Consider the following reduction potentials. Ag*(aq) + e → Ag(s) E° = + 0.80 V Sn2*(aq) + 2 e -→Sn(s) E° = - 0.14 V Mg2 (aq) + 2 e - → Mg(s) E° = - 2.37 V a.) Calculate the cell potential at standard conditions (E°cell) for a voltaic cell of Mg2+/Mg and Ag*/Ag, in Volts. E° cell = v b.) Calculate Ecel in V at 298 K if [Mg2*] = 0.100 M and [Ag*] = 0.100 M. %3D Ecell = V
Consider the following reduction potentials. Ag*(aq) + e → Ag(s) E° = + 0.80 V Sn2*(aq) + 2 e -→Sn(s) E° = - 0.14 V Mg2 (aq) + 2 e - → Mg(s) E° = - 2.37 V a.) Calculate the cell potential at standard conditions (E°cell) for a voltaic cell of Mg2+/Mg and Ag*/Ag, in Volts. E° cell = v b.) Calculate Ecel in V at 298 K if [Mg2*] = 0.100 M and [Ag*] = 0.100 M. %3D Ecell = V
Chemistry
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ISBN:9781305957404
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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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![Consider the following reduction potentials.
Ag*(aq) + e
→ Ag(s)
E° = + 0.80 V
Sn2*(aq) + 2 e -→Sn(s)
E° = - 0.14 V
Mg2 (aq) + 2 e -
→ Mg(s)
E° = - 2.37 V
a.) Calculate the cell potential at standard conditions (E°cell) for a voltaic cell of Mg2+/Mg and Ag*/Ag, in Volts.
E° cell =
v
b.) Calculate Ecel in V at 298 K if [Mg2*] = 0.100 M and [Ag*] = 0.100 M.
%3D
Ecell =
V](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fcc98fecb-f16a-4e13-92da-567b0deca283%2Ff4a57524-1627-4eef-87fe-61556ceda8f1%2Fhh3jjfh_processed.png&w=3840&q=75)
Transcribed Image Text:Consider the following reduction potentials.
Ag*(aq) + e
→ Ag(s)
E° = + 0.80 V
Sn2*(aq) + 2 e -→Sn(s)
E° = - 0.14 V
Mg2 (aq) + 2 e -
→ Mg(s)
E° = - 2.37 V
a.) Calculate the cell potential at standard conditions (E°cell) for a voltaic cell of Mg2+/Mg and Ag*/Ag, in Volts.
E° cell =
v
b.) Calculate Ecel in V at 298 K if [Mg2*] = 0.100 M and [Ag*] = 0.100 M.
%3D
Ecell =
V
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