-Equilibrium Concentration of [Fe(SCN)2+] – Reacted Concentration of Fe3+ – Reacted Concentration of SCN- –...
-Equilibrium Concentration of [Fe(SCN)2+]
– Reacted Concentration of Fe3+
– Reacted Concentration of SCN-
– Equilibrium Concentration of Fe3+
– Equilibrium Concentration of SCN-
– Equilibrium Constant, Kc
| M(Fe) | M(SCN) |
| 0.00229 | 0.00206 |
| Test Solutions | Concentration | Absorbance |
| 1 | 0 | 0 |
| 2 | 0.0000618 | 0.154 |
| 3 | 0.000103 | 0.22 |
| 4 | 0.000144 | 0.352 |
| 5 | 0.000206 | 0.514 |
From Graph: y = 0.1226x - 0.1198
R² = 0.9844
Homework Answers
Answer:
Given that your lab results:
From the graph of Absorbance (y-axis) versus concentration(x-axis) shown in attached excel image.
Plot Absorbance on y axis and concentration on x-axis.
You can draw trendline also.
The equation is y = 2483.23x = Beer's law constant
The slope is 2483.23
M(Fe3+) = 0.00229, M(SCN-) = 0.00206
The equilibrium reaction is
Fe3+ +. SCN- 
. FeSCN2+
I 0.00229 0.00206 0
C. -x. -x. +x
E. (0.00229-x) (0.00206-x). x
The expression for the equilibrium constant Kc is
Kc = [FeSCN2+]/ [Fe3+][SCN-]
Kc = x/(0.00229-x)(0.00206-x)............(1)
Here x is equilibrium concentration of FeSCN2+ which can be obtained by using Beer's law
A=
lc
Where A is Absorbance
l
= slope of the line = 2483.23
c = conc. of FeSCN2+
or c = A/slope = A/2483.23 .............(2)
since you have not given the value of A Absorptivity at which the equilibrium is reached. But if you have the value of A substitute in equation 2 to get the value of c or x.
x = A/2483.23
Equilibrium concentration of FeSCN2+ = x
Reacted concentration of fe3+ = SCN- = x
Equilibrium concentration of Fe3+ = (0.0029-x)
Equilibrium concentration of SCN- = (0.00206-x)
Substitute the values in equation 1 to get the value of Kc
Add Answer to:
-Equilibrium Concentration of [Fe(SCN)2+]
– Reacted Concentration of Fe3+
– Reacted Concentration of SCN-
–...
1) Consider the following equilibrium: Fe3+(aq) + SCN-(aq) ⇌ FeSCN2+(aq) Initial concentrations: [Fe3+] = 0.590; [SCN-]...
1) Consider the following equilibrium: Fe3+(aq) + SCN-(aq) ⇌ FeSCN2+(aq) Initial concentrations: [Fe3+] = 0.590; [SCN-] = 1.239; [FeSCN2+] = 0 The equilibrium concentration of [FeSCN2+]eq = 0.454 M. What is the numerical value of KC for this equilibrium? KC = __________________ 2) Consider the following equilibrium: Fe3+(aq) + SCN-(aq) ⇌ FeSCN2+(aq) Initial concentrations: [Fe3+] = 0.370; [SCN-] = 0.777; [FeSCN2+] = 0 The equilibrium concentration of [FeSCN2+]eq = 0.285 M. What is the equilibrium concentration of Fe3+? [Fe3+]eq =...
help with calculating the “initial [SCN^—]” M and the Equilibrium [Fe(SCN^2+)] M. i have one. just...
help with calculating the “initial [SCN^—]” M and the Equilibrium
[Fe(SCN^2+)] M.
i
have one. just not sure how to set up the equation to find the
inital [SCN^-] . not sure if im calculating it correctly.
Data Manipulation and Calculations Calibration Solutions Data 1. Calculate the "Initial [SCN']" molarities for the solutions using the dilution equation CiVI=C2V2 2. Use the net ionic equation for the reaction, the ratio of [Fe3 [SCN'] used, and your knowledge of Le Châtelier's Principle...
help with finding the equilibrium of [Fe(SCN)^2+] morality value Equilibrium Solutions Data 1. Use your "Absorbance...
help with finding the equilibrium of [Fe(SCN)^2+] morality value
Equilibrium Solutions Data 1. Use your "Absorbance of Solution" values and the graph you made above to interpolate the "Equilibrium [Fe(SCN)]" molarity values. 2. Calculate both the "Initial [Fe ]" and the "Initial [SCN']" molarity values using then dilution equation CiVi C2V2. 3. Calculate the "Equilibrium [Fe ]" molarity values by subtracting the "Equilibrium [Fe(SCN) " molarity values from the "Initial [Fe'" molarity values. 4. Calculate the "Equilibrium [SCN']" molarity values...
