Rhodium is a bright, hard, and highly reflective metal. It is most commonly used to plate white gold as this metal naturally has a yellow tone. If 1.91 g of rhodium is deposited at the cathode when a current of 6.65 A passes through an electrolytic cell for 1620 seconds, what is the oxidation state of rhodium in the aqueous solution? (MW of rhodium=102.91 g/mol; Faraday constant = 96485 C/mol e').

Aluminum is produced commercially by the electrolysis of Al203 in the presence of a molten salt. If a plant has a continuous capacity of 1.09 million A, what mass of aluminum can be produced in 3.00 h? Mass = 5.94x10^5

How many grams of iron may be formed by the passage of 6,931 C through an electrolytic cell that contains an aqueous ferrous (Fe(II)) salt.

1.A metal "X" is used as a “sacrificial” anode on hulls of salt water vessels made of iron. The effect is to reverse the oxidation of iron to iron (II) by causing X to oxidize to the X ion. Calculate the voltage (in V, to two decimal places) for this reaction if it takes place under standard conditions. The standard reduction potential for X is -0.52 V (minus 0.52 V). 2.Batteries are charged and discharged due to the concentration of the solutions inside. Calculate the voltage of a battery made from zinc in a 0.1M solution of Zn2+ and a metal X in a 1 M X2+ solution using the table of reduction potentials and Eq. 6 at 25 degrees C. Answer with the unit V, to two decimal places. The standard reduction potential of X is -0.46 volts.

The molar mass of a metal (M) is 50.9 g/mol; it forms a chlorideof unknown composition. Electrolysis of a sample of the moltenchloride with a current of 6.42 A for 23.6 minutes produces1.20 g of M at the cathode. Determine the empirical formula ofthe chloride.

Tin cans are made of a steel, the inside of which is coated with a thin layer of tin. The tin protects the steel from corrosion by food products in the same manner as zinc protects steel from atmospheric corrosion. Briefly explain how this cathodic protection of tin cans is possible, given that tin is electrochemically less active than steel in the galvanic series.

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A metal "X" is used as a “sacrificial” anode on hulls of salt water vessels made of iron. The effect is to reverse the oxidation of iron to iron (II) by causing X to oxidize to the X ion. Calculate the voltage (in V, to two decimal places) for this reaction if it takes place under standard conditions. The standard reduction potential for X is -1.20 V (minus 1.20 V).

A metal "X" is used as a “sacrificial” anode on hulls of salt water vessels made of iron. The effect is to reverse the oxidation of iron to iron (II) by causing X to oxidize to the X ion. Calculate the voltage (in V, to two decimal places) for this reaction if it takes place under standard conditions. The standard reduction potential for X is -1.08 V (minus 1.08 V).

What period of time (in hours) is required to produce 1.00mol of chlorine using a current of 5.00A?