Question

Constants | Periodic Table The following reaction was monitored as a function of time: A→B+C A...

Constants | Periodic Table

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

Previous Answers

Correct

Part C

Part complete

What is the half-life?

Express your answer using two significant figures.

t1/2 =

140

 s

Previous Answers

Correct

Part D

If the initial concentration of A is 0.220 M , what is the concentration after 235 s ?
[A] =
M

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Homework Answers

Answer #1

1. As the slope is given,The slope is the rate constant of the reaction.

Determining the units of rate constants can give us the order

Rate ∝ Concentration

Also the first order equation,

ln[A]=-kt + ln[Ao]

Hence,this is a first order reaction

As rate constant of 1st order is per second

rate constant (k)= 0.0050

2. Rate law= Rate=k[A]

3. Half life = ln2/rate constant= 40 seconds

4. Initial conc.= 0.220 Final be=x Time=235second,k=0.005

ln[A]=-kt + ln[Ao]

ln[Ao/A]=kt

ln[0.22/A]= 0.005*235

ln[0.22/A]=1.175

Taking anti log'

0.22/A=3.23

A=0.067

Final conc.= 0.067

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