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in part 1 gires us absorbance values for each sample , changes in concentration...
After completing Part A of this experiment, a student determines the slope of their calibration graph...
After completing Part A of this experiment, a student determines
the slope of their calibration graph of absorbance versus [FeSCN2]
to be 5140 M1. In Part B, a student combines 2.00 mL of a 0.00200 M
solution of KSCN with 5.00 mL of 0.00200 M solution of Fe(NO,), and
3.00 mL of water. The following equilibrium is established. Fe (aq)
+ SCN (aq) FeSCN (aq) The absorbance of the equilibrium solution is
measured as 0.246. What is the equilibrium constant...
누 4. After completing Part A of this experiment, a student determines the slope of their...
누 4. After completing Part A of this experiment, a student determines the slope of their calibration graph of absorbance versus [FeSCN"] to be 5140 M1. In Part B, a student combines 2.00 mL of a 0.00200 M solution of KSCN with 5.00 mL of 0.00200 M solution of Fe(NO,), and 3.00 mL of water. The following equilibrium is established. Fe (aq)+ SCN (aq) - FeSCN (aq) The absorbance of the equilibrium solution is measured as 0.246. What is the...
DETERMINATION OF AN EQUILIBRIUM CONSTANT FOR A CHEMICAL REACTION Name TA Name (posted on A2L under...
DETERMINATION OF AN EQUILIBRIUM CONSTANT FOR A CHEMICAL REACTION Name TA Name (posted on A2L under "Grades") Lab Bench (posted on A2L under "Grades") Lab Room (posted on A2L under "Grades") Date Complete the following pre-lab questions before coming to lab. Your TA will collect this page at the start of your lab period. In your laboratory notebook, prepare the axes of your calibration graph for Part A. The graph should take up an entire page with a y-axis range...
What's the concentration of [FeSCN2+] using limiting reactant theory and equation? For each test tube solution...
What's the concentration of [FeSCN2+] using limiting
reactant theory and equation?
For each test tube solution enter the initial concentration of Fe+ and SCNthe equilibrium concentration of FeSCN2: into the ICE table given. Complete entries for the rest of the table and calculate the K value for each of the tables. The values of K should be confined to a narrow range to reflect constancy. Comment on the quality of your work in this regard and calculate the average K....
4.81 mL of 0.00200 M Fe(NO3)3, 2.85 mL of 0.00200 M KSCN and 2.34 mL of...
4.81 mL of 0.00200 M Fe(NO3)3, 2.85 mL of 0.00200 M KSCN and 2.34 mL of distilled water were mixed. The resulting solution was allowed to attain equilibrium at 24 oC. The absorbance of the equilibrium solution was recorded, and the [FeSCN2+] was determined graphically to be 7.58 x 10-5 M. Part A: Calculate the number of moles of Fe3+ initially added to the solution. Part B: Calculate the number of moles of FeSCN2+ formed in the solution at equilibrium....
Question 13 of 13> Attempt 1 A standard solution of FeSCN2+ is prepared by combining 9.0...
Question 13 of 13> Attempt 1 A standard solution of FeSCN2+ is prepared by combining 9.0 ml of 0.20 M Fe(NO) with I.0 mL of 0.0020 M KSCN. The standard solution had an absorbance of 0.540. Fe* (ag)+SCN (ag)FeSCN*(a) A trial solution was made in a similar manner, but with a more dilute Fe(NO,), reagent. The initial SCN" concentration. immediately after mixing, was 0.00060 M. This trial solution had absorbance of 0.250. What is the equilibrium concentration of SCN in...
5. A student does an experiment to determine the equili but at a higher temperature. ermine...
5. A student does an experiment to determine the equili but at a higher temperature. ermine the equilibrium constant for the same reaction that you will study, Fe** (aq) + SCN (aq) FeSCN2+ (aq) The student prepares solution 1, by mixing 5. s Solution, by mixing 5.00 ml of 0.002 M Fe(NO2)2 solution with 5.00 mL of .00011M KSCN solution, heats the mixture, and finds that the equilibrium concentration of F and finds that the equilibrium concentration of FeSCN2+ in...
