ost-Lab Questions (record the answers in you lab notebook): Part of your data an

Question

ost-Lab Questions (record the answers in you lab notebook): Part of your data analysis is to determine the order with respect to crystal violet. Based on your experimentally determined order, calculate the half-life. 1. X. 2. Assuming the CV initial concentration is 1.2 x 105 M, calculate the time required for the concentration to decrease to 40% of the initial value If the experimental rate l If the experimental rate law was determined to be 3. rate - k [OH] What would be the order with respect to CV and if the CV concentration increased by a factor of two, what effect would it have on the rate of reaction?

Explanation / Answer

1. Based on this data,

rate constant k = 0.2183 s-1

2. For a first order reaction,

ln[CV] = ln[CVo] - kt

with,

[CVo] = 1.2 x 10^-5 M

[CV] = 0.40 x 1.2 x 10^-5 = 4.8 x 10^-6 M

we get,

ln(4.8 x 10^-6) = ln(1.2 x 10^-5) - 0.2183 x t

t = 4.20 s

so it would take 4.20 s for the initial concentration to reduce to 40%.

3. If rate law is,

rate = k[OH-]

the order with respect to CV would be zero

Increasing the concentration of CV would not affect the rate of the reaction

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