99.0 kJ/mol and a rate constant of 1.8 s-1 at 123.…

A: Given : Activation energy of reaction = 99.0 KJ/mol = 99000 J/mol.…

Q: The activation energy, Ea, for a particular reaction is

A: logK2K1 = Ea2.303 R 1T1 - 1T2 where K1 = 0.178 M/s at T1 = 280 K K2 = ? M/s at T2…

Q: The activation energy, Ea, for a particular reaction is 13.6 kJ/mol. If the rate constant at 754 °C…

Q: The rate constant of a reaction at 500 K and 700 K are 0.02 s-1 and 0.07 s-1 respectively. Calculate…

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

Q: Calculate the rate constant, k, for a reaction at 75.0 °C that has an activation energy of 82.7…

A: According to the Arrhenius equation, the rate constant can be calculated by knowing the frequency…

Q: The rate constant for a reaction is 1.08×10^7 M^-1 s^-1 at 298 K and 3.81 x 10^6 M^-1 s^-1 at 243K.…

A: Arrhenius equation:If we know the value of the rate constant at two different temperatures, we can…

Q: The activation energy for a particular reaction is 102 kJ/mol. If the rate constant is 1.35 x 10-ª…

Q: The activation energy for this reaction is 274 kJ mol^-1. By what factor does the rate of reaction…

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: The activation energy, Ea, for a particular reaction is 19.4 kJ/ mol. If the rate constant at 80 °C…

Q: A reaction has an activation energy of 195.0 kJ/mol. When the temperature is increased from 200°C to…

Q: The activation energy for a particular reaction is 102 kJ/mol. If the rate constant is 1.35 x 10-4…

Q: What is the activation energy for a reaction if the rate of the reaction doubles when the…

A: Temperature,T1 = 20°C or 293K Temperature,T2 = 35°C or 308K Value of Gas constant, R = 8.314J/mol K…

Q: The activation energy, Ea, for a particular reaction is 19.4 kJ/mol. If the rate constant at 80 °C…

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

Q: A second order reaction whose rate constant at 800 °C was found to be 5.0 x 10* L mol s' has an…

A: Given K1 = 5.0×10-3 L/mol.s T1 = 800°C T2 = 875°C Activation energy (Ea) = 45 kJ

Q: In the Haber process, nitrogen and hydrogen react together to produce ammonia, NH3 according to the…

Q: What is the activation energy in kJ/mol for a reaction that has a rate constant that is (2.73x10^0)…

A: Rate constant is temperature dependent

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

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

Q: The activation energy, Ea, for a particular reaction is 13.6 kJ/mol. If the rate constant at 754 °C…

A: Given, Activation energy , Ea = 13.6 Kj/mol = 13.6 x 103 J/mol K2 = 24.5 /min K1 = 19.5/min T2 =…

Q: The activation energy for a particular reaction is 102 kJ/ mol. If the rate constant is 1.35 x 10-4…

Q: The activation energy, Ea, for a particular reaction is 13.6 kJ/mol. If the rate constant at 475 K…

A: The relation between rate constant and temperature is given by Arrhenius Equation which is k =…

Q: A reaction has an activation energy of 3.79 kJ/mol. If the rate constant for the reaction is 6.4E-1…

A: Given activation energy, Ea = 3.79 kJ.mol-1 * (1000 J / 1kJ) = 3790 J.mol-1 Initial state: Initial…

Q: The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an…

A: Given information: Activation energy = 45.0 kJ/mol Rate constant (k1) = 1.8×104 M-1s-1 Temperature…

Q: The activation energy for a particular reaction is 102 kJ/mol. If the rate constant is 1.35 x 10 s1…

A: The rate constant will be calculated by using integrated arrhenius equation. Rate constant of…

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: When heated, cyclopropane is converted to propene. Rate constants for this reaction at 470. °C and…

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 activation energy for a particular reaction is 102 kJ/mol. If the rate constant is 1.35 × 10⁻⁴…

A: Activation energy at two different temperature related with rate constants. The relationship is…

Q: The activation energy, Ea, for a particular reaction is 37.8 kJ/mol. If the rate constant at 280 K…

