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10 Nov 2019

Compare the average rate from trials 1 and 2 to the average rate of trials 5 and 6 to determine the order in I-. Report the order in I-. Show your work.

Trial

[FeCl3](M)

[KI] (M)

Average initial rate (units of absorbance/s)

Value must have >1 sig figure

1, 2

.01

.005

.00155

3, 4

.005

.01

.0021

5, 6

.01

.01

.0032

.

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Trinidad Tremblay
Trinidad TremblayLv2
13 Apr 2019

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Related questions

Can you please help post lab question..

DATA AND CALCULATIONS

Absorbance

Trial 1

0.039

Trial 2

0.045

Trial 3

0.063

Trial 4

0.086

Absorbance of standard (Trial 5)

0.792

Temperature

25°C

Kc expression Kc =

[Fe3+]i

Trial 1

Trial 2

Trial 3

Trial 4

[SCN–]i

[FeSCN2+]eq

[Fe3+]eq

[SCN–]eq

Kc value

Average of Kc values

Kc = ________________________ at ___25_____°C

beaker

Fe(NO3)3
(mL)

KSCN
(mL)

H2O
(mL)

1

5

2

93

2

5

3

92

3

5

4

91

4

5

5

90

PROCESSING THE DATA
1. Write the Kc expression for the reaction in the Data and Calculation table.
2. Calculate the initial concentration of Fe3+, based on the dilution that results from addingKSCN solution and water to the original 0.0020 M Fe(NO3)3 solution. See Step 2 of theprocedure for the volume of each substance used in Trials 1-4. Calculate [Fe3+]i using theequation:

[Fe3+]i =

Fe(NO3)3 mLtotal mL X (0.0020 M)

This should be the same for all four test tubes.
3. Calculate the initial concentration of SCN–, based on its dilution by Fe(NO3)3 and water:

[SCN–]i =

KSCN mLtotal mL X (0.0020 M)

In beaker 1, [SCN–]i = (2 mL / 100 mL)(.0020 M) = .000040 M. Calculate this for the otherthree beakers.
4. [FeSCN2+]eq is calculated using the formula:

[FeSCN2+]eq =

AeqAstd

X [FeSCN2+]std

where Aeq and Astd are the absorbance values for the equilibrium and standard solutions,
respectively, and [FeSCN2+]std = (1/100)(0.0020) = 0.000020 M. Calculate [FeSCN2+]eq foreach of the four trials.
5. [Fe3+]eq: Calculate the concentration of Fe3+ at equilibrium for Trials 1-4 using the equation:

[Fe3+]eq = [Fe3+]i – [FeSCN2+]eq

6. [SCN–]eq: Calculate the concentration of SCN- at equilibrium for Trials 1-4 using theequation:

[SCN–]eq = [SCN–]i – [FeSCN2+]eq

7. Calculate Kc for Trials 1-4. Be sure to show the Kc expression and the values substituted infor each of these calculations.
8. Using your four calculated Kc values, determine an average value for Kc.

the final concentrations of Iodate for runs 1 through 6 are shown in table 2.2. show how the final concentration fo run 4 was obtained by using values in table 2..4 and the balanced chemical equation for this reaction. you have to perform calculations and show all work


5So3 + 2IO+ 2H -----> I2 + 5So4 + H20


solution A, ml

.02 M KIO3 and .02 K2SO4 run 4= 25ml of solution A and 50 ml H20


solution B, ml

.01 M Na2SO3, .039M H2SO4 and 2% starch run 4= 25 ml of solution B and 50 ml H20


initial concentration of IO for run 4= .005 M and final concentration for run 4= .004 M

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