Mg Mg(NO₂) Voltmeter The electrons would flow [Select] V salt bridge Ag AgNO, Given the electrochemical cell in the picture: In the balanced cell reaction, the number of electrons transferred i The standard (assuming 1 M concentrations) cell potential is [Select [Select] 1 2 4 3
Mg Mg(NO₂) Voltmeter The electrons would flow [Select] V salt bridge Ag AgNO, Given the electrochemical cell in the picture: In the balanced cell reaction, the number of electrons transferred i The standard (assuming 1 M concentrations) cell potential is [Select [Select] 1 2 4 3
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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Question
![0
Standard Reduction Potentials (25 °C)
Half-Reaction
Co(aq)+e → + Co2*(aq)
Au³+ (aq) + 3e →→ Au(s)
Cl₂(g) +2e → 2CH(aq)
Pd2 (aq) + 2e → Pd(s)
Ag (aq) +eAg(s)
12(s) + 2e → 21 (aq)
Cu²+ (aq) + 2e ->> Cu(s)
Cu²+ (aq) + e→→ Cu*(aq)
2H*(aq) + 2e ->>
H₂(g)
Pb²+ (aq) + 2e-
->> Pb(s)
Ni²+ (aq) + 2e
Ni(s)
Cd²+ (aq) +2e
->> Cd(s)
Fe2+ (aq) + 2e → Fe(s)
Cr³+ (aq) + 3e → Cr(s)
->
Zn²+ (aq) + 2e
Zn(s)
2+
Mn²+ (aq) + 2e ->>> Mn(s)
Ti²+ (aq) + 2e →→ Ti(s)
Al³+ (aq) + 3e → Al(s)
Mg2+ (aq) + 2e
->>
-
->
Mg(s)
E° (V)
+1.92
+1.498
+1.36
+0.915
+0.80
+0.54
+0.34
+0.153
0.00
-0.13
-0.232
-0.40
-0.44
-0.740
-0.76
-1.185
-1.630
-1.67
-2.356](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff3a38996-6782-40c2-af9f-f624a7021da3%2Ff9df07f3-4272-4405-80d5-8df54fe824ae%2F2hgu2nm_processed.jpeg&w=3840&q=75)
Transcribed Image Text:0
Standard Reduction Potentials (25 °C)
Half-Reaction
Co(aq)+e → + Co2*(aq)
Au³+ (aq) + 3e →→ Au(s)
Cl₂(g) +2e → 2CH(aq)
Pd2 (aq) + 2e → Pd(s)
Ag (aq) +eAg(s)
12(s) + 2e → 21 (aq)
Cu²+ (aq) + 2e ->> Cu(s)
Cu²+ (aq) + e→→ Cu*(aq)
2H*(aq) + 2e ->>
H₂(g)
Pb²+ (aq) + 2e-
->> Pb(s)
Ni²+ (aq) + 2e
Ni(s)
Cd²+ (aq) +2e
->> Cd(s)
Fe2+ (aq) + 2e → Fe(s)
Cr³+ (aq) + 3e → Cr(s)
->
Zn²+ (aq) + 2e
Zn(s)
2+
Mn²+ (aq) + 2e ->>> Mn(s)
Ti²+ (aq) + 2e →→ Ti(s)
Al³+ (aq) + 3e → Al(s)
Mg2+ (aq) + 2e
->>
-
->
Mg(s)
E° (V)
+1.92
+1.498
+1.36
+0.915
+0.80
+0.54
+0.34
+0.153
0.00
-0.13
-0.232
-0.40
-0.44
-0.740
-0.76
-1.185
-1.630
-1.67
-2.356
![D
Question 1
The electrons would flow [Select]
Voltmeter
salt bridge
Mg
M
Mg(NO₂),
Given the electrochemical cell in the picture:
In the balanced cell reaction, the number of electrons transferred ✔ [ Select)
1
The [Select]
Ag
AgNO,
The standard (assuming 1 M concentrations) cell potential is [Select
Question 2
2
The change in standard Gibbs' Energy, AG, for the overall reaction would be [Select]
3
If the voltmeter was replaced with a resistor (that allows current to flow) and the current is measured to be a constant 1.250 A, it would take [Select]
If the concentrations were changed to [Mg2+] = 5.00 M and [Ag*] = 0.0100 M, the cell potential would then be
[Select]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff3a38996-6782-40c2-af9f-f624a7021da3%2Ff9df07f3-4272-4405-80d5-8df54fe824ae%2Ff1b68e_processed.jpeg&w=3840&q=75)
Transcribed Image Text:D
Question 1
The electrons would flow [Select]
Voltmeter
salt bridge
Mg
M
Mg(NO₂),
Given the electrochemical cell in the picture:
In the balanced cell reaction, the number of electrons transferred ✔ [ Select)
1
The [Select]
Ag
AgNO,
The standard (assuming 1 M concentrations) cell potential is [Select
Question 2
2
The change in standard Gibbs' Energy, AG, for the overall reaction would be [Select]
3
If the voltmeter was replaced with a resistor (that allows current to flow) and the current is measured to be a constant 1.250 A, it would take [Select]
If the concentrations were changed to [Mg2+] = 5.00 M and [Ag*] = 0.0100 M, the cell potential would then be
[Select]
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