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Data Sheet & Calculations. Part I: For this part of the experiment assume (SCN-1 = (FeSCN21...
Partner: Data Sheet & Calculations. Part I: For this part of the experiment assume (SCN"]= FeSCN21...
Partner: Data Sheet & Calculations. Part I: For this part of the experiment assume (SCN"]= FeSCN21 Table 3: Trial % Transmittance [SCN); [Fe(SCN)?) Absorbance 2 89.9 0.00004 0.0462 0.00004 3 79.1 0.00008 0-1018 0.00012 4 66.1 10.17918 000012 5 58.3 0.00016 10.2343 o.ooola 0.00020 6 51.0 0.2924 0.00 02 apb00% Calculate the [SCN Ji and [Fe3+]; accounting for dilution using MeV. - MV., for each solution in Table 1. Show one sample calculation for absorbance, (SCN) and [FeSCN?"). Enter all...
Beers law solve for E3 and E4 showing work Part II. Equilibrium Constant Calculations Calculate the...
Beers law solve for E3 and E4 showing work
Part II. Equilibrium Constant Calculations
Calculate the initial moles of Fe3+ and SCN- for solutions E2
through E6 and record these values in the table on your Data Sheet.
You obtain the moles of the reactants by multiplying their molarity
by the volume (in L) of their solution used.
Determine the equilibrium concentration of FeSCN2+ for each of
the solutions E2-E6 from your Beer’s Law plot. Using these
equilibrium concentrations, the...
I need the whole table to be completed and calculations only for E2 Beer's Law Plot...
I need the whole table to be
completed and calculations only for E2
Beer's Law Plot 0.45 Concentr. Absorbance 0 0 0.00004 0.074 0.00008 0.171 0.00012 0.252 0.00016 0.338 0.0002 0.416 0.4 0.35 I 0,3 y = 2109.3x -0.0024 R2 = 0.9991 0.25 Absorbance (A) 0.2 0.15 0.1 0.05 0 0 0.00005 0.0001 0.00015 0.0002 Concentration(FeSCN2+] Part II. Equilibrium Mixtures Stock solution concentration, [NaSCN) = 0.00200 M (in 0.10 M HNO3) Stock solution concentration, [Fe(NO3)3] = 0.00200 Min 0.10 M...
Calculate [Fe3+] and [SCN-] for each of the nine trials. Show the calculations for Sample 1...
Calculate [Fe3+] and [SCN-] for each of the nine trials. Show
the calculations for Sample 1
calibration curve is y=3967.7x-0.0822
the R^2 value is y=0.09959
Solution [SCN-1 2.06764 Stock solution B Absorbance Dilution 1 (50.0%) 1.0 xl-4 0.723 Dilution 2 (25.0%) S.Oxon Dilution 3 (12.5%) 2.5X2.5 (FeSCN2+). 2.0 X10" 1.0X10-4M 5.0x105m 2.5x105m 0.289 1o.lll 10.036 Calibration curve trendline equation Y 3967.7% -0.0823 R2 value of trendline R 0.99 se Sample Number 0.0020 M Fe(NO2), (ml) 0.0020 M KSCN (mL) 8...
. Determination of an equilibrium constant Use the calculated absorbance values from Table 4 in Part...
. Determination of an equilibrium constant Use the calculated absorbance values from Table 4 in Part II (y values and the best-fit line equation from Part I to calculate the [FeSCN2"), at equilibrium. Show two sets of calculations and complete Table 6 below. Sample Calculation with hypothetical values of Absorbance from Table 4 & fitted egn. from Table 3 y = mx + b (y is absorbance) 0.0620 - 2000x -0.0250 x-0.0620+ 0.0250 2000 = 4.35 x 10 с D...
can you please help me with this Data and Calculations Trial 0:29 Absorbance 0.378 Je 0.086...
can you please help me with this
Data and Calculations Trial 0:29 Absorbance 0.378 Je 0.086 Trial 2 0.47 Trial 3 0.632 Trial 4 0.729 0.686 Absorbance of standard Triw. 329 0.6 6 Temperature ke [Fe(SCN) 2+]/([Fe3+] [SCN-]) Ferrag) + SCN Cag) 2 FescN2t (ag) Absorbance of standard (Trial) Temperature 0.3 Ke expression: [Fe] 0.0010 [SCN) 10.00040 [FeSCN? Jeg [Fe [SCN ] Ke value Average of Ke values Percent error (see pg 7): (Discuss this result as part of your...
