USING DATA FROM TUBE #2!!!!!
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USING DATA FROM TUBE #2!!!!!
Table 2.1: Spectrophotometric data used to calculate the equilibrium constant for...
. 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...
values used for table 2 how do you do the Ice tables??? Experiment V. Equilibrium Constant...
values used for table 2
how do you do the Ice tables???
Experiment V. Equilibrium Constant Lab Report ( 50 pts) Calibration Curve 1. Record the absorbance for each of the standard solutions in the table below. Calculate the concentration of FeSCN)" in each of the standard solutions and record the values in the table below. Show a sample calculation (for A2) of your work in the space below the table. Solution Absorbance [Fe(SCN)" A-1 A-2 A-3 0.000 0.390 0.535...
Any help with this ICE table is very much appreciated! Thanks. In test tube 10, the...
Any help with this ICE table is very much appreciated!
Thanks.
In test tube 10, the following volumes of solutions are combined: 3+ 0.0025 M Fe (mL) 0.0025 M SCN (mL) 0.1 M HNO3 (mL) 3.0 3.0 1.0 The measured equilibrium concentration of the product, Fe(SCN), is 0.0000462 mol/L. Calculate the initial and equilibrium concentrations of reactants to complete the ICE table below. R+ SCN Fe(SCN) Fe 0 C -X - X 0.0000462
In test tube 10, the following volumes...
Need help finding equilibrium molarity Table 1: Calibration Curve Data (4 pts. total) Tube Vol. of...
Need help finding equilibrium molarity
Table 1: Calibration Curve Data (4 pts. total) Tube Vol. of 0.200M Volume of Volume of Total Vol. Fe(NO3)3 0.00200M KSCN 0.500M HNO; Smi 10.5 mL 150 mL zob 20.5ml 19.98m2 J 2 5.00mL lll ML 14.05 mL 20.16 mil 5.00 ml 1.5 mL 13.5 mL 20 ml 4 5.00mL 2.0 mL 13.01 mL 20.01 mL 15 500mL I 2.50 ML 12.5 mL 20 ml Table 2: Calibration Curve Calculations and Percent Transmittance Recorded (1/2...
Lab Report: Determination of Kc for a Complex Ion Formation tube 2.00e-3 Fe3+ (mL) 2.00E-3M SCN-...
Lab Report: Determination of Kc for a Complex Ion Formation
tube
2.00e-3 Fe3+ (mL)
2.00E-3M SCN- (mL)
water (mL)
initial conc. Fe3+
initial conc. SCN-
1
5.00
5.00
0
1.00e-3M
1.00E-3M
2
5.00
4.00
1.00
1.00E-3M
8.00E-3M
3
5.00
3.00
2.00
1.00E-3,
6.00E-3M
4
5.00
2.00
3.00
1.00E-3M
4.00E-3M
5
5.00
1.00
4.00
1.00E-3M
2.00E-3M
10ml of 0.200M Fe3+, 2.00ml of 0.00200M SCN-, AND 8.00ml of
water results in an eq. [FeSCN2+] IN Standard
Soln.:2.00E-4M
Could you please explain how...
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...
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...
A student made solution #3 using the experimental method in this lab, and measured an absorbance of 0.559. The starting...
A student made solution #3 using the experimental method in this
lab, and measured an absorbance of 0.559. The starting reagents are
2.00 x 10-3 M Fe(NO3)3 and 2.00 x
10-3 M KSCN.
The amount of absorption is proportional to the concentration
of
FeSCN2+. This relationship – true for many solutions – is called
“Beer’s Law”, and has the simple equation:
A = bc
where “A” is the absorption, “b” is 5174.6 for FeSCN2+ and “c”
is molarity
Make Five...
REPORT SHEET EXPERIMENT Colorimetric 22 Determination of an Equilibrium Constant in Aqueous Solut...
Determination of the equilibrum constant
REPORT SHEET EXPERIMENT Colorimetric 22 Determination of an Equilibrium Constant in Aqueous Solution A. Preparation of the Calibration Curve Concentration of Fe(NO,), in 0.10 M HNO, solution Concentration of NaSCN in 0.10 M HNO, solution Y Y Flask Number 2 Volume of NaSCN, mL Solution Initial [SCN 1.M Equil. [FeNCs". M Percent T Absorbance B. Determination of the Equilibrium Constant Concentration of Fe(NO,) in 0.10 M HNO, solution Concentration of NaSCN in 0.10 M HNO,...
Can someone help me out with #7. The chart above states the chemicals being used. 6....
Can someone help me out with
#7. The chart above states the chemicals being used.
