Part C Write the rate law for the reaction between HCl and Na 2 S 2 O 3 . Part D

Question

Part C

Write the rate law for the reaction between HCl and Na2S2O3.

Part D

Using the rate law that you determined for the reaction in (C), predict the rate of the reaction if the concentration of HCl was changed to 0.8M and the concentration of Na2S2O3 is 0.12M.

Part E

Using the following rate law, and the experimental values given, calculate k:

Rate = k [F2][ClO2]

Experiment

[F2] (M)

[ClO2] (M)

Initial rate (M/s)

1

0.5

0.5

0.3 M/s

2

0.8

0.8

0.768 M/s

3

0.5

0.8

0.48 M/s

Experiment

[F2] (M)

[ClO2] (M)

Initial rate (M/s)

1

0.5

0.5

0.3 M/s

2

0.8

0.8

0.768 M/s

3

0.5

0.8

0.48 M/s

Explanation / Answer

Part E )

rate= k [F2]x [ClO2]y

we need find out x and y

from data

0.3 = k [0.5]x [0.5]y ------------->(1)

0.768 = k [0.8]x [0.8]y ------------------> (2)

0.48 = k [0.5]x [0.8]y ------------------> (3)

by solving equation 1 & 3 we get y = 1

bysolving equation 2 & 3 we get x = 1

then

rate= k [F2]x [ClO2]y

rate= k [F2]1 [ClO2]1

rate = 0.3 M/s

0.3 = k [0.5]1 [0.5]1

k = 1.2 M-1s-1

C )

rate = k [ HCl.][ Na2S2O3]

D )

rate = k [0.8][0.12]

Note : part C and part D some data is missing just check once and if you have any doubt upload properly again

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