2. Chloroform (CHCI3) is a known anesthetic. It is also used to produce therefrigerant carbon tetrachloride (CCCA) according to the reactionCHCI3(g) + Cl2(g) Cl«(9) + HC(g)Several experiments obtained the following data:Initial [CHCI3](M)Initial [Cl2] (M)Initial Rate ofExperimentReaction (M/s)0.00110.0142.60 x 10-4II0.00110.0285.20 x 10-4II0.00220.0282.08 x 10-3IV0.00220.0141.04 x 10-3Write the rate law expression for this reaction. Determine the value of the rate constant.

The rate law for the reaction can be written as: rate=kCHCl3xCl2y ......(1) Here, x is the order…

Answered: Chloroform (CHCI3) is a known…

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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A possible reaction mechanism for the formation of NO2F is shown below. What is the molecularity of the rate-limiting step? (1) NO2(g) + F2(g) ↔ NO2F(g) + F(g) Slow, rate determining (2) F(g) + NO2(g)↔ NO2F(g) Fast, equilibrium
Use the References to access important values if needed for this question. A proposed mechanism for one of the pathways for the destruction of ozone in the atmosphere is: step 1 slow: 03 + NO → NO₂ + O₂ step 2 fast: NO₂+ONO + 0₂ (1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. + (2) Which species acts as a reaction intermediate? Enter formula. If none, leave box blank: Rate = - (3) Complete the rate law for the overall reaction that is consistent with this mechanism. (Use the form k[A][B]"..., where '1' is understood (so don't write it) for m, n etc.) Submit Answer Retry Entire Group 9 more group attempts remaining €
A proposed mechanism for one of the pathways for the destruction of ozone in the atmosphere is: step 1 slow: 03 + NO → NO2 + O2 step 2 fast: NO₂+0 → NO + O₂ (1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. + + (2) Which species acts as a catalyst? Enter formula. If none, leave box blank: (3) Which species acts as a reaction intermediate? Enter formula. If none, leave box blank: Rate = (4) Complete the rate law for the overall reaction that is consistent with this mechanism. (Use the form k[A][B]"..., where '1' is understood (so don't write it) for m, n etc.)
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The bromination of acetone is acid-catalyzed: CH3COCH3 + Br₂ The rate of disappearance of bromine was measured for several different concentrations of acetone, bromine, and H ions at a certain temperature: Part: 0/2 Part 1 of 2 Skip Part Experiment [CH₂COCH,] (M) [Br₂] (M) [H] (M) (1) (2) (3) (5) H catalyst Check 0.400 0.400 0.400 0.532 →CH3COCH₂Br + H + Br 0.532 What is the rate law for the reaction? 0.0400 0.0800 0.0400 0.0400 0.0400 rate=k[CH₂COCH₂] [B₂] [H]] 0.0400 X 0.0400 0.0800 0.160 0.0400 00 S Rate of Disappearance M of Br 5.80 x 10 5.80 × 10-5 5 1.16× 10 4 3.08 × 10 7.71 × 10 4 0 E 9 C
(a) Consider the combustion of butane, given below: If C4H10(9) is decreasing at the rate of 0.880 mol/s, what are the rates of change of O₂(g), CO₂(g), and H₂O(g)? AO₂(g)/At = ACO₂(g)/At = AH₂O(g)/At = mol/s mol/s APtot/At = mol/s (b) The decomposition reaction given below: 2 NOCI(g) → 2 NO(g) + 1 Cl₂(g) is carried out in a closed reaction vessel. If the partial pressure of NOCI(g) is decreasing at the rate of 837 torr/min, what is the rate of change of the total pressure in the vessel? 2 C4H10(9) + 13 O₂(g) → 8 CO₂(g) + 10 H₂O(g) torr/min
