When an aqueous solution of copper sulphate is electrolyzed, copper is deposited at the cathode (clue: get the reduction half equation from the table of standard reduction potentials). If a constant current was passed for 5 hours and 404 mg of Cu was deposited, calculate the current passed through CuSO₄. (Atomic mass of Cu is 63.55 amu).What is the number of faradays (F) of electricity required to liberate 134.4 L of hydrogen gas (H₂) from a solution containing H⁺ ions? (22.4 L of H₂ is equal to 1 mol of H₂) 2 H+ + 2 e- > H2 (g)References/Given Values: Faraday’s Constant: F = 96,485 C/mol eˉ; Atomic Mass of H = 1 amu Standard reduction potentials for some common metals - for aqueoussolutions of ions at 1.0 M concentration at 25 °C and H2 gas at 1.0 atmpressure and 25°CReduction Half-Cell EquationLi+ + 1e-K+ + 1e-Ba²+ + 2eCa²+ + 2e-Na+ + 1e-Mg²+ + 2e-Al3+ + ЗеZn²+ + 2e-Cr3+ + ЗеFe²+ + 2e-Cd²+ + 2e-Ni2+ + 2e-Sn²+ + 2e-Pb²+ + 2e-2 H+ + 2eCu²+ + 2e-↑ | I | I | I | I | I | I | 1←LiK1BaCaNaMgAIZnCrFeCdNisnPbH2Cu2 HgAgHg₂²+ + 2e →→Ag+ + 1e-Hg2+ + 2e-Au³+ + 3e- → AuHgE° (v)-3.04-2.92-2.91-2.87-2.71-2.36-1.66-0.76-0.74-0.44-0.40-0.25-0.14-0.130.00+0.34+0.79+0.80+0.85+1.42

Half-cell reaction for deposition of Cu is Cu2+ + 2e- --> Cu Calculate the moles of Cu Mass of…

Answered: When an aqueous solution of copper…

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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

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When an aqueous solution of copper sulphate is electrolyzed, copper is deposited at the cathode (clue: get the reduction half equation from the table of standard reduction potentials). If a constant current was passed for 5 hours and 404 mg of Cu was deposited, calculate the current passed through CuSO₄. (Atomic mass of Cu is 63.55 amu).

What is the number of faradays (F) of electricity required to liberate 134.4 L of hydrogen gas (H₂) from a solution containing H⁺ ions? (22.4 L of H₂ is equal to 1 mol of H₂) 2 H⁺+ 2 e^- > H₂ (g)

References/Given Values: Faraday’s Constant: F = 96,485 C/mol eˉ;

Atomic Mass of H = 1 amu

Standard reduction potentials for some common metals - for aqueous
solutions of ions at 1.0 M concentration at 25 °C and H2 gas at 1.0 atm
pressure and 25°C
Reduction Half-Cell Equation
Li+ + 1e-
K+ + 1e-
Ba²+ + 2e
Ca²+ + 2e-
Na+ + 1e-
Mg²+ + 2e-
Al3+ + Зе
Zn²+ + 2e-
Cr3+ + Зе
Fe²+ + 2e-
Cd²+ + 2e-
Ni2+ + 2e-
Sn²+ + 2e-
Pb²+ + 2e-
2 H+ + 2e
Cu²+ + 2e-
↑ | I | I | I | I | I | I | 1
←
Li
K
1
Ba
Ca
Na
Mg
AI
Zn
Cr
Fe
Cd
Ni
sn
Pb
H2
Cu
2 Hg
Ag
Hg₂²+ + 2e →→
Ag+ + 1e-
Hg2+ + 2e-
Au³+ + 3e- → Au
Hg
E° (v)
-3.04
-2.92
-2.91
-2.87
-2.71
-2.36
-1.66
-0.76
-0.74
-0.44
-0.40
-0.25
-0.14
-0.13
0.00
+0.34
+0.79
+0.80
+0.85
+1.42

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