What mass of Mg is produced (in grams) when a constant current of 0.752 A is passed through an electrolytic cell containing molen MgCl2 for 14.2 hours? Atomic weight for magnesium is 24.31 g/mol.  Mg2+(aq) + 2e- --> Mg(s) is 4.84 the answer? pls prove

(a) In the electrolysis of aqueous Na2C204, how many liters of H2(g) (at STP) are generated by a current of 82.6 A for a period of 54.0 min? The unbalanced chemical reaction representing this electrolysis is shown below. Na2C204(aq) + H20(1) → CO2(g) + H2(g) + NaOH(aq) liters of H2(g) is generated by this electrolysis. (b) How many moles of NaOH(aq) are formed in the solution in this process? moles of NaOH(aq) are formed.

4. A cell uses the following reaction: a. Zn (s) + 2 H* (aq) → Zn²* (aq) + H2 (g) (a) Determine the emf of the cell under standard conditions. (b) When PH,=1.0 atm and [Zn²*] = 1.0 M, the cell potential is 0.560 V. Determine the concentration of H* in the cathode compartment. Zn2“(aq) + 2e¯ → Zn(s) -0.763 2H*(aq) + 2e¯ –→ H2(g) b.

How many grams of X (MW = 44.20 g/mol)(in g) will be deposited on a cathode in 1.91 h by a current of 3.8 A?   X4+ + 4e- → X(s)

A galvanic cell is constructed in which the overall reac- tion is Pb(s) + 2 H;O* (aq) → Pb²+ (aq) + H2 (g) + 2 H20(e) (a) Calculate AE° for this cell. (b) Chloride ions are added until PbCl, precipitates at the anode and [CI-] reaches 0.15 M. The cell potential is then measured to be 0.22 V at pH = 0 and PH, 1.0 atm. Calculate [Pb2+] under these conditions. (c) Calculate the solubility product constant Kp of PbCl2.

A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 3Cu* (aq)+ 2Al (s) → 3Cu (s) + 2A1³* (aq) 2+ in one half-cell and 1.05 M Al' in the other. .3+ Suppose the cell is prepared with 5.97 M Cu Calculate the cell voltage under these conditions. Round your answer to 3 significant digits.

A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 210, (aq) + 12H" (aq)+ 5Co (s) → L, (s)+ 6H,0 (1)+ 5Co" (aq) Suppose the cell is prepared with 6.10 M IO, and 1.61 M H' in one half-cell and 7.06 M Co 2+ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. х10

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 >

This is the full question. Please help explain.