Data and Calculations: Determination of the Equilibrium Constant for a Chemical Reaction Method II Volume in...
Data and Calculations: Determination of the Equilibrium Constant for a Chemical Reaction Method II Volume in mL 2.00 x 103 M Fe(NO) Volume in mL, Depth in mm Volume in ml. 2.00 x 103 M Method I Mixture Unknówn KSCN Water Absorbance Standard FESCNP 4mL 1 5.00 x 10 M 1,00 .227 3mL 2 5,00 202 x 10 M 2,00 90 x 10 M .304 3 5,00 3.00 2mL 955 x 104 M I ImL 4 5.00 4,00 19x 10...
please do 1 through 4. Thank you. 0 1. Fe 1.SCN Procedure B: 1. Prepare ICE...
please do 1 through 4. Thank you.
0 1. Fe 1.SCN Procedure B: 1. Prepare ICE tables for beakers 2 - 6 using the example below as a guideline (you will have 5 different ICE tables). Table 3. Sample "ICE" table. Fe(aq)*3 + SCN(aq) = FeSCN2 Initial: **M calculated **M calculated using your Table 2 using your Table 2 volumes volumes Change: - 1x - 1x Equilibrium: M 1x 1x = concentration calculated from Procedure A slope-intercept equation +1x M...
So basically, this excel sheet shows how to get the Equilibrium Constant of Fe+3 + SCN-...
So basically, this excel sheet shows how to get the Equilibrium
Constant of Fe+3 + SCN- ⇆ FeSCN+2
and I'm not sure what I need to change in to formulas to replicate
this solution for Fe+3 + 2
SCN- ⇆ Fe(SCN)2+1
Thanks.
Laboratory Data 0.4084 Slope of cal curve (from your pre-lab -- the mo [Fe(NO3)3] 0.002 [KSCN] 0.002 from the bottles in the lab. from the bottles in the lab. Data analysis part 1 For Fe3+ + SCN- <=>...
For each equilibrium sample, calculate the initial concentrations (assuming no reaction occurred)...
For each equilibrium sample, calculate the initial
concentrations (assuming no reaction occurred) of SCN–
and Fe3+ based on the dilution factors used.
Enter the absorbance values for each sample.
For the standard solution, assume that, when equilibrium is
reached, the [FeSCN2+]eq is equal to
[SCN–]ini. Why is this a good
assumption?
For the equilibrium solutions, calculate the
[FeSCN2+]eq (Ceq) using Eq.
4.
Using Eq. 5 and 6, calculate
[Fe3+(aq)]eq and
[SCN–(aq)]eq for each equilibrium
solution.
Calculate values for the equilibrium...
Partner: Data Sheet & Calculations. Part I: For this part of the experiment assume (SCN"]= FeSCN21 Table 3: Trial % Transmittance [SCN); [Fe(SCN)?) Absorbance 2 89.9 0.00004 0.0462 0.00004 3 79.1 0.00008 0-1018 0.00012 4 66.1 10.17918 000012 5 58.3 0.00016 10.2343 o.ooola 0.00020 6 51.0 0.2924 0.00 02 apb00% Calculate the [SCN Ji and [Fe3+]; accounting for dilution using MeV. - MV., for each solution in Table 1. Show one sample calculation for absorbance, (SCN) and [FeSCN?"). Enter all...
Beers law solve for E3 and E4 showing work
Part II. Equilibrium Constant Calculations
Calculate the initial moles of Fe3+ and SCN- for solutions E2
through E6 and record these values in the table on your Data Sheet.
You obtain the moles of the reactants by multiplying their molarity
by the volume (in L) of their solution used.
Determine the equilibrium concentration of FeSCN2+ for each of
the solutions E2-E6 from your Beer’s Law plot. Using these
equilibrium concentrations, the...
I need the whole table to be
completed and calculations only for E2
Beer's Law Plot 0.45 Concentr. Absorbance 0 0 0.00004 0.074 0.00008 0.171 0.00012 0.252 0.00016 0.338 0.0002 0.416 0.4 0.35 I 0,3 y = 2109.3x -0.0024 R2 = 0.9991 0.25 Absorbance (A) 0.2 0.15 0.1 0.05 0 0 0.00005 0.0001 0.00015 0.0002 Concentration(FeSCN2+] Part II. Equilibrium Mixtures Stock solution concentration, [NaSCN) = 0.00200 M (in 0.10 M HNO3) Stock solution concentration, [Fe(NO3)3] = 0.00200 Min 0.10 M...
