Please help, Calculate the activation energy (in I and kJ), the pre- exponential term, and the rate constant and please show the work, that way i'm able to do the other questions on my own, please please please. Determining Activation Energy Using a Graphical Method 1. The decomposition of formic acid is measured at several temperatures. The temperature dependence of its first order rate constant is: HCOOH(g) → CO:(g) + Hz(g) T(K) 800 825 850 875 900 925 k (s.¹) 0.00027 0.00049 0.00086 0.00143 0.00234 0.00372 Calculate the activation energy (in J and kJ), the pre-exponential term, and the rate constant

Please help, Calculate the activation energy (in I and kJ), the pre- exponential term, and the rate constant and please show the work, that way i'm able to do the other questions on my own, please please please. Determining Activation Energy Using a Graphical Method 1. The decomposition of formic acid is measured at several temperatures. The temperature dependence of its first order rate constant is: HCOOH(g) → CO:(g) + Hz(g) T(K) 800 825 850 875 900 925 k (s.¹) 0.00027 0.00049 0.00086 0.00143 0.00234 0.00372 Calculate the activation energy (in J and kJ), the pre-exponential term, and the rate constant

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 the reactionBr(g)+O3(g) --> BrO(g)+O2(g)was determined at the four temperatures shown in the table below. T (K) k [cm3/(molecule•s) 238 5.90 x 10-13 258 7.70 x 10-13 278 9.60 x 10-13 298 1.20 x 10-12 Plot the above data, and then use that data to calculate the activation energy for this reaction.
the following first rate constant order and determine the rate kr were obtained for the thermal decomposition of ethane . 10^5 Kr ( S^-1) = 2,3, 4.7, 8.2, 12.3, 23.1, 35.5 , 57.6, 92.40 , 141.5 . TEMPERATURE ( K) = 823, 833, 843, 853, 863, 873, 883, 893, 903 . From these value determine the activation energy and the pre- exponential factor , state clearly the unit in which these quantities were measured
1) For a particular chemical reaction, the rate constant at 30.0 °C is 1.38 x 10-4 L mol-1 s-1, while the value at 49.0 °C is 1.21 x 10-3 L mol-1 s-1. What is the activation energy for this reaction? A) 200 kJ mol-1 B) 343 kJ mol-1 C) 40.4 kJ mol-1 D) 56.4 kJ mol-1 1)
Suppose the decomposition of ozone proceeds by the following mechanism: step elementary reaction rate constant 1 03(g) O₂(g) + 0(g) k₁ 2 03(g) + O(g) → 20₂(g) k₂ Suppose also k₁ »k₂. That is, the first step is much faster than the second. Write the balanced chemical equation for the overall chemical reaction: Write the experimentally- observable rate law for the overall chemical reaction. rate = k Note: your answer should not contain the concentrations of any intermediates. Express the rate constant k for the overall chemical reaction in terms of K₁, K2, and (if necessary) the rate constants k.1 and k-2 for the reverse of the two elementary reactions in the mechanism. = 0 k = 00 X 5 S ?
The table shows the variation of the rate constant with temperature for the first-order reaction. 2N₂O5 (g) 2N₂O₂(g) + O₂(g) Determine graphically the activation energy for the reaction. Be sure your answer has the correct number of significant digits. T(K)|*(--) S 298. 1.74 x 10 308. 6.61 × 10 318. 2.52 × 10 328. 7.59 × 10 338. 2.40 × 10 - 5 -5 -4 -4 3 Note: Reference the Fundamental constants table for additional information.
n
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.
The rate for the reaction H2 (g) + Br2 (g) 2 HBr (g)is first order in both H2 and Br2 concentrations, and the rate constant k at 287 \deg C is 5.87\times 10-4 L mol-1 s-1. Suppose 1.00 L of H2 (g) at a concentration of 6.60\times 10-2 M is rapidly mixed with the same volume of Br2 (g) also at a concentration of 6.60\times 10-2 M. Calculate the time (in seconds) required for the H2 concentration to decrease to a value of 2.55\times 10-2 M. (Enter your answer to three significant figures.)
Reaction of nitric oxide gas (NO) and chlorine gas (Cl2) produces a very poisonous gas called nitrosyl chloride (NOCl). The experimental data of the reaction is given below. Use the data to calculate the specific rate constant K and overall order of the reaction. Please show full work!
Be sure to answer all parts. The second-order rate constant for the decomposition of nitrous oxide to nitrogen molecules and oxygen atoms has been determined at various temperatures: Determine the activation energy graphically. k(M−1 · s−1) T( ° C) 1.87 × 10−3 600 0.0113 650 0.0569 700 0.244 750
Enter your answer in the provided box. The variation of the rate constant with temperature for the first-order reaction 2N205(g) 2N204(g) + 02(g) is given in the following table. Determine graphically the activation energy in kJ/mol for the reaction. T(K)k(s1) 298 1.74 x 10-5 308 6.61 x 10-5 318 2.52 x 10 4 328 7.59 x 10 338 2.40 x 103 kJ/mol