Question

In: Chemistry

Metallic magnesium can be made by the electrolysis of molten MgCl2. Part A What mass of...

Metallic magnesium can be made by the electrolysis of molten MgCl2.

Part A

What mass of Mg is formed by passing a current of 6.00 A through molten MgCl2 for 4.60 days?

m =   g Mg  

Part B

How many minutes are needed to plate out 29.00 g Mg from molten MgCl2, using 4.10 A of current?

t =   min

Solutions

Expert Solution

A)

the electrolysis expression is:

Mg2+ + 2e- ------> Mg

1 mol of Mg requires 2 mol of electron

1 mol of electron = 96485 C

So,1 mol of Mg requires 192970 C

let us calculate the charge passed:

t = 4.6 days = 4.6*24*3600 s = 397439 s

time, t = 397439s

Q = I*t

= 6A * 397439s

= 2384634 C

mol of Mg plated = 2384634/192970 = 12.35754 mol

Molar mass of Mg = 24.31 g/mol

mass of Mg = number of mol * molar mass

= 12.35754 * 24.31

= 300. g

Answer = 300. g

B)

the electrolysis expression is:

Mg2+ + 2e- ------> Mg

1 mol of Mg requires 2 mol of electron

1 mol of electron = 96485 C

So,1 mol of Mg requires 192970 C

let us calculate mol of element deposited:

we have below equation to be used:

number of mol, n = mass/molar mass

= 29/24.31

= 1.19292 mol

total charge = mol of element deposited * charge required for 1 mol

= 1.19292*192970

= 230198.6837 C

we have below equation to be used:

time = Q/i

= 230198.6837/4.1

= 56146.0204 seconds

= 56146.0204/60 min

= 936 min

Answer: 936 min


Related Solutions

Metallic magnesium can be made by the electrolysis of molten MgCl2. Part A What mass of...
Metallic magnesium can be made by the electrolysis of molten MgCl2. Part A What mass of Mg is formed by passing a current of 4.00 A through molten MgCl2 for 4.70 days? Express your answer using three significant figures. Part B How many minutes are needed to plate out 26.00 g Mg from molten MgCl2, using 2.90 A of current? Express your answer using three significant figures.
Metallic magnesium can be made by the electrolysis of molten MgCl2. a. What mass of Mg...
Metallic magnesium can be made by the electrolysis of molten MgCl2. a. What mass of Mg is formed by passing a current of 5.35 A through molten MgCl2 for 3.30 days? b. How many minutes are needed to plate out 18.00 g Mg from molten MgCl2, using 3.20 A of current?
A current of 6.15×104 A is passed through an electrolysis cell containing molten MgCl2 for 6.50...
A current of 6.15×104 A is passed through an electrolysis cell containing molten MgCl2 for 6.50 days. (a) How many grams of magnesium are produced? _____g (b) How many liters of chlorine are collected, if the gas is at a temperature of 273 K and a pressure of 1.00 atm? _____L
What substance is produced at the cathode during the electrolysis of molten calcium bromide, CaBr2
Part A: What substance is produced at the cathode during the electrolysis of molten calcium bromide, CaBr2? Assume standard conditions. Express your answer as a chemical formula. Part B: What substance is produced at the anode during the electrolysis of molten calcium bromide, CaBr2? Assume standard conditions. Part C: What substance is produced at the cathode during the electrolysis of a mixture of molten calcium bromide, CaBr2(l), and molten magnesium iodide MgI2(l),? Assume standard conditions. Express your answer as a...
Magnesium oxide can be made by heating magnesium metal in the presence of the oxygen. The...
Magnesium oxide can be made by heating magnesium metal in the presence of the oxygen. The balanced equation for the reaction is 2Mg(s)+O2(g)→2MgO(s) When 10.15 g Mg is allowed to react with 10.40 g O2, 11.85 g MgO is collected. Determine the theoretical yield for the reaction. Express your answer in grams. Determine the percent yield for the reaction. Express your answer as a percent.
Magnesium oxide can be made by heating magnesium metal in the presence of oxygen. The balanced...
Magnesium oxide can be made by heating magnesium metal in the presence of oxygen. The balanced equation for the reaction is: 2Mg(s)+O2(g)→2MgO(s) When 10.1 g of Mg are allowed to react with 10.5 g of O2, 12.4 g of MgO are collected. Part A:    Determine the limiting reactant for the reaction. Express your answer as a chemical formula. Part B: Determine the theoretical yield for the reaction. Part C: Determine percent yield for the reaction.
The following data was obtained for Part B of the lab: Mass of Cu before electrolysis...
The following data was obtained for Part B of the lab: Mass of Cu before electrolysis = 20.6133 g Mass of Cu after electrolysis = 20.4697 g Time of electrolysis = 514 sec Average current = 0.85 Amp Volume of gas collected = 55.6 mL Atmospheric pressure (corrected to standard conditions) = 758.4 mmHg Room temperature = 19.2 °C Vapour pressure of water at 19.2 °C = 16.7 mmHg Using this data determine: Moles of Cu consumed: Moles of H2...
The following data was obtained for Part B of the lab: Mass of Cu before electrolysis...
The following data was obtained for Part B of the lab: Mass of Cu before electrolysis = 20.5492 g Mass of Cu after electrolysis = 20.3860 g Time of electrolysis = 563 sec Average current = 0.88 Amp Volume of gas collected = 62.7 mL Atmospheric pressure (corrected to standard conditions) = 760.4 mmHg Room temperature = 18.1 °C Vapour pressure of water at 18.1 °C = 15.6 mmHg Using this data determine: Moles of Cu consumed:---------- moles Moles of...
You are given some ferrous iodide, , and are asked to extract the iron through electrolysis. What can be said about the merits of molten versus aqueous FeI2
You are given some ferrous iodide and are asked to extract the iron through electrolysis. What can be said about the merits of molten versus aqueous FeI2? You'll have to perform electrolysis of the aqueous solution because you can't get iron metal from electrolysis of the molten salt. You'll have to perform electrolysis on the molten salt because you can't get iron metal from electrolysis of the aqueous solution. Electrolysis of either the molten or aqueous salt will produce solid...
QUESTION 1 Magnesium chloride (MgCl2) dissolves completely in water. What is the molarity of the Mg2+(aq)...
QUESTION 1 Magnesium chloride (MgCl2) dissolves completely in water. What is the molarity of the Mg2+(aq) cation in a 0.00500 M MgCl2(aq) solution? (3 significant digits, units M) 1 points    QUESTION 2 What is the molarity of Cl-(aq) anion in the same solution as Question 1? (3 significant digits, units M) 1 points    QUESTION 3 The parts per million (ppm) unit can be expressed as mg solute per liter solution (mg/L) for dilute aqueous solutions. Convert the Mg2+(aq)concentration...
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT