Homework Answers
![2000n 0.0250 7 Tablets (using Table 4) Test tube # B c D E [Fes CN²+] ez 9.370578 x 10-5 -5 m 6.6299 8.29 3x10 x105m S ~8.29x](http://img.homeworklib.com/questions/735ed690-eaec-11ea-984b-47e637028634.png?x-oss-process=image/resize,w_560)
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. Determination of an equilibrium constant Use the calculated absorbance values from Table 4 in Part...
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...
please help me with this bullet point!! U E F G H 1 K L M...
please help me with this bullet point!!
U E F G H 1 K L M 0.00025 y = 0.0003x + 2E-06 0.0002 0.00015 [Fe(SCN^2+) 0.0001 0.00005 *********......... 0 0.000 0.100 0.200 0.600 0.700 0.800 0.300 0.400 0.500 Absorbance Determination of an equilibrium constant Part II: Data and Calculations Table 4: Trial А % Transmittance 71.1 B 61.6 с 53.2 Absorbance 0.148 0.210 0.274 0.333 0.395 D 46.4 E 40.3 Calculate the absorbance and complete Table 4 above. A=2.000-log(71.4) A...
USING DATA FROM TUBE #2!!!!! Table 2.1: Spectrophotometric data used to calculate the equilibrium constant for...
USING DATA FROM TUBE #2!!!!!
Table 2.1: Spectrophotometric data used to calculate the equilibrium constant for Fe(SCN)* Initial Conc. of the Reactants in the test tubes (M) Equilibrium Concentrationin Reaction Constants Concentrat the test tubes (M) (see next page) Fe Source Tube # 1 Auconn Fel SCN Fe SCN Fe(SCN)K рк. C o1oA NA Stock 7.612 Solution A 2 3u QUESTIONS 1) Complete Table 2.1. With the results of tube #2, show the calculations for the determination of the equilibrium...
To calculate the equilibrium concentration, you can use the ICE table approach. ICE stands for initial"...
To calculate the equilibrium concentration, you can use the ICE table approach. ICE stands for initial" (1). "change" (C) and equilibrium" (E). The use of ICE tables may have been covered in your lecture. If not, please review the background knowledge posted on iCollege. Answer the following questions. 1. In an experiment of determining the equilibrium constant of ferric thiocyanate, a student group got the absorbance vs [FeSCN*) as shown below. Absorbance vs (FeSCN2+] y=4312x+0.0075 R2=0.9935 Absorbance 0 0000 00001...
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...
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...
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...
As you will do in lab, a student prepared the following 2 mixtures and recorded their absorbances...
As you will do in lab, a student prepared the following 2 mixtures and recorded their absorbances in a cuvette with a 1.00 cm path length Table 1.Absorbance of iron (Il) thiocyanate Volume, ml Fe3- 10.0 0.020 M2.64 x 10M Absorbance SCN 10.0 10.0 Mix #1 0.20 M Fel 10.01 0.769 0.495 1. Write the balanced equilibrium reaction of Fe(aq) with SCN (aq) to form [FeSCNJ (aq). 2. Write the equilibrium formation constant expression for the reaction (Kyexpression) Determination of...
Data Test Tube el=A_ 0.370 C X154 = 3700 10158184 (10.047 3100 5 1.2703 YID Absorbance...
Data Test Tube el=A_ 0.370 C X154 = 3700 10158184 (10.047 3100 5 1.2703 YID Absorbance [FeSCN ] at equilibrium 0.047 A 1o 3x105 0.198 A 5.358los Oo 303 A 8.19x105 0.425 A 0. 560 A 1.51x10-9 Test Tube 6(standard, 1 x 106m). Absorbance O: 3:04. 1-3X10 Xool Results Initial Moles Moles at Equilibrium Fe* SCN Fe(SCN)2 Fe IX 105 2x106 11.3x107 1x100 4x106 15.358 lot 1x 105 68106 8.19x107 1x10.5 8X 106 1.15X106 5 | 1x10.5 1x10-5 1.51x106 0.196...
Section Name Experiment 23 Advance Study Assignment: Determination of the Equilibrium Constant for a Chemical Reaction...
