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In order to decrease (make it a smaller If the current is set to a constant of 5.37 A for 5.00 min. then 0.901 g of metal would deposit on the cathode.

In order to decrease (make it a smaller If the current is set to a constant of 5.37 A for 5.00 min. then 0.901 g of metal would deposit on the cathode.

Chemistry
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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Just the last one. And use table if needed
D the standard reduction potential for hypock NOTE: logs.20 x 102-129.716 Question 3 Mg Mg(NO₂), The following statement is true: Question 4 Voltage Source salt bridge If the cell pictured above is driven as an electrolytic cell: The electrons would flow from the Mg anode to the Ag If the salt bridge contains KCI, then The standard (assuming 1 M concentrations) cell potential is [Select] Ag AgNO, The potassium ions go towarı v In order to decrease (make it a smaller number) the potential necessary for electrolysis, [Mg2+) should be decreased a Voltmeter +3.16 V If the current is set to a constant of 5.37 A for 5.00 min. then 0.901 g salt bridge of metal would deposit on the cathode.
Transcribed Image Text:D the standard reduction potential for hypock NOTE: logs.20 x 102-129.716 Question 3 Mg Mg(NO₂), The following statement is true: Question 4 Voltage Source salt bridge If the cell pictured above is driven as an electrolytic cell: The electrons would flow from the Mg anode to the Ag If the salt bridge contains KCI, then The standard (assuming 1 M concentrations) cell potential is [Select] Ag AgNO, The potassium ions go towarı v In order to decrease (make it a smaller number) the potential necessary for electrolysis, [Mg2+) should be decreased a Voltmeter +3.16 V If the current is set to a constant of 5.37 A for 5.00 min. then 0.901 g salt bridge of metal would deposit on the cathode.
Standard Reduction Potentials (25 °C) Half-Reaction Co**(aq)+e→ Co (aq) Au³(aq) + 3e →→ Au(s) ->> Cl₂(g) +2e- 2Cl (aq) Pd2 (aq) + 2e → Pd(s) -> Ag (aq) + e → Ag(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) 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
Transcribed Image Text:Standard Reduction Potentials (25 °C) Half-Reaction Co**(aq)+e→ Co (aq) Au³(aq) + 3e →→ Au(s) ->> Cl₂(g) +2e- 2Cl (aq) Pd2 (aq) + 2e → Pd(s) -> Ag (aq) + e → Ag(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) 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
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