Calculate [Fe3+] and [SCN-] for each of the nine trials. Show
the calculations for Sample 1
calibration curve is y=3967.7x-0.0822
the R^2 value is y=0.09959
Solution [SCN-1 2.06764 Stock solution B Absorbance Dilution 1 (50.0%) 1.0 xl-4 0.723 Dilution 2 (25.0%) S.Oxon Dilution 3 (12.5%) 2.5X2.5 (FeSCN2+). 2.0 X10" 1.0X10-4M 5.0x105m 2.5x105m 0.289 1o.lll 10.036 Calibration curve trendline equation Y 3967.7% -0.0823 R2 value of trendline R 0.99 se Sample Number 0.0020 M Fe(NO2), (ml) 0.0020 M KSCN (mL) 8...
. Determination of an equilibrium constant Use the calculated absorbance values from Table 4 in Part II (y values and the best-fit line equation from Part I to calculate the [FeSCN2"), at equilibrium. Show two sets of calculations and complete Table 6 below. Sample Calculation with hypothetical values of Absorbance from Table 4 & fitted egn. from Table 3 y = mx + b (y is absorbance) 0.0620 - 2000x -0.0250 x-0.0620+ 0.0250 2000 = 4.35 x 10 с D...
can you please help me with this
Data and Calculations Trial 0:29 Absorbance 0.378 Je 0.086 Trial 2 0.47 Trial 3 0.632 Trial 4 0.729 0.686 Absorbance of standard Triw. 329 0.6 6 Temperature ke [Fe(SCN) 2+]/([Fe3+] [SCN-]) Ferrag) + SCN Cag) 2 FescN2t (ag) Absorbance of standard (Trial) Temperature 0.3 Ke expression: [Fe] 0.0010 [SCN) 10.00040 [FeSCN? Jeg [Fe [SCN ] Ke value Average of Ke values Percent error (see pg 7): (Discuss this result as part of your...
Data and Calculations: Determination of the Equilibrium Constant for a Chemical Reaction Method II Volume in mL 2.00 x 103 M Fe(NO) Volume in mL, Depth in mm Volume in ml. 2.00 x 103 M Method I Mixture Unknówn KSCN Water Absorbance Standard FESCNP 4mL 1 5.00 x 10 M 1,00 .227 3mL 2 5,00 202 x 10 M 2,00 90 x 10 M .304 3 5,00 3.00 2mL 955 x 104 M I ImL 4 5.00 4,00 19x 10...
please do 1 through 4. Thank you.
0 1. Fe 1.SCN Procedure B: 1. Prepare ICE tables for beakers 2 - 6 using the example below as a guideline (you will have 5 different ICE tables). Table 3. Sample "ICE" table. Fe(aq)*3 + SCN(aq) = FeSCN2 Initial: **M calculated **M calculated using your Table 2 using your Table 2 volumes volumes Change: - 1x - 1x Equilibrium: M 1x 1x = concentration calculated from Procedure A slope-intercept equation +1x M...
So basically, this excel sheet shows how to get the Equilibrium
Constant of Fe+3 + SCN- ⇆ FeSCN+2
and I'm not sure what I need to change in to formulas to replicate
this solution for Fe+3 + 2
SCN- ⇆ Fe(SCN)2+1
Thanks.
Laboratory Data 0.4084 Slope of cal curve (from your pre-lab -- the mo [Fe(NO3)3] 0.002 [KSCN] 0.002 from the bottles in the lab. from the bottles in the lab. Data analysis part 1 For Fe3+ + SCN- <=>...
For each equilibrium sample, calculate the initial
concentrations (assuming no reaction occurred) of SCN–
and Fe3+ based on the dilution factors used.
Enter the absorbance values for each sample.
For the standard solution, assume that, when equilibrium is
reached, the [FeSCN2+]eq is equal to
[SCN–]ini. Why is this a good
assumption?
For the equilibrium solutions, calculate the
[FeSCN2+]eq (Ceq) using Eq.
4.
Using Eq. 5 and 6, calculate
[Fe3+(aq)]eq and
[SCN–(aq)]eq for each equilibrium
solution.
Calculate values for the equilibrium...
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