Consider the following reaction: 2 CH3l (aq)C2H6 (g) + 12 (g)This reaction is first-order, and its rate constant, k at 25°C is 0.0115 s¹.a) If the initial concentration of CH3l is 6.75 M, what is the concentration of CH3I after the reaction has been carried out for 1.83 hours? Report your answer usingmost of the decimal places reported on your calculator. Do not use scientific notation[CH31]=Mb) If the rate constant is increased by a factor of 2.36 when the temperature is raised from 25°C to 76.6 °C, what is the activation energy (in kJ/mol) for this reaction? Report youranswer using most of the decimal places reported on your calculator. Do not use scientific notationEakJ/mol

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Answered: Consider the following reaction: 2 CH3l…

Chemistry

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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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At a certain temperature the rate of this reaction is second order in H₂CO3 with a rate constant of 2.44M *S : H₂CO3(aq) → H₂O (aq) + CO₂ (aq) Suppose a vessel contains H₂CO3 at a concentration of 0.840M. Calculate the concentration of H₂CO3 in the vessel 5.60 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 X
Bromide ion is oxidized by bromate ion in acidic solution. 5Br (aq) + BrO3 (aq)+ 6H"(aq) → 3Br,(aq) + 3H,O(1) The experimentally determined rate law is Rate = k[Br ][BrO; ]H7? What is the order of reaction with respect to each reactant species? What is the overall order of the reaction? Br order: O first order O second order O third order O fourth order O fifth order BrO3 order: O first order second order O third order
The decomposition of phosphorus pentachloride (PCI5) into phosphorus trichloride (PCI3) and chlorine gas (Cl2) is a first order process with a rate constant of 0.0842 s1 at a certain temperature. If 40.4 s after the reaction begins, the concentration of PCI; is 0.0203 M, what was the initial concentration of PCI;? 6.76 x 104 M (A) (B) 0.609 M (C) (D) 3.42 M 0.495 M (E) 0.820 Mt
The decomposition of N2O5 in solution in carbon tetrachloride proceeds via the reaction2N2O5 (soln) → 4NO2 (soln) + O2 (soln)The reaction is first order and has a rate constant of 4.82 × 10-3 s-1 at 64°C. If the reaction is initiated with 0.063 mol in a 1.00-L vessel, how many moles remain after 151 s? The decomposition of N2O5 in solution in carbon tetrachloride proceeds via the reaction2N2O5 (soln) → 4NO2 (soln) + O2 (soln)The reaction is first order and has a rate constant of 4.82 × 10-3 s-1 at 64°C. If the reaction is initiated with 0.063 mol in a 1.00-L vessel, how many moles remain after 151 s? 1.8 × 103 M 11 M 0.030 M 0.065 M 0.059 M
Calculate the concentration of HI in the vessel 89.0 seconds later.
The gas phase decomposition of hydrogen peroxide at 400 °C H2O2(g)H20(g) + ½ O2(g) is second order in H2O2. In one experiment, when the initial concentration of H,O2 was 0.242 M, the concentration of H,O, dropped to 4.09×10 M after 23.5 seconds had passed. Based on these data, the rate constant for the reaction is M1s1.
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
At a certain temperature the rate of this reaction is second order in C1₂0, with a rate constant of 4.83M¯¹ -1 S : 2C1₂05 (g) → 2Cl₂ (g) +50₂ (g) Suppose a vessel contains C1₂05 at a concentration of 1.28M. Calculate how long it takes for the concentration of Cl₂O5 to decrease to 19.0% of its initial value. You may assume no other reaction is important. Round your answer to 2 significant digits. S x10 ? X Ś
At a certain temperature the rate of this reaction is second order in HI with a rate constant of 0.22M¹s¹: 2 HI(g) → H₂(g) + 1₂ (8) Suppose a vessel contains HI at a concentration of 0.910M. Calculate how long it takes for the concentration of HI to decrease to 0.064 M. You may assume no other reaction is important. Round your answer to 2 significant digits. 0.9 X 圖图

At a certain temperature the rate of this reaction is second order in SO₂ with a rate constant of 0.013 M¹s¹: 2SO3 (g) → 2SO₂(g) + O₂(g) Suppose a vessel contains SO3 at a concentration of 1.36M. Calculate how long it takes for the concentration of SO3 to decrease by 91.%. You may assume no other reaction is important. Round your answer to 2 significant digits. ? Submit Ass Continue Ⓒ2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | A 80°F Partly sunny e here to search B D x10 X S O
The decomposition of hydrogen peroxide is described by the equation: 2H₂O₂ (aq)-2H₂O(0) + O₂(g) The reaction is first order in H₂O₂. It takes 10.0 hours for the concentration of H₂O₂ to drop from 2.0 M to 1.0 M. How many hours are required for the concentration of H₂O₂ to drop from 0.80 M to 0.050 M? 15.0 40.0 50.0 30.0 20.0 OOOOO R

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