6. A student is performs the reaction below in three experiments studying initial concentrations and initial rates. The data is summarized in the table below. 2C10220HClO3 + CO2 + H₂O Experiment [ClO2] mol/L [OH] mol/L Rate (mol/L.s) 1 8.0 x 102 3.60 x 10 3.71 x 102 2 8.0 x 102 1.20 x 10 4.12 x 10 3 1.60 x 10-¹ 1.20 x 10 8.24 x 10-3 a. What is the order of this reaction with respect to CIO₂? b. What is the order of this reaction with respect to OH ? c. What is the overall order of this reaction? d. What is the rate law constant, k, for this reaction? (Be sure to include the value and the units.)

6. A student is performs the reaction below in three experiments studying initial concentrations and initial rates. The data is summarized in the table below. 2C10220HClO3 + CO2 + H₂O Experiment [ClO2] mol/L [OH] mol/L Rate (mol/L.s) 1 8.0 x 102 3.60 x 10 3.71 x 102 2 8.0 x 102 1.20 x 10 4.12 x 10 3 1.60 x 10-¹ 1.20 x 10 8.24 x 10-3 a. What is the order of this reaction with respect to CIO₂? b. What is the order of this reaction with respect to OH ? c. What is the overall order of this reaction? d. What is the rate law constant, k, for this reaction? (Be sure to include the value and the units.)

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

Every year Every second (1 year 365 days).
A chemist prepares a solution of nickel(II) chloride NiCl2 by measuring out 97.μmol of nickel(II) chloride into a 150.mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in mmol/L of the chemist's nickel(II) chloride solution. Round your answer to 2 significant digits.
Of the flasks or laboratory instruments that are given, express their function (specify -if they can be used to measure- if their measurements are approximate or relatively exact) Erlenmeyer flask beaker burette
A typical sports drink comes in a 20 fluid ounce bottle. 1 fluid ounce is 29.57 mL. Given your observed dye concentration, if you drank one bottle of sports drink per day for a year, how many grams of dye would you consume?
A chemist working as a safety inspector finds an unmarked bottle in a lab cabinet. A note on the door of the cabinet says the cabinet is used to store bottles of glycerol, carbon tetrachloride, pentane, tetrahydrofuran, and acetone. The chemist plans to try to identify the unknown liquid by measuring the density and comparing to known densities. First, from her collection of Material Safety Data Sheets (MSDS), the chemist finds the following information: liquid density glycerol -3 1.3 g-cm - 3 1.6 g cm carbon tetrachloride -3 0.63 g·cm pentane tetrahydrofuran -3 0.89 g·cm -3 0.79 g·cm acetone Next, the chemist measures the volume of the unknown liquid as 0.786 L and the mass of the unknown liquid as 991. g. Calculate the density of the liquid. Round your g. cm answer to 3 significant digits. yes Given the data above, is it possible to identify the liquid? no glycerol carbon tetrachloride pentane If it is possible to identify the liquid, do so. tetrahydrofuran acetone
Sand and iron particles that are similar in size and color are mixed together in a beaker. What would be the best method of separating the particles? A- Add water to the mixture B- Use tweezers to separate them. C- Pour the mixture into a filter. Use a magnet to separate them.
Example 2
A chemist prepares a solution of mercury(1) chloride (Hg₂Cl₂) by measuring out 1.96 mg of mercury(1) chloride into a 500. mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in mol/L of the chemist's mercury (1) chloride solution. Be sure your answer has the correct number of significant digits. mol/L mo x10 x S
The chemistry teacher needs a solution made up of a 3 g sugar cube (C6H1206) dissolved in a 250 ml teacup. Find the molarity of this solution. Be sure to report your answer to the correct number of significant figures. Do not include units.
Your 50 mL beaker has a mass of 5.85 g. You add 10.00 mL to the 50 mL beaker and now the total mass is 16.05 g. You originally used 5.29 g of NaCl to make the solution. What is the percent composition of your solution?
The chemical formula for hydrogen bromide is HBr. A chemist measured the amount of hydrogen bromide produced during an experiment. She finds that 5.9 g of hydrogen bromide is produced. Calculate the number of moles of hydrogen bromide produced. Be sure your answer has the correct number of significant digits. 477. mol x10 X S 4