The deadly gas phosgene is produced by reacting carbon monoxide with chlorine according the the reaction below: CO (g) + Cl2 (g) COCl2 (g) The following rate data was collected at a particulat temperature: Determine the rate law equation, and calculate the value of the rate constant with proper units; be sure to include a complete rate law equation at the end, with the value of the rate constant subbed in.

The deadly gas phosgene is produced by reacting carbon monoxide with chlorine according the the reaction below: CO (g) + Cl2 (g) COCl2 (g) The following rate data was collected at a particulat temperature: Determine the rate law equation, and calculate the value of the rate constant with proper units; be sure to include a complete rate law equation at the end, with the value of the rate constant subbed in.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter11: Chemical Kinetics: Rates Of Reactions

Section: Chapter Questions

Problem 36QRT

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For the reaction 2N2O5(g) → 4NO2(g) + O2(g), the following data were collected. t (minutes) [N2O5] (mol/L) 0 1.24 × 10–2 10. 0.92 × 10–2 20. 0.68 × 10–2 30. 0.50 × 10–2 40. 0.37 × 10–2 50. 0.28 × 10–2 70. 0.15 × 10–2 The concentration of O2 at t = 10. min is Question 16 options: A) 0.32 × 10–2 mol/L B) 2.0 × 10–4 mol/L C) 0.64 × 10–2 mol/L D) 0.16 × 10–2 mol/L E) none of these
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Consider the reaction A(g) + 2B(g) → 2C(g) + 2D(g) and associated that was collected at a constant temperature. Trial Initial [A] Initial [B] Initial Rate (mol/L) (mol/L) (mol/(L·min)) 1 0.125 0.200 7.25 2 0.375 0.200 21.75 3 0.250 0.400 14.50 4 0.375 0.400 21.75
Plot on to graph moles of S2O8 vs time to achieve M/s. The initial concentration of S2O8: 0.05M (added is 2.5mL of 0.200M, but it was diluted so 0.200 x 2.5/10mL = 0.05M). Below is the time (s) and moles consumed. 188s - 0.00002 moles 362s - 0.00004 moles 548s - 0.00006 moles 740s - 0.00008 moles 1001s - 0.0001 moles I was told to plot concentration vs time then subtract the moles, but I'm confused how to do that.
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Run Reactants Temperature (Celsius) Initial Rate (kPa/s) 1 10 ml 3% H2O2 = 5ml 0.5M KI 23.0 0.0798 2 5ml 3% H2O2 = 5ml 0.5 M KI 23.0 0.0391 3 5ml 3% H2O2 + 10ml 0.5 M KI 23.0 0.0794 Run Initial Rate (mol/L*s) [H2O2] after mixing [I-] after mixing 1 3.24 x 10^-5 0.147 M 0.0417 M 2 1.59 x 10^-5 0.0733 M 0.417 M 3 3.23 x 10^-5 0.0733 M 0.0833 M Calculate the rate law for the reaction
The decomposition of aqueous sucrose to form the isomers glucose and fructose is a common organic reaction, which requires a strong catalyst: C12H22O11(aq) + H2O(l) → 2C6H12O6(aq). The following data were collected during the process: Time (min) [C12H22O11] (mol/L) 0 0.316 39 0.274 80 0.238 140 0.190 210 0.146 (A) If we performed a new trial with an initial concentration of sucrose of 0.400 mol/L, what concentration would remain after 4.0 h has passed?
For the following reaction 6 experiments have been run and the data collected is in the following table: 2 MnO4-(aq) + 5 H2C2O4 (aq) + 6 H+ (aq) ---> 2 Mn2+ (aq) + 10 CO2 (g) + 8 H2O (l) Experiment [MnO4-], M [H2C2O4], M [H+], M Rate, M/s 1 0.2410 0.3470 0.2690 0.1147 2 0.3260 0.6210 0.2270 0.2776 3 0.5630 0.5740 0.7420 0.4431 4 0.2410 0.3470 0.3840 0.1147 5 0.4140 0.5740 0.5610 0.3258 6 0.3260 0.4930 0.4910 0.2203 a) Find the order of the reaction with respect to H+. _______________ b) Find the order of the reaction with respect to MnO4-. ______________ c) Find the order of the reaction with respect to H2C2O4. _____________ d) What is the overall order of the reaction? ________________________
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1. The decomposition of aqueous sucrose to form the isomers glucose and fructose is a common organic reaction, which requires a strong catalyst: C12H22O11(aq) + H2O(l) → 2C6H12O6(aq). The following data were collected during the process: Time (min) [C12H22O11] (mol/L) 0 0.316 39 0.274 80 0.238 140 0.190 210 0.146 (a)If we performed a new trial with an initial concentration of sucrose of 0.400 mol/L, what concentration would remain after 4.0 h has passed? 2. Methyl isomerizes to acetonitrile, CH3NC(g) → CH3CN(g) at 215°C. The following data were collected during the process: Time (sec) [CH3NC] (mol/L) 2000 0.0110 5000 0.0059 8000 0.0031 12000 0.0014 15000 0.0007 2. (a)Assuming the process continues, what concentration of methyl isonitrile would we expect after 5.00 h?
Consider the experimental data collected for the following chemical reaction: 2H2(g) + 2NO(g) → N2(g) + 2H2O(g) Trial Initial [H2] (mol/L) Initial [NO] (mol/L) Rate of Reaction (mol/L∙s) 1 0.031 0.0025 2.0 x 10-3 2 0.062 0.0025 4.0 x 10-3 3 0.031 0.0050 8.0 x 10-3 4 0.062 0.0050 1.6 x 10-2 Which action will have more effect on the rate of this reaction; changing the concentration of H2(g) or that of NO(g)? Explain your reasoning by considering the orders of reactants and writing the corresponding rate law equation.