Constants | Periodic Table The following reaction was monitored as a function of

Question

Constants | Periodic Table

The following reaction was monitored as a function of time:
AB+C
A plot of ln[A] versus time yields a straight line with slope 5.0×103 /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.

5.0×103

Previous Answers

Correct

Part B

Part complete

Write the rate law for the reaction.

Previous Answers

Correct

Part C

Part complete

What is the half-life?

Express your answer using two significant figures.

140

Previous Answers

Correct

Part D

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

Request Answer

Constants | Periodic Table

The following reaction was monitored as a function of time:
AB+C
A plot of ln[A] versus time yields a straight line with slope 5.0×103 /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.

5.0×103

Explanation / Answer

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

Related Questions

Navigate

• Browse (All)
• Browse C
• Subjects