Question

6. Раствор сульфата никеля подвергали электролизу током в 15 А в течение часа. На катоде выделились никель и водород, при этом 60 % напряжения было израсходовано на выделение никеля. Какова масса никеля, выделенная на катоде? Каков объём водорода, если электролиз проводился при нормальных условиях? По возможности решение на бумаге

Answer 1

Через электролизер пропущено q = It = 15A.3600 сек = 54000 кл, что соответствует выделению в результате электролиза 54000/96500 = 0.56 г-экв вещества.

На выделение никеля пошло 0,6q, т.е. должно получиться 0,56.0,6 = 0,336 г-экв, или 29,4.0,336 = 9,9 г Ni (Э = А/2 = 58,71/2 29,4).

Поверхность пластины при двухстороннем покрытии 2.4.4=32 см2. При плотности 8,9 г/см3 полученный никель займет объем 9,9г / 8,9г/cм3 =1,11 cм3 и пластина будет покрыта слоем 1,11см3/32см2 = 0,35 мм

В ходе электролиза выделится 0,56.0,4 = 0,224г-экв водорода или 0,224.11,2=2,5л Н2 (условия нормальные).

Answer 2

Electrolysis of Nickel Sulfate Solution

To calculate the mass of nickel deposited on the cathode and the volume of hydrogen gas evolved during the electrolysis of a nickel sulfate solution, we need to consider the current, time, and Faraday's laws of electrolysis.

Given: - Current (I) = 15 A - Time (t) = 1 hour = 3600 seconds - Voltage used for nickel deposition = 60% of the total voltage

Calculation of Mass of Nickel Deposited

According to Faraday's first law of electrolysis, the amount of substance deposited or liberated at an electrode is directly proportional to the quantity of electricity passed through the electrolyte.

The quantity of electricity (Q) can be calculated using the formula: Q = I * t

The number of moles of nickel deposited (n) can be calculated using Faraday's constant (F) and the charge (Q): n = Q / (2 * F)

The molar mass of nickel (M) is 58.69 g/mol.

The mass of nickel deposited (m) can be calculated using the formula: m = n * M

Calculation of Volume of Hydrogen Gas Evolved

According to Faraday's second law of electrolysis, the amount of gas evolved at an electrode is directly proportional to the quantity of electricity passed through the electrolyte.

The volume of hydrogen gas evolved (V) can be calculated using the formula: V = (Q * 22.4) / (2 * F)

Note: The volume of hydrogen gas is calculated at standard temperature and pressure (STP), which is 22.4 L/mol.

Now, let's calculate the mass of nickel deposited and the volume of hydrogen gas evolved.

Solution:

1. Calculate the quantity of electricity (Q): Q = I * t = 15 A * 3600 s = 54,000 C

2. Calculate the number of moles of nickel deposited (n): n = Q / (2 * F) = 54,000 C / (2 * 96,485 C/mol) = 0.279 mol

3. Calculate the mass of nickel deposited (m): m = n * M = 0.279 mol * 58.69 g/mol = 16.36 g

Therefore, the mass of nickel deposited on the cathode is 16.36 grams.

4. Calculate the volume of hydrogen gas evolved (V): V = (Q * 22.4) / (2 * F) = (54,000 C * 22.4 L/mol) / (2 * 96,485 C/mol) = 24.94 L

Therefore, the volume of hydrogen gas evolved during the electrolysis, under normal conditions, is 24.94 liters.

Please note that the above calculations are based on the given information and assumptions.