Question

ДОПОМОЖІТЬ БУДЬ ЛАСКА ДУЖЕ СРОЧНО Визначте масу нікелю, що виділиться під час електролізу на катоді, якщо при силі струму 0,6 А процес тривав 1 годину  У повному колі зовнішній опір провідника 40 Ом, а сила струму в ньому 0,5 А. ЕРС гальванічної батареї дорівнює 25 В. Знайдіть внутрішній опір гальванічної батареї.

Answer 1

Ответ: 12

Объяснение:0потом

Answer 2

Calculation of the Mass of Nickel Deposited during Electrolysis

To determine the mass of nickel that is deposited during electrolysis, we can use Faraday's laws of electrolysis. According to Faraday's laws, the mass of a substance deposited or liberated during electrolysis is directly proportional to the quantity of electricity passed through the electrolyte.

The formula to calculate the mass of a substance deposited during electrolysis is:

m = (Q × M) / (n × F)

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

In this case, we want to calculate the mass of nickel deposited, so we need to know the molar mass of nickel. The molar mass of nickel is approximately 58.69 g/mol.

Given: - Current (I) = 0.6 A - Time (t) = 1 hour = 3600 seconds - External resistance (R) = 40 Ω - Current in the circuit (I') = 0.5 A - EMF of the galvanic cell (E) = 25 V

To calculate the quantity of electricity passed through the electrolyte (Q), we can use the formula:

Q = I × t

Substituting the given values:

Q = 0.6 A × 3600 s = 2160 C

Now, let's calculate the number of moles of electrons involved in the reaction (n). We can use the formula:

n = Q / (I' × t)

Substituting the given values:

n = 2160 C / (0.5 A × 3600 s) = 0.12 mol

Now, we can calculate the mass of nickel deposited (m) using the formula mentioned earlier:

m = (Q × M) / (n × F)

Substituting the given values:

m = (2160 C × 58.69 g/mol) / (0.12 mol × 96,485 C/mol) ≈ 0.27 g

Therefore, the mass of nickel that will be deposited during electrolysis is approximately 0.27 grams.

Calculation of the Internal Resistance of the Galvanic Cell

To find the internal resistance of the galvanic cell, we can use Ohm's law. Ohm's law states that the current flowing through a conductor is directly proportional to the voltage across it and inversely proportional to its resistance.

The formula to calculate the internal resistance (r) of the galvanic cell is:

r = (E - I' × R) / I'

Where: - r is the internal resistance of the galvanic cell (in ohms) - E is the EMF of the galvanic cell (in volts) - I' is the current in the circuit (in amperes) - R is the external resistance (in ohms)

Given: - EMF of the galvanic cell (E) = 25 V - Current in the circuit (I') = 0.5 A - External resistance (R) = 40 Ω

Substituting the given values into the formula:

r = (25 V - 0.5 A × 40 Ω) / 0.5 A ≈ 5 Ω

Therefore, the internal resistance of the galvanic cell is approximately 5 ohms.

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