Question 2 Consider the following voltaic cell at 298K. Select only the statements that are TRUE. Cu (s) I Cu2+ (1.0 M) II A1³+ (1.0 M) I AI (s) Al³+ (aq) + 3 e →→ Al(s) Ered=-1.66V Cu2+ (aq) + 2e →→ Cu(s) Ered = 0.34V The reducing agent is Al³+ (aq). In the Nernst equation, the value of n = 5. The anode is Cu(s). Al³+ (aq) is reduced. Question 1 Consider the following voltaic cell at 298K. Select only the statements that are TRUE. Mg (s) 1 Mg2+ (1.0 M) II A13+ (1.0 M) I Al (s) Al3+ (aq) + 3 e →→Al(s) Ered = -1.66 V Mg2+ (aq) + 2 e→→Mg(s) Ered = -2.38 V The reaction is spontaneous in the reverse direction. The standard AG° must be positive. The equilibrium constant, K, for this reaction will be greater than 1. The standard Ecell must be positive.
Question 2 Consider the following voltaic cell at 298K. Select only the statements that are TRUE. Cu (s) I Cu2+ (1.0 M) II A1³+ (1.0 M) I AI (s) Al³+ (aq) + 3 e →→ Al(s) Ered=-1.66V Cu2+ (aq) + 2e →→ Cu(s) Ered = 0.34V The reducing agent is Al³+ (aq). In the Nernst equation, the value of n = 5. The anode is Cu(s). Al³+ (aq) is reduced. Question 1 Consider the following voltaic cell at 298K. Select only the statements that are TRUE. Mg (s) 1 Mg2+ (1.0 M) II A13+ (1.0 M) I Al (s) Al3+ (aq) + 3 e →→Al(s) Ered = -1.66 V Mg2+ (aq) + 2 e→→Mg(s) Ered = -2.38 V The reaction is spontaneous in the reverse direction. The standard AG° must be positive. The equilibrium constant, K, for this reaction will be greater than 1. The standard Ecell must be positive.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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please help me with these four questions. i will really appreciated it

Transcribed Image Text:Question 4
Consider the following voltaic cell at 298K. Select ONLY the conditions in which Ecell
O
> E° cell.
Mg (s) | Mg2+ (1.0 M) II A1³+ (1.0 M) I Al (s)
Al³+ (aq) + 3 e →→ Al (s)
Mg2+ (aq) + 2 e → Mg (s)
Ered = -1.66V
Ered = -2.38 V
The mass of Mg (s) is increased to 2g.
The concentration Al³+ (aq) is increased to 2M.
The concentration Mg2+ (aq) is increased to 2M.
The concentration Al³+ (aq) is decreased to 0.5M.
Question 3
At equilibrium, the standard cell potential is equal to zero for all redox reactions.
True
False

Transcribed Image Text:Question 2
Consider the following voltaic cell at 298K. Select only the statements that are TRUE.
Cu (s) I Cu²+ (1.0 M) II A1³+ (1.0 M) I AI (s)
Al³+ (aq) + 3 e →→ Al(s)
E red=-1.66V
Cu2+ (aq) + 2e →→ Cu(s)
Ered = 0.34V
The reducing agent is Al³+ (aq).
In the Nernst equation, the value of n = 5.
The anode is Cu(s).
Al³+ (aq) is reduced.
Question 1
Consider the following voltaic cell at 298K. Select only the statements that are TRUE.
Mg (s) 1 Mg2+ (1.0 M) II A13+ (1.0 M) I Al (s)
Al³+ (aq) + 3 e →→Al(s)
Ered = -1.66 V
Mg2+ (aq) + 2 e →→ Mg(s) Ered= -2.38 V
The reaction is spontaneous in the reverse direction.
The standard AG° must be positive.
The equilibrium constant, K, for this reaction will be greater than 1.
The standard Ecell must be positive.
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