A current of 3.21 A is passed through a Pb(NO3)2 solution. How long, in hours, would this current have to be applied to plate out 7.50 g of lead?

A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2VO₂ (aq) + 4H* (aq) + Fe (s) → 2VO²+ (aq) + 2H₂O (1)+Fe²+ (aq) Suppose the cell is prepared with 3.37 M VO and 3.31 MH* in one half-cell and 6.13 M VO²+ and 2.52 M Fe²+ in the other. 2+ 2+ Calculate the cell voltage under these conditions. Round your answer to 3 significant digits.

what mass, in g, of copper will be deposited from a solution of Cu^2+ by a current of 2.43 A in 7.52 h?

A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 2+ Cu²+ (aq) + Zn (s) → Cu (s) + Zn²+ (aq) 2+ Suppose the cell is prepared with 5.43 M Cu²+ in one half-cell and 3.33 M Zn in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. 0 x10 X μ 00 Ś

A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 2103 (aq) +12H* (aq) + 5Co (s) → 1₂ (s) + 6H₂O (1) +5Co²+ (aq) 2+ Suppose the cell is prepared with 5.23 M IO3 and 2.31 M H in one half-cell and 6.84 M Co in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits.

What mass of Molybdenum (Mo) could be deposited by electrolysis of an aqueous solution of Mo2(SO4)3 for 125 min using a constant current of 12.0 A?

A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 3+ 2+ 2 Cr³+ (aq) + 3Ca (s) → 2Cr (s) + 3 Ca²+ (aq) 3+ 2+ Suppose the cell is prepared with 2.68 M Cr in one half-cell and 7.85 M Ca in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. x10 ロ・ロ × μ 0|0 Ś

Calculate the voltage of the redox reaction of element X (group 2) if the Gibb’s free energy evolved during the redox reaction is + 150 kJ/mol. (Faraday constant, 9.649 x 104C)

A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2Cr³+ (aq) + 3 Ca(s) → 2Cr(s) + 3Ca²+ (aq) Suppose the cell is prepared with 6.35 M Cr3+ in one half-cell and 0.492 M Ca²+ in the other half. Calculate the cell voltage under these conditions. Ered red= -0.744 V Cr³+ (aq) + 3e → Cr(s) Ca²+ (aq) + 2e → Ca(s) Ered= -2.868 V The standard cell potential (E°) for this galvanic cell is [Select] There are [Select] galvanic cell. Under these conditions, the reaction quotient is [Select] volatage is [Select] moles of electrons transferred during to operate this VV. In order to increase the cell voltage for this cell, [Select] V. ✓and the cell >