Cr(s) Cr(NO3)3 Cr³+ (aq) + 3 e Pb²+ (aq) + 2 e NaCl(aq) Pb(s) Pb(NO32 → Cr (s) E° = -0.41 V → Pb (s) E° = -0.12 V The concentration of the solutions in each half-cell is 1.0 mol/L. Placing some Cr(s) in a solution containing Pb²+ ions. Placing some Pb(s) in a solution containing Cr³+ ions. Placing some Cr(s) in a solution containing Cr³+ ions. Placing some Pb(s) in a solution containing Pb3+ ions. Based on the given reduction potentials, which of the following would lead to a reaction?
Cr(s) Cr(NO3)3 Cr³+ (aq) + 3 e Pb²+ (aq) + 2 e NaCl(aq) Pb(s) Pb(NO32 → Cr (s) E° = -0.41 V → Pb (s) E° = -0.12 V The concentration of the solutions in each half-cell is 1.0 mol/L. Placing some Cr(s) in a solution containing Pb²+ ions. Placing some Pb(s) in a solution containing Cr³+ ions. Placing some Cr(s) in a solution containing Cr³+ ions. Placing some Pb(s) in a solution containing Pb3+ ions. Based on the given reduction potentials, which of the following would lead to a reaction?
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter17: Electrochemistry And Its Applications
Section: Chapter Questions
Problem 22QRT
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give explanation for correct and incorrect option plz with detail explanation
Transcribed Image Text:Cr(s)
Cr(NO3)3
A Voltaic Cell
NaCl(aq)
Pb(s)
Pb(NO3)2
Cr³+ (aq) + 3 eCr (s) E° = -0.41 V
Pb²+ (aq) + 2 e¯¯ → Pb (s) E° = -0.12 V
The concentration of the solutions in each half-cell is 1.0
mol/L.
Placing some Cr(s) in a solution containing Pb2+ ions.
Placing some Pb(s) in a solution containing Cr³+ ions.
O Placing some Cr(s) in a solution containing Cr³+ ions.
O Placing some Pb(s) in a solution containing Pb³+ ions.
Based on the given reduction potentials, which of the following would lead to a reaction?
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