Section Name Experiment 23 Advance Study Assignment: Determination of the Equilibrium Constant for a Chemical Reaction 1. A student mixes 5.00 mL 2.00 X 10M Fe(NO), with 5.00 ml 2.00 x 10-M KSCN. She finds that in the equilibrium mixture the concentration of FeSCN is 1.40 x 10M. Find K for the reaction Fe(aq) + SCN (aq) FeSCN2(aq). Step 1 Find the number of moles Fe and SCN initially present. (Use Eq. 3.) (5.00 x103 LX (300X163) = (x 103...
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...
please help me with this bullet point!!
U E F G H 1 K L M 0.00025 y = 0.0003x + 2E-06 0.0002 0.00015 [Fe(SCN^2+) 0.0001 0.00005 *********......... 0 0.000 0.100 0.200 0.600 0.700 0.800 0.300 0.400 0.500 Absorbance Determination of an equilibrium constant Part II: Data and Calculations Table 4: Trial А % Transmittance 71.1 B 61.6 с 53.2 Absorbance 0.148 0.210 0.274 0.333 0.395 D 46.4 E 40.3 Calculate the absorbance and complete Table 4 above. A=2.000-log(71.4) A...
USING DATA FROM TUBE #2!!!!!
Table 2.1: Spectrophotometric data used to calculate the equilibrium constant for Fe(SCN)* Initial Conc. of the Reactants in the test tubes (M) Equilibrium Concentrationin Reaction Constants Concentrat the test tubes (M) (see next page) Fe Source Tube # 1 Auconn Fel SCN Fe SCN Fe(SCN)K рк. C o1oA NA Stock 7.612 Solution A 2 3u QUESTIONS 1) Complete Table 2.1. With the results of tube #2, show the calculations for the determination of the equilibrium...
To calculate the equilibrium concentration, you can use the ICE table approach. ICE stands for initial" (1). "change" (C) and equilibrium" (E). The use of ICE tables may have been covered in your lecture. If not, please review the background knowledge posted on iCollege. Answer the following questions. 1. In an experiment of determining the equilibrium constant of ferric thiocyanate, a student group got the absorbance vs [FeSCN*) as shown below. Absorbance vs (FeSCN2+] y=4312x+0.0075 R2=0.9935 Absorbance 0 0000 00001...
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...
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...
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...
As you will do in lab, a student prepared the following 2 mixtures and recorded their absorbances in a cuvette with a 1.00 cm path length Table 1.Absorbance of iron (Il) thiocyanate Volume, ml Fe3- 10.0 0.020 M2.64 x 10M Absorbance SCN 10.0 10.0 Mix #1 0.20 M Fel 10.01 0.769 0.495 1. Write the balanced equilibrium reaction of Fe(aq) with SCN (aq) to form [FeSCNJ (aq). 2. Write the equilibrium formation constant expression for the reaction (Kyexpression) Determination of...
Data Test Tube el=A_ 0.370 C X154 = 3700 10158184 (10.047 3100 5 1.2703 YID Absorbance [FeSCN ] at equilibrium 0.047 A 1o 3x105 0.198 A 5.358los Oo 303 A 8.19x105 0.425 A 0. 560 A 1.51x10-9 Test Tube 6(standard, 1 x 106m). Absorbance O: 3:04. 1-3X10 Xool Results Initial Moles Moles at Equilibrium Fe* SCN Fe(SCN)2 Fe IX 105 2x106 11.3x107 1x100 4x106 15.358 lot 1x 105 68106 8.19x107 1x10.5 8X 106 1.15X106 5 | 1x10.5 1x10-5 1.51x106 0.196...
Section Name Experiment 23 Advance Study Assignment: Determination of the Equilibrium Constant for a Chemical Reaction 1. A student mixes 5.00 mL 2.00 X 10M Fe(NO), with 5.00 ml 2.00 x 10-M KSCN. She finds that in the equilibrium mixture the concentration of FeSCN is 1.40 x 10M. Find K for the reaction Fe(aq) + SCN (aq) FeSCN2(aq). Step 1 Find the number of moles Fe and SCN initially present. (Use Eq. 3.) (5.00 x103 LX (300X163) = (x 103...
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