6. Determine the equilibrium concentrations of each of using the table provided below (ICE table). Fill in all blank values concentrations of each of the reactants and products in solution B-5 [Fe3+] (SCN) [Fe(SCN)2+) Initial Concentration Change in Concentration 10.00091 12.1 E-4 T7.0x10-4 Equilibrium Concentration To 00090 1-2.1 E-4 16.9x16-4 +2.12 E-4 201810-9 7. What is the expression for the equilibrium expression for the reaction...
. 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...
values used for table 2
how do you do the Ice tables???
Experiment V. Equilibrium Constant Lab Report ( 50 pts) Calibration Curve 1. Record the absorbance for each of the standard solutions in the table below. Calculate the concentration of FeSCN)" in each of the standard solutions and record the values in the table below. Show a sample calculation (for A2) of your work in the space below the table. Solution Absorbance [Fe(SCN)" A-1 A-2 A-3 0.000 0.390 0.535...
Any help with this ICE table is very much appreciated!
Thanks.
In test tube 10, the following volumes of solutions are combined: 3+ 0.0025 M Fe (mL) 0.0025 M SCN (mL) 0.1 M HNO3 (mL) 3.0 3.0 1.0 The measured equilibrium concentration of the product, Fe(SCN), is 0.0000462 mol/L. Calculate the initial and equilibrium concentrations of reactants to complete the ICE table below. R+ SCN Fe(SCN) Fe 0 C -X - X 0.0000462
In test tube 10, the following volumes...
Need help finding equilibrium molarity
Table 1: Calibration Curve Data (4 pts. total) Tube Vol. of 0.200M Volume of Volume of Total Vol. Fe(NO3)3 0.00200M KSCN 0.500M HNO; Smi 10.5 mL 150 mL zob 20.5ml 19.98m2 J 2 5.00mL lll ML 14.05 mL 20.16 mil 5.00 ml 1.5 mL 13.5 mL 20 ml 4 5.00mL 2.0 mL 13.01 mL 20.01 mL 15 500mL I 2.50 ML 12.5 mL 20 ml Table 2: Calibration Curve Calculations and Percent Transmittance Recorded (1/2...
Lab Report: Determination of Kc for a Complex Ion Formation
tube
2.00e-3 Fe3+ (mL)
2.00E-3M SCN- (mL)
water (mL)
initial conc. Fe3+
initial conc. SCN-
1
5.00
5.00
0
1.00e-3M
1.00E-3M
2
5.00
4.00
1.00
1.00E-3M
8.00E-3M
3
5.00
3.00
2.00
1.00E-3,
6.00E-3M
4
5.00
2.00
3.00
1.00E-3M
4.00E-3M
5
5.00
1.00
4.00
1.00E-3M
2.00E-3M
10ml of 0.200M Fe3+, 2.00ml of 0.00200M SCN-, AND 8.00ml of
water results in an eq. [FeSCN2+] IN Standard
Soln.:2.00E-4M
Could you please explain how...
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...
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...
A student made solution #3 using the experimental method in this
lab, and measured an absorbance of 0.559. The starting reagents are
2.00 x 10-3 M Fe(NO3)3 and 2.00 x
10-3 M KSCN.
The amount of absorption is proportional to the concentration
of
FeSCN2+. This relationship – true for many solutions – is called
“Beer’s Law”, and has the simple equation:
A = bc
where “A” is the absorption, “b” is 5174.6 for FeSCN2+ and “c”
is molarity
Make Five...
Determination of the equilibrum constant
REPORT SHEET EXPERIMENT Colorimetric 22 Determination of an Equilibrium Constant in Aqueous Solution A. Preparation of the Calibration Curve Concentration of Fe(NO,), in 0.10 M HNO, solution Concentration of NaSCN in 0.10 M HNO, solution Y Y Flask Number 2 Volume of NaSCN, mL Solution Initial [SCN 1.M Equil. [FeNCs". M Percent T Absorbance B. Determination of the Equilibrium Constant Concentration of Fe(NO,) in 0.10 M HNO, solution Concentration of NaSCN in 0.10 M HNO,...
Can someone help me out with
#7. The chart above states the chemicals being used.
6. Determine the equilibrium concentrations of each of using the table provided below (ICE table). Fill in all blank values concentrations of each of the reactants and products in solution B-5 [Fe3+] (SCN) [Fe(SCN)2+) Initial Concentration Change in Concentration 10.00091 12.1 E-4 T7.0x10-4 Equilibrium Concentration To 00090 1-2.1 E-4 16.9x16-4 +2.12 E-4 201810-9 7. What is the expression for the equilibrium expression for the reaction...
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