Question
The following reaction was monitored as a function of time: AB→A+B A plot of 1/[AB] versus...
The following reaction was monitored as a function of time: AB→A+B A plot of 1/[AB] versus time yields a straight line with slope 5.8×10−2 (M⋅s)−1 .
What is the value of the rate constant (k) for this reaction at this temperature?
What is the half-life when the initial concentration is 0.55 M
If the initial concentration of AB is 0.220 M , and the reaction mixture initially contains no products, what are the concentrations of A and B after 70 s ?
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Answer #1
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The following reaction was monitored as a function of time: AB→A+B A plot of 1/[AB] versus...
The following reaction was monitored as a function of
time:
AB→A+B
A plot of 1/[AB] versus time yields a straight line with slope
5.8×10−2 (M⋅s)−1 .
1)What is the half-life when the initial concentration is 0.59 M
?
2)if the initial concentration of AB is 0.290 M , and the
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concentrations of A and Bafter 80 s ?
The following reaction was monitored as a function of time: AB→A+B A plot of 1/[AB] versus...
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The following reaction was monitored as a function of
time:
A→B+C
A plot of ln[A] versus time yields a straight
line with slope −5.0×10−3 /s .
Part A
Part complete
What is the value of the rate constant (k) for this
reaction at this temperature?
Express your answer using two significant figures.
k =
5.0×10−3
s−1
Previous Answers
Correct
Part B
Part complete
Write the rate law for the reaction.
Rate=k
Rate=k[A]
Rate=k[A]2
Rate=k[A]3
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