The table gives the concentrations of C₂H₂O(g) as a function of time at a certain temperature for the reaction shown. C,H,O(g) — CH,(g)+CO(g) Verify that this is a first-order reaction by plotting In[C₂H₂O] versus time and determining the value of the rate constant. [C₂H4O] (M) 0.0860 0.0465 0.0355 0.0274 0.0174 Time (min) 0.00 56.0 80.0 103.0 144.0 k= 0.00022 Incorrect min

The table gives the concentrations of C₂H₂O(g) as a function of time at a certain temperature for the reaction shown. C,H,O(g) — CH,(g)+CO(g) Verify that this is a first-order reaction by plotting In[C₂H₂O] versus time and determining the value of the rate constant. [C₂H4O] (M) 0.0860 0.0465 0.0355 0.0274 0.0174 Time (min) 0.00 56.0 80.0 103.0 144.0 k= 0.00022 Incorrect min

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 data below were collected for this reaction: CH3Cl (g) + 3 Cl2(g) → CCl4 (g) + 3 HCl (g) Expt. [CH3Cl] (M) [Cl2] (M) Initial Rate (M/s) 1 0.050 0.050 0.014 2 0.100 0.050 0.029 3 0.100 0.100 0.057 Provide the rate law for this reaction. Include the numerical value of the specific rate constant, k. Rate = - Δ [Cl2]3 / Δ t Rate = Δ [HCl] / 3 Δ t Rate = k [CH3Cl] [Cl2]2 Rate = -Δ [CH3Cl] / 3 Δ t Rate = 5.7 [CH3Cl] [Cl2]
273.15 K = 0 °C NA = 6.02, RT/F = 0.025693 V (RT/F) In10 = 0.059160 V @ T = 298.15 K R = 8.3145 J K-1 mol-¹ = 0.082057 L atm K-1 mol-1 F = 96,485.3 C/mol 1 atm = 1.01325 bar = 760 Torr = 101325 Pa 1023 mol-1
The table gives the concentrations of C₂H₂O(g) as a function of time at a certain temperature for the reaction shown. C,H,Og) —CH,(g) +CO(g) Verify that this is a first-order reaction by plotting In[C,H,O] versus time and determining the value of the rate constant. [C₂H4O] (M) 0.0860 0.0465 0.0355 0.0274 0.0174 Time (min) 0.00 52.0 75.0 97.0 135.0 k == min!
A student studies the concentration of reactant A over time in a reaction and gathers the following data. Use a spreadsheet program (or graph on paper) to determine the order of the reaction with respect to [A] and the rate constant. Enter the numeric value of the rate constant with at least 2 sig figs. time (sec) 0 34.6 82.3 103.1 142.2 179.7 230.0 [A]t [M] 1.146 0.984 0.794 0.708 0.558 0.413 0.233
How do you find the order for [O2]?
The table gives the concentrations of C₂H₂O(g) as a function of time at a certain temperature for the reaction shown. C,H,Og) —CH,(g)+CO(g) Verify that this is a first-order reaction by plotting In[C,H,O] versus time and determining the value of the rate constant. [C₂H4O] (M) 0.0860 0.0465 0.0355 0.0274 0.0174 Time (min) 0.00 50.0 72.0 93.0 130.0 min
Given the information based on time and concentration, determine the order of the reaction and the rate constant k when graphing the following data: A--> C+D Time (s) (A] M 10 0.1000 50 0.0856 100 0.0749 200 0.0598 350 0.0460 500 0.0373 800 0,0271
At a certain temperature this reaction follows first-order kinetics with a rate constant of 0.00717 s : CICH,CH,CI (g) → CH,CHCI (g) + HCI (g) Suppose a vessel contains CICH,CH,Cl at a concentration of 1.00M. Calculate the concentration of CICH,CH,Cl in the vessel 89.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. |M Ox10 ?
Nitrosyl bromide decomposes by the reaction 2 NOBr(g) → 2 NO(g) + Br₂(g). Show that the following data are consistent with a second-order reaction and determine the second-order rate constant for the reaction. Students may do this by plotting the data three different ways. For each plot, time goes on the x-axis. A zero-order reaction is linear when [NOBr] on the y-axis. A first-order reaction is linear when In [NOBr] is on the y-axis. A second-order reaction is linear when 1/[NOBr] is on the y-axis. t [NOBr] 0 0.0653 OM-2.5-2 O M-¹. S-1 What are the units for the rate law? O M-2. s-1 OM-3. s-1 5 15 50 10 85 0.0514 0.0424 0.0361 0.0177 0.0117 What is the rate law for the reaction? (Rate equations take the general form 'rate = k. [A] . [B]'.) What is the value of the rate constant at the temperature of the experiment? 4.0✔ S M chemPad XX⁰ ← → Help Greek
A scientist already determined the rate of the reaction is first order with respect to I - . Determine the rate law and the value of k for the following reaction using the data provided. Hint, you only need to find the reaction order for S2O82⁻ because it is first order for I - . After you find the reaction order for S2O82⁻ you need to calculate k. S2O82⁻ (aq) + 3 I⁻ (aq) → 2 SO42⁻ (g) + I3⁻ (aq) [S2O82⁻ ]i (M) [I⁻ ]i (M) Initial Rate (M -1 s -1 ) 0.30 0.42 4.54 0.44 0.42 6.65 Rate = 120 M-2s-1 [S2O82⁻]2[I⁻] Rate = 195 M-3s-1 [S2O82⁻]2[I⁻] Rate = 86 M-2s-1 [S2O82⁻][I⁻] Rate = 23 M-1/2s-1 [S2O82⁻][I⁻] Rate = 36 M-1s-1 [S2O82⁻][I⁻]
At a certain temperature the rate of this reaction is second order in CICH₂CH₂Cl with a rate constant of 0.00455 M S -1 CICH₂CH₂Cl (g) → CH₂CHC1 (g) + HC1 (g) Suppose a vessel contains CICH₂CH₂Cl at a concentration of 1.11 M. Calculate the concentration of CICH₂CH₂Cl in the vessel 900. seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits.
Using an integrated rate law for a first-order reaction At a certain temperature this reaction follows first-order kinetics with a rate constant of 0.141 s¯¹: H₂CO3(aq) → H₂O (aq) + CO₂ (aq) Suppose a vessel contains H₂CO3 at a concentration of 0.290M. Calculate the concentration of H₂CO3 in the vessel 4.40 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 X Ś