The gas phase reaction of iodine with silane takes place according to a second-order reaction:I2(g) +SİH4(g)–→HI(g) +SIH3I(g)The activation energy is Ea = 83.2 kJ mol-1. At 269°C, the reaction rate constant is 3.49 L mols.(a) Calculate the Arrhenius factor A for this reaction.L mols1(b) Calculate the rate constant for this reaction at 235°C.L molls1

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Answered: The gas phase reaction of iodine with…

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...

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The gas phase reaction of iodine with silane takes place according to a second-order reaction: I2(9) +SiH4(9) HI(g) +SiH3I(g) The activation energy is Ea= 83.2 kJ mol-¹. At 271°C, the reaction rate constant is 3.73 L mol-1 s-1. (a) Calculate the Arrhenius factor A for this reaction. (b) Calculate the rate constant for this reaction at 253°C. Submit Answer Try Another Version L mol-1 s-1 1 item attempt remaining L mol-1 s-1
Be sure to answer all parts. Acetone is one of the most important solvents in organic chemistry. It is used to dissolve everything from fats and waxes to airplane glue and nail polish. At high temperatures, it decomposes in a first- order process to methane and ketene (CH,=C=0). At 600°C, the rate constant is 8.7 x 103 s1. (a) What is the half-life of the reaction? Give your answer in scientific notation. x 10 (select) A (b) How long does it take for 42% of a sample of acetone to decompose? (c) How long does it take for 82% of a sample of acetone to decompose? Give your answer in scientific notation. x 10 (select) O S
the rate of decomposition of hydrogen peroxide in dilute sodium hydroxide at room temperature is as follows: 2H2O2(aq)-> 2H2O(l) +O2(g). the reaction is a first-order in H2O2. The rate constant for the decomposition of H2O2 at 20oC is 1.8x10-5 s-1, and the initial concentration of H2O2 is 0.80 mol L-1. (i)What is the concentration of H2O2 after 8.0hours? (ii) how long will it take for the concentration of H2O2 to drop to 0.10M? (iii) how long will it take for 75% of the H2O2 to decompose? (iii)
(a) Suppose the rate of formation of Br2 is 4.0 x 10° M/s in a reaction in water described by the following net ionic equation: 5Br +BrO3¯ + 6H* → 3B12 + 3H20. What are the rates of reaction of each of the reactants and the reaction velocity? 14. (b) List two possible scenarios that may lead to zero-order reactions.
Chloroethane decomposes at elevated temperatures accord- ing to the reaction C:HSCI(g) → C2H4 (g) + HCl(g) This reaction obeys first-order kinetics. After 340 s at 800 K, a measurement shows that the concentration of C,H;Cl has decreased from 0.0098 mol L¯' to 0.0016 mol L-'. Calculate the rate constant k at 800 K.
Molecular iodine, I2(g), dissociates into iodine atoms at 625 K with a first-order rate constant of 0.271 s-1. (a) What is the half-life for this reaction? _______ s(b) If you start with 0.047 M I2 at this temperature, how much will remain after 5.18 s assuming that the iodine atoms do not recombine to form I2? _______ M
Writing the rate law implied by a simple mechanism Suppose the formation of nitrogen dioxide proceeds by the following mechanism: step elementary reaction rate constant 1 2 NO(g) → N,O2(9) 2 N2O2(9) + O2(9) → 2 NO,(9) olo Suppose als0 k, «k,. That is, the first step is much slower than the second. Write the balanced O-0 chemical equation for the overall chemical reaction: 믐 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 k = the reverse of the two elementary reactions in the mechanism. ||
The relative initial rates of the reaction A 2 + B 2→ products in vessels (a)-(d) are 1:1:4:4. Unshaded spheres represent A 2 molecules, and shaded spheres represent B 2 molecules present at the beginning of the reaction. 8. 8. 8 8|| 8 00 이| 8 6 (a) (b) (c) (d) What is the overall order of reaction? O - N 3
6
The rate of the elementary reaction O2 + H2H + HO2 has been studied as a function of temperature between 1000 and 1400 K. The following data were obtained for the rate constant k: (a) Calculate the activation energy of this reaction. kJ mol-1 (b) Calculate the factor A in the Arrhenius equation for the temperature dependence of the rate constant.
The rate constant for the first order reaction A ---> B + C is k = 0.016 min-1 at 300 K. What is the half-life for this reaction at 300 K?
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.

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