Assuming the reaction stoichiometry is correct, Ka should be the same (within the bounds of experimental error). But if the assumed reaction stoichiometry is incorrect, the equilibrium constant will vary greatly. K = Fe(SCN) Fe(SCN) [Fe³[SCN] If this was the actual reaction, the concentration of Fe(SCN), determined from the absorbance measurements would have been half of the concentration of FeSCN as shown in the table below. Use these new equilibrium concentrations to calculate the equilibrium constant for the reaction above. Consider the following reaction: 3+ Fe³+ + 2 SCN
Assuming the reaction stoichiometry is correct, Ka should be the same (within the bounds of experimental error). But if the assumed reaction stoichiometry is incorrect, the equilibrium constant will vary greatly. K = Fe(SCN) Fe(SCN) [Fe³[SCN] If this was the actual reaction, the concentration of Fe(SCN), determined from the absorbance measurements would have been half of the concentration of FeSCN as shown in the table below. Use these new equilibrium concentrations to calculate the equilibrium constant for the reaction above. Consider the following reaction: 3+ Fe³+ + 2 SCN
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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Lock And Key Model
The lock-and-key model is used to describe the catalytic enzyme activity, based on the interaction between enzyme and substrate. This model considers the lock as an enzyme and the key as a substrate to explain this model. The concept of how a unique distinct key only can have the access to open a particular lock resembles how the specific substrate can only fit into the particular active site of the enzyme. This is significant in understanding the intermolecular interaction between proteins and plays a vital role in drug interaction.
Question
Can you help me with Part 3. U don’t have to answer the table at the bottom
Transcribed Image Text:Sample
Number
1
2
3
4
5
Initial moles
Equilibrium moles
Fe³+
SCN
00 18.24
01
-01 4×40.50
.01 6×103 2.19
.01 8x10 3.89
0101 6.64
Fe³+
Equilibrium
Concentration (in M)
SCN FeSCN²
SCN FeSCN²
18.298 18.3 +1.83
0.506.51 .05
2.194 2.2 2,22
3.892 39
·6.04 6.05.0
Fe³+
initial moles
moles od Fest.002.5=.01 moles
Concentration of fe ScN²³:
y=0.374 +0.174
.85-0.37x +0.174
,83 = x
4
39
Calculations
Fe ² (ag) + SCN (ay)<> Fe(SCN) an)
Fe³: My₁ = my SCN²: M₁ V₁ -M₂ √₂
Fest
(2) (10) - (20) M₂
(002) (5) = M₂
20
0.1M - M₂
5+105-1₂
1.83.83
.055
051 201
22 22 045
39
39 0.26
05
1.60
Kea
605
0-17
Concentration
J
![Name
Part III: What if?
Assuming the reaction stoichiometry is correct, Ke should be the same (within the bounds of experimental error). But if the assumed reaction
stoichiometry is incorrect, the equilibrium constant will vary greatly.
Consider the following reaction:
Fe(SCN)
K =
Fe(SCN)
[Fe³][SCN]
If this was the actual reaction, the concentration of Fe(SCN), determined from the absorbance measurements would have been half of the
concentration of FeSCN* as shown in the table below. Use these new equilibrium concentrations to calculate the equilibrium constant for the
reaction above.
Sample
Number
1
3
5
Fe
Initial mols
SCN
Fe +2 SCN=
Fe**
Equilibrium mols
SCN
Fe(SCN)
Equilibrium Concentration
Fe
(M)
SCN
Fe(SCN)
Calculated
Kea
Based on the results above, which of the two possible reactions represents the correct equilibrium? How do you know? Explain.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd3a80bdb-dbe3-4058-9ea9-0990b19198fe%2F3d35daf3-8210-4ea5-b5ce-c87f6a9aa2f4%2F6aavnk_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Name
Part III: What if?
Assuming the reaction stoichiometry is correct, Ke should be the same (within the bounds of experimental error). But if the assumed reaction
stoichiometry is incorrect, the equilibrium constant will vary greatly.
Consider the following reaction:
Fe(SCN)
K =
Fe(SCN)
[Fe³][SCN]
If this was the actual reaction, the concentration of Fe(SCN), determined from the absorbance measurements would have been half of the
concentration of FeSCN* as shown in the table below. Use these new equilibrium concentrations to calculate the equilibrium constant for the
reaction above.
Sample
Number
1
3
5
Fe
Initial mols
SCN
Fe +2 SCN=
Fe**
Equilibrium mols
SCN
Fe(SCN)
Equilibrium Concentration
Fe
(M)
SCN
Fe(SCN)
Calculated
Kea
Based on the results above, which of the two possible reactions represents the correct equilibrium? How do you know? Explain.
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