|
5 |
0.0030 |
0.0015 |
0.0005 |
|
6 |
0.0030 |
0.0057 |
0.0089 |
|
7 |
0.0086 |
0.0057 |
0.0089 |
Show the Calculations of Qc and Kc for Exp. 5-7
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![Wilbur Wright College
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Table 1: Initial & Equilibrium Concentrations
[Fe") (M)
[SCN] (M)
(FESCN) (M)
(Fe"l (M)
5.58 10 M
(SCN J (M)
(FESCN (M)
4.42 *10 M
Exp.
5.58 *10 M
1
0.010
0.010
3.38 *10 M
3.38 * 10 M
1.62 10 M
2
0.0050
0.0050
4.55 10 M
4.55 10 M
2.95 10 M
3
0.0050
0.0050
0.0025
4.99* 10 M
8.49 10 M
6.01 10 M
4
0.0025
0.0060
0.0085
2.9* 20 M
1.41 10 M
5.85 10 M
5
0.0030
0.0015
0.0005
6
0.0030
0.0057
0.0089
5.50* 10 M
8.20* 10 M
6.40* 10 M
9.22* 10 M
6.32* 10 M
8.28* 10 M
0.0086
0.0057
0.0089](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F23029c3f-32e4-4946-9f07-7f9c026ab9f8%2F27470415-11ff-43e5-b37e-a1053fe231b2%2Ftgiby2e_processed.png&w=3840&q=75)
The equilibrium reaction between the Fe3+ ion and SCN- ion to given an iron thiocyanate complex can be written as follows.
Qc is the reaction quotient for the given reaction, which can be defined as the ratio of the molar concentration of product to that of the molar concentration of the reactant at that instant of time raised that are raised to their respective stoichiometric coefficient.
So, for this the reaction quotient Qc can be written as the following expression.
The equilibrium constant Kc is similar to the reaction quotient but differs in terms of the concentrations that are used to find the ratio. In equilibrium constant, the equilibrium concentration of the products and reactants are used. For equilibrium concentration, subscript of 'eq' can be used to differentiate the concentration temp used for the expression of equilibrium constant.
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