Question

Вычислите массу металла, выделившего на катоде и объем газа, образовавшегося на аноде при пропускании тока сильной 5 А через раствор нитрата меди (II) в течении 30 минут.

Answer 1

m=Mэ*Q / F;           Q=J*t;

Q=5*60*30=9000Кл;

m(Cu)=32*9000/ 9500=30,32г.

 

2Cu(NO3)2+2H2O= 2Cu + 4HNO3+O2

                                        2                          1

n(Cu)=30,32 : 64=0,47моль;  n(O2)=0,47/2=0,235моль;  V(O2)=0,235*22,4=5,264л.

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Answer 2

Calculation of Mass of Metal and Volume of Gas

To calculate the mass of metal deposited on the cathode and the volume of gas formed at the anode during the passage of a strong 5 A current through a solution of copper (II) nitrate for 30 minutes, we need to use Faraday's laws of electrolysis.

According to Faraday's laws of electrolysis, the mass of a substance deposited or liberated at an electrode is directly proportional to the quantity of electricity passed through the electrolyte. The relationship is given by the equation:

m = (Q * M) / (n * F)

Where: - m is the mass of the substance deposited or liberated (in grams) - Q is the quantity of electricity passed (in coulombs) - M is the molar mass of the substance (in grams per mole) - n is the number of electrons involved in the reaction - F is Faraday's constant (approximately 96,485 C/mol)

Similarly, the volume of gas formed can be calculated using the ideal gas law:

V = (Q * RT) / (P * nF)

Where: - V is the volume of gas formed (in liters) - Q is the quantity of electricity passed (in coulombs) - R is the ideal gas constant (approximately 0.0821 L·atm/(mol·K)) - T is the temperature (in Kelvin) - P is the pressure (in atmospheres) - n is the number of electrons involved in the reaction - F is Faraday's constant (approximately 96,485 C/mol)

Now, let's calculate the mass of metal and the volume of gas using the given information.

Calculation Steps:

1. Convert the current from amperes to coulombs per second: - 5 A = 5 C/s

2. Calculate the total charge passed (Q) using the current and time: - Q = current * time - Q = 5 C/s * 30 min * 60 s/min - Q = 9000 C

3. Determine the molar mass of copper (II) nitrate (Cu(NO3)2): - The molar mass of Cu(NO3)2 = atomic mass of Cu + (2 * atomic mass of N) + (6 * atomic mass of O) - The atomic masses can be found in the periodic table. - Molar mass of Cu = 63.55 g/mol - Molar mass of N = 14.01 g/mol - Molar mass of O = 16.00 g/mol - Molar mass of Cu(NO3)2 = 63.55 g/mol + (2 * 14.01 g/mol) + (6 * 16.00 g/mol) - Molar mass of Cu(NO3)2 = 187.55 g/mol

4. Determine the number of electrons involved in the reaction: - The reaction at the cathode is the reduction of Cu^2+ ions to Cu metal. - The reaction at the anode is the oxidation of NO3^- ions to form oxygen gas. - The balanced equation for the reduction reaction is: Cu^2+ + 2e^- -> Cu - The balanced equation for the oxidation reaction is: 2NO3^- -> O2 + 2e^- - Since 2 electrons are involved in both reactions, n = 2.

5. Calculate the mass of metal deposited on the cathode: - m = (Q * M) / (n * F) - m = (9000 C * 187.55 g/mol) / (2 * 96,485 C/mol) - m ≈ 8.78 g

6. Calculate the volume of gas formed at the anode: - Convert the temperature to Kelvin: - The operating time is 'Wednesday, December 06, 2023 03:44:10 UTC', which does not provide the temperature information. Therefore, we cannot calculate the volume of gas without the temperature.

Unfortunately, without the temperature information, we cannot calculate the volume of gas formed at the anode. Please provide the temperature so that we can complete the calculation.

Please note that the calculations provided above are based on the given information and assumptions. If there are any additional factors or conditions that need to be considered, please let me know.