A student made measurements on some electrochemical cells and calculated three quantities: • The standard reaction free energy AG. • The equilibrium constant K at 25.0 °C. • The cell potential under standard conditions º His results are listed below. Unfortunately, the student may have made some mistakes. Examine his results carefully and tick the box next to the incorrect quantity in each row, if any. Note: If there is a mistake in a row, only one of the three quantities listed is wrong. Also, you may assume the number of significant digits in each quantity is correct. Also note: for each cell, the number n of electrons transferred per redox reaction is 1. calculated quantities (Check the box next to any that are wrong.) cell n AGⓇ Fº K - 16 A 1 90. kJ/mol 1.71 x 10 O 0.93 V B 1 108. kJ/mol 8.33 x 10 O - 1.12 V C 1 -69. kJ/mol 8.16 x 10 O 0.71 V O OO 18 -13 O O
A student made measurements on some electrochemical cells and calculated three quantities: • The standard reaction free energy AG. • The equilibrium constant K at 25.0 °C. • The cell potential under standard conditions º His results are listed below. Unfortunately, the student may have made some mistakes. Examine his results carefully and tick the box next to the incorrect quantity in each row, if any. Note: If there is a mistake in a row, only one of the three quantities listed is wrong. Also, you may assume the number of significant digits in each quantity is correct. Also note: for each cell, the number n of electrons transferred per redox reaction is 1. calculated quantities (Check the box next to any that are wrong.) cell n AGⓇ Fº K - 16 A 1 90. kJ/mol 1.71 x 10 O 0.93 V B 1 108. kJ/mol 8.33 x 10 O - 1.12 V C 1 -69. kJ/mol 8.16 x 10 O 0.71 V O OO 18 -13 O O
A student made measurements on some electrochemical cells and calculated three quantities: • The standard reaction free energy AG. • The equilibrium constant K at 25.0 °C. • The cell potential under standard conditions º His results are listed below. Unfortunately, the student may have made some mistakes. Examine his results carefully and tick the box next to the incorrect quantity in each row, if any. Note: If there is a mistake in a row, only one of the three quantities listed is wrong. Also, you may assume the number of significant digits in each quantity is correct. Also note: for each cell, the number n of electrons transferred per redox reaction is 1. calculated quantities (Check the box next to any that are wrong.) cell n AGⓇ Fº K - 16 A 1 90. kJ/mol 1.71 x 10 O 0.93 V B 1 108. kJ/mol 8.33 x 10 O - 1.12 V C 1 -69. kJ/mol 8.16 x 10 O 0.71 V O OO 18 -13 O O
A student made measurements on some electrochemical cells and calculated three quantities:
The standard reaction free energy .
The equilibrium constant at .
The cell potential under standard conditions .
His results are listed below.
Unfortunately, the student may have made some mistakes. Examine his results carefully and tick the box next to the incorrect quantity in each row, if any.
Note: If there is a mistake in a row, only one of the three quantities listed is wrong. Also, you may assume the number of significant digits in each quantity is correct.
Also note: for each cell, the number of electrons transferred per redox reaction is .
Transcribed Image Text:A student made measurements on some electrochemical cells and calculated three quantities:
• The standard reaction free energy AG.
• The equilibrium constant K at 25.0 °C.
• The cell potential under standard conditions
His results are listed below.
Unfortunately, the student may have made some mistakes. Examine his results carefully and tick the box next to the incorrect quantity in each row, if any.
Note: If there is a mistake in a row, only one of the three quantities listed is wrong. Also, you may assume the number of significant digits in each quantity is
correct.
Also note: for each cell, the number n of electrons transferred per redox reaction is 1.
calculated quantities
(Check the box next to any that are wrong.)
cell
AG
K
E
- 16
A
90. kJ/mol O
1.71 x 10 O
0.93 V
18
B
108. kJ/mol
O
8.33 × 10
- 1.12 V
O
4
с
O
-69. kJ/mol
8.16 × 10
0.71 V
O
S
n
1
1
1
13
O
O
O
Definition Definition Chemical reactions involving both oxidation and reduction processes. During a redox reaction, electron transfer takes place in such a way that one chemical compound gets reduced and the other gets oxidized.
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