- The following experimental data was collected for the reaction at 298 K.
- What is the reaction rate between 1.0 and 1.1 seconds?
- What is the reaction rate between 20.0 and 20.1 seconds?
- Assume that the reaction is first order and calculate the rate constant (k) for each of these times.
- Assume that the reaction is second order and calculate the rate constant (k) for each of these times.
- Based upon the above calculations what is the reaction order?
- Assume that the reaction is first order. Graph the data to show if this assumption is correct and if so use the graph to determine the rate constant.
- Assume that the reaction is second order. Graph the data to show if this assumption is correct and if so use the graph to determine the rate constant.
time

(seconds)[N _{2}O_{5}]

(mole*liter^{-1})0.0 1.500 x 10 ^{-3}1.0 1.1837 x 10 ^{-3}1.1 1.1560 x 10 ^{-3}10.0 1.4043 x 10 ^{-4}20.0 1.3147 x 10 ^{-5}20.1 1.2839x10 ^{-5}40.0 1.1522 x 10 ^{-7}100.0 7.7575 x 10 ^{-14} - The above experiment is repeated at several temperatures to obtain the following
experimental data. Based upon this experimental data, determine the activation energy for this
reaction and the preexponential factor.
T (C) rate constant (sec ^{-1})0 9.16 x 10 ^{-3}20 0.12919 40 1.2993 50 3.7017 70 25.017 - Using the constants determined above If the initial concentration of N
_{2}O_{5}is 3.0 x 10^{-4}M: - What is the concentration of NO
_{2}after 5 seconds at 10 C? - What is the concentration of N
_{2}O_{5}after 10 seconds at 10 C? - What is the concentration of NO
_{2}after 5 seconds at 20 C? - What is the concentration of N
_{2}O_{5}after 10 seconds at 20 C?

Please send comments or suggestions to svanbram@science.widener.edu

Scott Van Bramer

Department of Chemistry

Widener University

Chester, PA 19013

*© copyright 1996, S.E. Van Bramer*

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