The dependence of rate constant on temperature is normally given by the Arrhenius relation: k = Ae-Ea/RT It was noted that the rate constant of a certain reaction TRIPLED (increased by a factor of three) when the temperature increased from 50 degrees Celsius to 65 degrees Celsius. Calculate the activation energy (Ea) for this reaction. Select one:

The dependence of rate constant on temperature is normally given by the Arrhenius relation: k = Ae-Ea/RT It was noted that the rate constant of a certain reaction TRIPLED (increased by a factor of three) when the temperature increased from 50 degrees Celsius to 65 degrees Celsius. Calculate the activation energy (Ea) for this reaction. Select one:

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

Similar questions

The rate constant for a first-order reaction is 1.6  10–2s–1at 668 K and 5.1  10–2 s–1at 916 K. What is the activation energy? (R = 8.31 J/(mol · K))
A certain reaction has k = 8.82 x 10-4 s-1 at 373 K and k = 2.36 × 10-3 s-1 at 401 K. What is the numerical value of the activation energy (in kJ/mol) for this reaction? Give your answer to three sig figs.
The activation energy of a reaction is 33.4 kJ/mol. The rate constant for this reaction is 3.5 x 10-4 at 297.4 K. What is its rate constant at 347.7 K?
Initial-rate data at a certain temperature is given in the table for the reaction SO₂Cl₂(g) SO₂(g) + Cl₂(g) [SO₂Cl₂], (M) k= 0.100 0.200 0.300 Initial rate (M/s) 2.00 x 10-6 4.00 x 10-6 6.00 x 10-6 Determine the value and units of the rate constant. units:
The following data were obtained at constant temperature for the reaction: 4A(g) + 4B (g) → 3C(g) Initial [A] Initial [B] mol Experiment mol mol Initial Rate L-min L L 1 0.105 0.215 4.50 2 0.315 0.215 13.5 3 0.105 0.430 18.0 4 0.315 0.430 54.0 Part 1 of 2 Select the single best expression for the rate law for the reaction. Ok [A]³ [B]³ G Ok [A] [B] Ok [A] [B] Ok [A][B]²
The temperature dependence of the rate constant for the gas-phase reaction are as follows 2 N₂Os(g) Temperature (°C) K(s¹) 2.0 × 10 7.3 × 10-' 2.7 × 10 - 9.1 × 10 2.9 × 10-¹ Determine the values of activation energy (Ea) and frequency factor (A) for this reaction 20 30 40 50 60 4NO2(g) + O2(g) a. Activation energy = 1.22 kJ/mol and frequency factor = 2.14E+13 b. Activation energy = 101.21 kJ/mol and frequency factor = 30.70 c. Activation energy = 101.21 kJ/mol and frequency factor = 2.14E+13 d. Activation energy = 1.22 kJ/mol and frequency factor = 30.70 What is the volume at the equivalence point volume? a. 50.001 b. 50.000 IC 50.011 49.932 le 49.861 Clear my choice Liptoad YOUR eacel für showing all work
The activation energy for a particular reaction is 102 kJ/mol. If the rate constant is 1.35 × 10-4 s-¹ at 310 K, what is the rate constant at 273 K? 1 4 7 +/- 2 LO 5 8 1/s 3 6 9 O X C x 100
Consider a reaction A → B with activation energy 50.7 kJ/mol. At 19.5 °C, the rate constant, k, for this reaction is 0.095 s−1. Calculate the temperature, T (in °C), at which k = 0.329 s−1. Assume the pre-exponential factor (A) is constant with temperature. �=0.08206 L⋅atmmol⋅K=8.314 Jmol⋅K �K=�∘C+273.15 1 kJ = 1000 J Report your answer to three significant figures without the unit. Example: 20.0. Be sure that your answer is in °C and not Kelvin!
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
The reaction C₂H₂(g) → 2C₂H₂(g) - has an activation energy of 262 kJ/mol. At 600.0 K, the rate constant, k, is 6.1 x 10-8 s-1. What is the value of the rate constant at 820.0 K? k = 9.42 X10-26 Incorrect S-1
When a reaction is performed at a temperature of 314. K, the rate constant is 1.9 x 10-6 s-1. When performed at 457. K, the rate constant is 8.5 x 104s-1. Calculate the activation energy_(Ea) of this reaction, in units of kJ/mol.
The rate constant k for a certain reaction is measured at two different temperatures: temperature k 258.0 °C 3.9 x 1010 153.0 °C 1.5 × 1010 Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E, for this reaction. Round your answer to 2 significant digits. kJ E х10 a mol