Use the data from experimental trials 1 and 2. When the concentration of C2H5OH doubles from 0.15M to 0.30M, what happens to the initial rate? What kinetic order is present? Use experiments 2 and 3. When the concentration of Cr2O72- doubles from 0.050 M to 0.10 M, what happens to the initial rate? What kinetic order is presentWhen the concentration of H+ increases from 0.010M to 0.100 M, what happens to the initial rate? What kinetic order is present? Use experimental trials 2 and 4. Using the data from experiment 1, solve the reaction rate constant, K. Calculate the overall reaction order.
Use the data from experimental trials 1 and 2. When the concentration of C2H5OH doubles from 0.15M to 0.30M, what happens to the initial rate? What kinetic order is present? Use experiments 2 and 3. When the concentration of Cr2O72- doubles from 0.050 M to 0.10 M, what happens to the initial rate? What kinetic order is presentWhen the concentration of H+ increases from 0.010M to 0.100 M, what happens to the initial rate? What kinetic order is present? Use experimental trials 2 and 4. Using the data from experiment 1, solve the reaction rate constant, K. Calculate the overall reaction order.
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
Section11.1: Reaction Rate
Problem 11.2CE: Instantaneous rates for the reaction of hydroxide ion with Cv+ can be determined from the slope of...
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Questions:
- Use the data from experimental trials 1 and 2. When the concentration of C2H5OH doubles from 0.15M to 0.30M, what happens to the initial rate? What kinetic order is present?
- Use experiments 2 and 3. When the concentration of Cr2O72- doubles from 0.050 M to 0.10 M, what happens to the initial rate?
- What kinetic order is presentWhen the concentration of H+ increases from 0.010M to 0.100 M, what happens to the initial rate? What kinetic order is present? Use experimental trials 2 and 4.
- Using the data from experiment 1, solve the reaction rate constant, K.
- Calculate the overall reaction order.
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