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...
Determine the equilibrium concentration of FeSCN2+ in each solution. (Page below are the initial concentrations of...
Determine the equilibrium concentration of FeSCN2+ in each
solution. (Page below are the initial concentrations of FE3+ and
scn- for each solution )
Secondly, use stoichiometry to determine equilibrium FE3+ and
SCN -. ( concentration used for FE and KSCN are both 0.002M )
the absorbance of each standard in the same test tube used to blank the spectrophoto standards from least to most concentrated, rinsing with a small amount of the next sta tilling the test tube. Record absorbance...
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- <=>...
After the preparation of a solution with solutions containing Fe3+ and SCN- respectively, the final solution...
After the preparation of a solution with solutions containing Fe3+ and SCN- respectively, the final solution has a concentration of Fe(NCS)2+ 5.0x10-4 M, 1.0x10-3 M Fe3+ and 5.0x10-3 M SCN-. Calculate Kc for the following reaction. Fe3+ (aq) + SCN- (aq) ↔ Fe(NCS)2+ (aq) a. 80 b. 100 c. 0.01 d. 0.001
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,...
For this equilibrium : Fe3+ + SCN- <====> [FeSCN]2+ If Z = 4.28103 M -1. A...
For this equilibrium : Fe3+ + SCN- <====> [FeSCN]2+ If Z = 4.28103 M -1. A solution at equilibrium that initially contained 1.59 x10-3[SCN] and 8.46x10-4 M [Fe2+] was found to have an absorbance of 0.402 units. What is the equilibrium constant? please explain
2.) Explain why the concentration of Fe(SCN)2+ is equal to the intial concentration of the SCN- f...
2.) Explain why the concentration of Fe(SCN)2+ is equal to the
intial concentration of the SCN- for each solution in part A?
3.) also!!
thank you!!! :)
Post-Lab Questions: A solution is made by mixing 5.00 ml. of 0.00300 M Fe(NO,)s with 4.00 mL. of 0.00300 M KSCN and 3.00 mL. of 1.0 MHNO,. After equilibrium is established, the concentration Fe(SCN)P was determined to be 2.72 x 10* M. Calculate the value of the equilibrium constant for the reaction. Fe...
help with calculating the “initial [SCN^—]” M and the Equilibrium
[Fe(SCN^2+)] M.
i
have one. just not sure how to set up the equation to find the
inital [SCN^-] . not sure if im calculating it correctly.
Data Manipulation and Calculations Calibration Solutions Data 1. Calculate the "Initial [SCN']" molarities for the solutions using the dilution equation CiVI=C2V2 2. Use the net ionic equation for the reaction, the ratio of [Fe3 [SCN'] used, and your knowledge of Le Châtelier's Principle...
help with finding the equilibrium of [Fe(SCN)^2+] morality value
Equilibrium Solutions Data 1. Use your "Absorbance of Solution" values and the graph you made above to interpolate the "Equilibrium [Fe(SCN)]" molarity values. 2. Calculate both the "Initial [Fe ]" and the "Initial [SCN']" molarity values using then dilution equation CiVi C2V2. 3. Calculate the "Equilibrium [Fe ]" molarity values by subtracting the "Equilibrium [Fe(SCN) " molarity values from the "Initial [Fe'" molarity values. 4. Calculate the "Equilibrium [SCN']" molarity values...
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...
Determine the equilibrium concentration of FeSCN2+ in each
solution. (Page below are the initial concentrations of FE3+ and
scn- for each solution )
Secondly, use stoichiometry to determine equilibrium FE3+ and
SCN -. ( concentration used for FE and KSCN are both 0.002M )
the absorbance of each standard in the same test tube used to blank the spectrophoto standards from least to most concentrated, rinsing with a small amount of the next sta tilling the test tube. Record absorbance...
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- <=>...
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,...
2.) Explain why the concentration of Fe(SCN)2+ is equal to the
intial concentration of the SCN- for each solution in part A?
3.) also!!
thank you!!! :)
Post-Lab Questions: A solution is made by mixing 5.00 ml. of 0.00300 M Fe(NO,)s with 4.00 mL. of 0.00300 M KSCN and 3.00 mL. of 1.0 MHNO,. After equilibrium is established, the concentration Fe(SCN)P was determined to be 2.72 x 10* M. Calculate the value of the equilibrium constant for the reaction. Fe...
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