A: Given,

Q: The activation energy, Ea, for a particular reaction is 13.6 kJ/mol. If the rate constant at 754 °C…

A: The relationship between rate constant , activation energy and temperature is given by Arrhenius…

Q: Calculate the rate constant, k, for a reaction at 57.0 °C that has an activation energy of 79.0…

A: Arrhenius equation is k = A. e(-Ea/RT), A= frequency factor Ea= Activation energy R=gas constant T=…

Q: The activation energy, Ea, for a particular reaction is 19.4 kJ/mol. If the rate constant at 80 °C…

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: Calculate the rate constant, k, for a reaction at 61.0 °C that has an activation energy of 78.9…

A: Answer:- This question is answered by using the simple formula of calculation of rate constant using…

Q: 4. A certain chemical reaction has a rate constant of 1.50 L/mol·min at 45.0°C with an activation…

A: The question is based on the concept of chemical kinetics. We have to calculate rate constant at…

Q: The activation energy, Ea, for a particular reaction is 37.8 kJ/mol. If the rate constant at 280 K…

A: The answer is given below

Q: The activation energy, Ea, for a particular reaction is 13.6 kJ/mol. If the rate constant at 754 °C…

Q: A particular reaction has an activation energy, Ea, of 189 kJ/mol. If the rate constant for the…

A: The Arrhenius equation establishes the relationship between activation energy (Ea), rate constants…

Q: The rate of a reaction becomes four times when the temperature changes from 293 K to 313 K.…

Q: Define activation energy Calculate the activation energy for a first order reaction, given that the…

Q: Determine the activation energy, Ea, (in kJ/mol) of the decomposition reaction, CH3CHO → CH4 + CO.…

A: Welcome to bartleby !

Q: The rate constant, k, for a first-order reaction is 1.36 x 10^3 s –1 at 90.°C and the activation…

A: Given-> K1 = 1.36 × 103 s-1 T1 = 90°C = 90 + 273 = 363 K K2 = ? T2 =…

Q: (b) For a particular reaction, the rate constant k is 2.8 x 105 L mol·' s'' at 27 °C and 7.0 x 10$ L…

A: The given data contains, Rate constant k1 =2.8 ×10-5 L mol-1 s-1Rate constant k2 =7.0 ×10-5 L mol-1…

Q: When a reaction is performed at a temperature of 314. K, the rate constant is 1.9 x 10-6 s-1. When…

A: Given,

Q: Calculate the rate constant, k, for a reaction at 54.0 °C that has an activation energy of 86.9…

A: Answer: This question is based on Arrhenius equation which is shown below: logk=-Ea2.303RT+logA…

Question

Help

A reaction is found to have an activation energy of 108 kJ/mol. If the rate constant for this reaction is 4.60 × 10¯65-1
at 275 K, what is the rate constant at 366 K?
O 0.58 s1
O 1.9 × 10-4 s-1
O 1.7 s1
O 12 s1
O 5.4 x 10-5 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

Step 3

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 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

