(a) In the electrolysis of aqueous Na2O2, how many liters of H2(g) (at STP) are generated by a current of 64.5 A for a period of 90.0 min? The unbalanced chemical reaction representing this electrolysis is shown below. Na2O2(aq) + H2O(l)  O2(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.

Metallic iron can be made by the electrolysis of molten Fe2O3.(a) What mass of Fe is formed by passing a current of 6.22 A through molten Fe2O3 for 1.10 days? The unbalanced chemical reaction representing this electrolysis is shown below.Fe2O3  Fe + O2______ g of Fe is formed by this electrolysis.(b) How many minutes are needed to plate out 6.00 g of Fe from molten Fe2O3 using 6.15 A current?_______ minutes are needed.

What mass of each of the following substances can be produced in 1.2 h with a current of 11 A? (a) Co from aqueous Co²+ 14 g (b) 21 (c) (d) Hf from aqueous Hf4+ g I₂ from aqueous KI X g Cr from molten CrO3 X 9

An aqueous solution of an unknown salt of rhodium is electrolyzed by a current of 2.50 A passing for 51.0 min. If 2.720 g Rh is produced at the cathode, what is the charge on the rhodium ions in solution? (Enter your answer using the format +1 and -2.)

Consider the following half-reactions: Half-reaction E° (V) I2(s) + + 2e 21(aq) 0.535V Ni2+ "(aq) + 2e¯ → Ni(s)|-0.250V A³*(aq) + 3e Al(s) -1.660V > (1) The strongest oxidizing agent is: enter formula (2) The weakest oxidizing agent is: (3) The weakest reducing agent is: (4) The strongest reducing agent is: (5) Will Al*(aq) oxidize I'(aq) to I2(s)? (6) Which species can be reduced by Ni(s)? If none, leave box blank.

Give typed full explanation not a single word hand written otherwise leave it

For the cell shown, the measured cell potential, Ecell, is -0.3537 V at 25 °C. Pt(s) | H₂(g, 0.837 atm) | H+ (aq, ? M) || Cd²+(aq, 1.00 M) | Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, Eº, are 2 H+ (aq) + 2 e- Cd²+(aq) + 2 e H₂(g) Cd(s) Calculate the H+ concentration. [H+] = Eº = 0.00 V E° -0.403 V M

An aqueous sodium chloride solution is electrolyzed using a current of 4.42 A. How much time (min) is required to collect 15.5 L of chlorine if the gas is collected over water at 20.0°C ánd the total pressure is 107.5 kPa? Assume that the water is already saturated with chlorine so no more dissolves. Assume Ptotal(gas) P(Cl2,g) + P(H20,g) and that the correction for column height is negligible. The vapor pressure of water at 20.0°C is 2.34 kPa, F = 96485 C/mol e". and R = 8.314 kPa-L-mol1.K´1 Enter your final answer for the time required in units of minutes. Include only the numerical answer (no units).

For the cell shown, the measured cell potential, Ecell, is -0.3651 V at 25 °C. Pt(s) | H₂(g, 0.797 atm) | H+ (aq, ? M) || Cd²+ (aq, 1.00 M) | Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, Eº, are 2 H+ (aq) + 2 e- → H₂(g) Cd²+ (aq) + 2e → Cd(s) Calculate the H+ concentration. [H+] = x10 TOOLS - Eº = 0.00 V Eº = -0.403 V M

A galvanic cell Mn(s)|Mn2+(aq) || Pb2+(aq)|Pb(s) is constructed using a completely immersed Mn electrode that weighs 34.9 g and a Pb electrode immersed in 532 mL of 1.00 M Pb2+(ag) solution. A steady current of 0.0519 A is drawn from the cell as the electrons move from the Mn electrode to the Pb electrode. (a) Which reactant is the limiting reactant in this cell? Enter symbol (b) How long does it take for the cell to be completely discharged? (c) How much mass has the Pb electrode gained when the cell is completely discharged? g (d) What is the concentration of the Pb2+(aq) when the cell is completely discharged? (Assume that the limiting reactant is 100% reacted.) M