Acetaldehyde decomposes to methane and carbon monoxide according
to the following balanced equation:
CH3CHO → CH4 + CO
In a particular experiment, the following kinetic data for the
decomposition of acetaldehyde were obtained:
Time(s) | 0 | 1000 | 2000 | 3000 | 4000 | |
[CH3CHO] (M) | 0.2160 | 0.1095 | 0.0734 | 0.0552 | 0.0442 |
What is the value of the rate constant at the temperature of
this experiment?
Give an answer with concentration units of molarity and time units
of seconds.
When you plot a graph of
1 / [Concentration] vs time
Your slope is the rate constant.
[CH3CHO] 1/[CH3CHO]
0.216 | 4.62962963 |
0.1095 | 9.132420091 |
0.0734 | 13.6239782 |
0.0552 | 18.11594203 |
0.0442 | 22.62443439 |
Now ploting the graph , we get slope = 0.0045 (as shown in the graph).
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