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...
Doing a Chem Review, these are just study scenarios that I need to have a good...
Doing a Chem Review, these are just study scenarios that I need
to have a good understanding of
6. To determine the concentration of SCN in our saliva, we reacted the SCN in the saliva with Fe' according to the following reaction: We measured the absorbance of the FeSCN and used the absorbance value of the FesCN2 to obtain the concentration of the FesCN2*. This was achieved by measuring the absorbance values of standard FeSCN2+ solutions and constructing a calibration...
. 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...
After completing Part A of this experiment, a student determines
the slope of their calibration graph of absorbance versus [FeSCN2]
to be 5140 M1. In Part B, a student combines 2.00 mL of a 0.00200 M
solution of KSCN with 5.00 mL of 0.00200 M solution of Fe(NO,), and
3.00 mL of water. The following equilibrium is established. Fe (aq)
+ SCN (aq) FeSCN (aq) The absorbance of the equilibrium solution is
measured as 0.246. What is the equilibrium constant...
누 4. After completing Part A of this experiment, a student determines the slope of their calibration graph of absorbance versus [FeSCN"] to be 5140 M1. In Part B, a student combines 2.00 mL of a 0.00200 M solution of KSCN with 5.00 mL of 0.00200 M solution of Fe(NO,), and 3.00 mL of water. The following equilibrium is established. Fe (aq)+ SCN (aq) - FeSCN (aq) The absorbance of the equilibrium solution is measured as 0.246. What is the...
DETERMINATION OF AN EQUILIBRIUM CONSTANT FOR A CHEMICAL REACTION Name TA Name (posted on A2L under "Grades") Lab Bench (posted on A2L under "Grades") Lab Room (posted on A2L under "Grades") Date Complete the following pre-lab questions before coming to lab. Your TA will collect this page at the start of your lab period. In your laboratory notebook, prepare the axes of your calibration graph for Part A. The graph should take up an entire page with a y-axis range...
What's the concentration of [FeSCN2+] using limiting
reactant theory and equation?
For each test tube solution enter the initial concentration of Fe+ and SCNthe equilibrium concentration of FeSCN2: into the ICE table given. Complete entries for the rest of the table and calculate the K value for each of the tables. The values of K should be confined to a narrow range to reflect constancy. Comment on the quality of your work in this regard and calculate the average K....
Question 13 of 13> Attempt 1 A standard solution of FeSCN2+ is prepared by combining 9.0 ml of 0.20 M Fe(NO) with I.0 mL of 0.0020 M KSCN. The standard solution had an absorbance of 0.540. Fe* (ag)+SCN (ag)FeSCN*(a) A trial solution was made in a similar manner, but with a more dilute Fe(NO,), reagent. The initial SCN" concentration. immediately after mixing, was 0.00060 M. This trial solution had absorbance of 0.250. What is the equilibrium concentration of SCN in...
5. A student does an experiment to determine the equili but at a higher temperature. ermine the equilibrium constant for the same reaction that you will study, Fe** (aq) + SCN (aq) FeSCN2+ (aq) The student prepares solution 1, by mixing 5. s Solution, by mixing 5.00 ml of 0.002 M Fe(NO2)2 solution with 5.00 mL of .00011M KSCN solution, heats the mixture, and finds that the equilibrium concentration of F and finds that the equilibrium concentration of FeSCN2+ in...
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...
Doing a Chem Review, these are just study scenarios that I need
to have a good understanding of
6. To determine the concentration of SCN in our saliva, we reacted the SCN in the saliva with Fe' according to the following reaction: We measured the absorbance of the FeSCN and used the absorbance value of the FesCN2 to obtain the concentration of the FesCN2*. This was achieved by measuring the absorbance values of standard FeSCN2+ solutions and constructing a calibration...
. 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...
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