11.35 For the reaction 2 NO(g) + 2 H?(g) — N,(g) + 2 H,O(g) at 1100°C, the following data have been obtained: [NOJ [HJ Rate = A(N2]/At (mol L~1) (mol L_1) (mol L-1 s_1) 5.0 X 10’1 0.32 0.012 1.0 X 10~’ 0.32 0.048 1.0 X 10"2 0.64 0.096 Derive a rate law for the reaction and determine the value of the rate constant.
The reaction NO(g) + O,(g) — NO,(g) + 0(g) plays a role in the formation of nitrogen dioxide in automobile engines. Suppose that a series of experiments measured the rate of this reaction at 500 K and produced the following data; [NO] (mol L ’) [OJ (mol L 1) Rate = -A[NO]/Af (mol L_1 s-1) 0.002 0.005 8.0 X 10"'7 0.002 0.010 1.6 X 10-'6 0.006 0.005 2.4 X IO-'6 Derive a rate law for the reaction and determine the value of the rate constant.
The following statements relate to the reaction for the formation of HI: H2(g) + I2(g) -* 2 HI(g) Rate = it[HJ [I2J Determine which of the following statements are true. If a statement is false, indicate why it is incorrect. The reaction must occur in a single step. This is a second-order reaction overall. Raising the temperature will cause the value of k to decrease. Raising the temperature lowers the activation energy' for this reaction. If the concentrations of both reactants are doubled, the rate will double. Adding a catalyst in the reaction will cause the initial rate to increase.
The reaction H2SeO3(aq) + 6I-(aq) + 4H+(aq) Se(s) + 2I-3(aq) + 3H2O(l) was studied at 0C, and the following data were obtained: [H2SeO3]0 (mol/L) [H+]0 (mol/L) [I]0(mol/L) Initial Rate (mol/L s) 1.0 104 2.0 102 2.0 102 1.66 107 2.0 104 2.0 102 2.0 10-2 3.33 107 3.0 104 2.0 102 2.0 102 4.99 107 1.0 104 4.0 102 2.0 102 6.66 107 1.0 104 1.0 102 2.0 102 0.42 107 1.0 104 2.0 102 4.0 102 13.2 107 1.0 104 1.0 102 4.0 102 3.36 107 These relationships hold only if there is a very small amount of I3 present. What is the rate law and the value of the rate constant? (Assumethatrate=[H2SeO3]t)
The reaction 2 NO(g) + 2 H2(g) N2(g) + 2 H2O(g) was studied at 904 C, and the data in the table were collected. (a) Determine the order of the reaction for each reactant. (b) Write the rate equation for the reaction. (c) Calculate the rate constant for the reaction. (d) Find the rate of appearance of N2 at the instant when [NO] = 0.350 mol/L and [H] = 0.205 mol/L.
Consider a hypothetical reaction between A and B: A + B products Use the following initial rate data to calculate the rate constant for this reaction. [A] (mol/L) [B] (mol/L) Initial Rate (mol/L s) 0.20 1.0 3.0 0.50 1.0 11.8 2.0 2.0 189.5
Consider the hypothetical reaction A2(g) + B2(g) 2AB(g), where the rate law is: [A2]t=k[A2][B2] The value of the rate constant at 302C is 2.45 104 L/mol s, and at 508C the rate constant is 0.891 L/mol s. What is the activation energy for this reaction? What is the value of the rate constant for this reaction at 375C?
The data in the table are for the reaction of NO and O2 at 660 K. NO(g) + O2(g) NO2(g) (a) Determine the order of the reaction for each reactant. (b) Write the rate equation for the reaction. (c) Calculate the rate constant. (d) Calculate the rate (in mol/L s) at the instant when [NO] = 0.015 mol/L and [O2] = 0.0050 mol/L. (e) At the instant when NO is reacting at the rate 1.0 104 mol/L s, what is the rate at which O2 is reacting and NO2 is forming?
Nitrogen monoxide reacts with chlorine according to the equation: 2NOCI(g)2NOCI(g) The following initial rates of reaction have been observed for certain reactant concentrations: [NO] (moI/L1) [CI2] (mol/L) Rate (moI/L/h) 0.50 0.50 1.14 1.00 0.50 4.56 1.00 1.00 9.12 What is the rate equation that describes the rate’s dependence on the concentrations of NO and CI2? What is the rate constant? What are the orders with respect to each reactant?
If a textbook defined a catalyst as "a substance that increases the rate of a reaction," would that definition be adequate?
Consider the following statements: In general, the rate of a chemical reaction increases a bit at first because it takes a while for the reaction to get warmed up. After that, however, the rate of the reaction decreases because its rate is dependent on the concentrations of the reactants, and these are decreasing. Indicate everything that is correct in these statements, and indicate everything that is incorrect. Correct the incorrect statements and explain.
At 40C, H2O2 (aq) will decompose according to the following reaction: 2H2O2(aq)2H2O(l)+O2(g) The following data were collected for the concentration of H2O2 at various times. Times(s) [H2O2](mol/L) 0 1.000 2.16 104 0.500 4.32 104 0.250 a. Calculate the average rate of decomposition of H2O2 between 0 and 2.16 104 s. Use this rate to calculate the average rate of production of O2(g) over the same time period. b. What are these rates for the time period 2.16 104 s to 4.32 104 s?