Consider this reaction: 2SO3 (g) →2SO₂ (g) +0₂ (8) At a certain temperature it obeys this rate law. rate = (2.99 M¹.5-¹) [SO] Suppose a vessel contains SO3 at a concentration of 0.160 M. Calculate the concentration of SO3 in the vessel 24.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M 0 x10 X G
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Use this data for the following four (4) questions: The relative initial rates of the reaction A2 + B2-products in vessels (a)-(d) are 1:1:4:4. The spheres represent the number of molecules of present at the beginning of the reaction. [Unshaded spheres = A2 molecules; shaded spheres = B2 molecules] %3D For example, vessel (a) contains 2 A2 molecules and 2 B2 at the beginning of the reaction. Rate = 1 Rate 1 Rate = 4 Rate = 4 %3D 2. 8. 80 (c) (a) 11) What is the order of reaction with respect to A2? (b) (d) BA 11) A))0 B) 1 C) 2 D) 3 12) What is the order of reaction with respect to B2? 12) C A) 0 B) 1 D) 3 13) o c 13) What is the overall order of reaction? A) 0 B) 1 D) B 14) 14) What is the rate law for this reaction? B) Rate k[B2]2 D) Rate = k[A2]2[B2]² A) Rate = k[A2]² %3D C) Rate = k[A2][B2] %3D %3D nation below: 15) 8. 8.
Choose the correct molecularity and rate law for each of the elementary reactions shown below. (a) Cl(g) + CCl3(g) CCl4(9) Molecularity: ---Select--- V (b) SO3(9) SO₂(g) + 0(g) Molecularity: ---Select--- (c) NO₂(g) + SO₂(g) NO(g) + SO3(9) Molecularity: ---Select--- (d) 2 NO₂(g) N₂04(9) Molecularity: ---Select--- (e) CH₂OOCH3(g) 2 CH₂O(g) Molecularity: ---Select--- Rate Law: Rate = k [CC14]² Rate = k [CI] [CC13] Rate = k [CI]² [CC13]² Rate = k [CCl4] Rate Law: Rate = k [S0₂] [0] Rate = k [SO3] Rate = k [SO3]² O Rate = k [S0₂]² [0]² Rate Law: O Rate = k [NO₂] [SO₂] Rate = k [NO₂]² [S0₂]² O Rate = k [NO]² [S03]² O Rate = k [NO] [S03] Rate Law: O Rate = k [NO ₂] Rate = k [N₂04]² Rate = k [N₂04] O Rate = k [NO₂]² Rate Law: O Rate = k [CH30] Rate = k [CH300CH3]² Rate = k [CH30]² Rate = k [CH3OOCH3]
Be sure to answer all parts. The reaction between NO2 and CO to produce NO and CO2 is thought to occur in two steps: Step 1: NO2 + NO2 NO + NO3 Step 2: NO3 + CO NO2 + CO2 The experimental rate law is rate = k[NO2]2. (a) Write the equation for the overall reaction. Do not include phase abbreviations. (b) Identify the intermediate(s). NO3 NO2 NO CO2 CO (c) Identify the rate-determining step. Step 1 Step 2 Neither step
View Policies Show Attempt History Current Attempt in Progress X Incorrect. -1 The catalyzed decomposition of ethanol at 327°C has a rate constant of 4,00 x 105 L mol¹1A graph of the reciprocal of ethanol concentration versus time gives a straight line. The chemical equation for the reaction at this temperature is C₂H₂OH(g)-CHg) + H₂O(g) If the initial concentration of ethanol is 0.023 mol L¹, how long will it take for the pressure to reach 1.4 atm at 327°C? i 60 eTextbook and Media Hint 1. The unit of the rate constant indicates the order of reaction. 2. Use partial pressures and the universal gas law to calculate moles and concentrations. 3. Set up a table showing initial molar concentrations and concentrations at time t Save for Later 45 hours 80 d F4 MacBook Air F6 Attempts: 4 of 15 used Submit Answer Assistance Used 8: DII 8² St

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