How many hours does it take to form 15.0 L of O₂ measured at 750 torr and 30°C from water by passing 2.75 A of current through an electrolytic cell?

Write the cell notation for an electrochemical cell consisting of an anode where Sn (s) is oxidized to Sn2+ (aq) and a cathode where H+ (aq) is reduced to H2 (g) at a platinum electrode . Assume all aqueous solutions have a concentration of 1 mol/L and gases have a pressure of 1 bar.

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The Nernst equation is one of the most important equations in electrochemistry. To calculate the cell potential at non-standard-state conditions, the equation is E = E-2.303RTn Flog 10Q where E is the potential in volts, Eo is the standard potential in volts, R is the gas constant, T is the temperature in kelvins, n is the number of moles of electrons transferred, F is the Faraday constant, and Q is the reaction quotient. Using the common reference temperature, 25 °C or 298 K, the equation has the form E = E-(0.0592n)logQ The reaction quotient has the usual form Q = [products]x[ reactants]y A table of standard reduction potentials gives the voltage at standard conditions, 1.00 M for all solutions and 1.00 atm for all gases. The Nernst equation allows for the calculation of the cell potential E at other conditions of concentration and pressure. Part A For the reaction 2C03 + (aq) + 2CI-(aq)-> 2Co2 + (aq )+ Cl2(g). E = 0.483 V what is the cell potential at 25° C if the concentrations are…

What is the electrical current, in Amperes, that must be applied if 6.50 g Ag is deposited at the cathode in 2.00 hrs during the electrolysis of AgNO3 (aq)? Please show your work

Determine the cell potential (in volts) of a standard galvanic cell constructed using iron and lead metals and their associated solutions, 1M FeSO4 and 1M PbSO4.

Write the cell notation for an electrochemical cell consisting of an anode where Mg (s) is oxidized to Mg2+ (aq) and a cathode where Cr3+ (aq) is reduced to Cr2+ (aq) at a platinum electrode . Assume all aqueous solutions have a concentration of 1 mol/L and gases have a pressure of 1 bar.

Write the cell notation for an electrochemical cell consisting of an anode where Mg (s) is oxidized to Mg²+ (aq) and a cathode where Cr³+ (aq) is reduced to Cr²+ (aq) at a platinum electrode. Assume all aqueous solutions have a concentration of 1 mol/L. Mg(s)| Mg2+ (aq)|| Cr³+ (aq)| Cr²+ (aq)| Pt(s)

From the following reaction. Ni + Sn+2 Ni2 + Sn Determine the cell formed; reactions; E°r; Ke and the type of reaction.