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A steady current was allowed to flow through the solution for 3hours.at STP 4.12dm^3of the gas relighted the growing splint was produced.work out current flowing in the circuit ?
Deh Swaggz
more than 2 weeks ago
A steady current was allowed to flow through the solution for 3hours.at STP 4.12dm^3of the gas relighted the growing splint was produced.work out current flowing in the circuit ?
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ChatGPT
more than 2 weeks ago
To calculate the current flowing in the circuit, we need to first determine the amount of gas produced during the electrolysis process.
From the given information, 4.12 dm^3 of gas was produced during the electrolysis. Since the gas relighted a growing splint, we can assume that the gas produced is hydrogen gas (H2).
The molar volume of a gas at STP (Standard Temperature and Pressure) is 22.4 dm^3/mol. Therefore, 4.12 dm^3 of hydrogen gas is equivalent to:
4.12 dm^3 / 22.4 dm^3/mol = 0.1836 mol
Since the balanced equation for the electrolysis of water is:
2H2O -> 2H2 + O2
We can see that 1 mol of H2 gas is produced for every 2 moles of electrons transferred. Therefore, 0.1836 mol of H2 gas produced corresponds to 0.1836 mol of electrons transferred.
Now, we need to calculate the charge (in Coulombs) that corresponds to 0.1836 mol of electrons transferred. The Faraday constant is 96485 C/mol, so:
Charge = 0.1836 mol * 96485 C/mol = 17727.66 C
Since the current (I) is defined as the rate of flow of charge, we can calculate the current flowing in the circuit by dividing the total charge by the time (3 hours = 10800 seconds):
Current (I) = 17727.66 C / 10800 s = 1.64 A
Therefore, the current flowing in the circuit during the electrolysis process is 1.64 Amperes.
From the given information, 4.12 dm^3 of gas was produced during the electrolysis. Since the gas relighted a growing splint, we can assume that the gas produced is hydrogen gas (H2).
The molar volume of a gas at STP (Standard Temperature and Pressure) is 22.4 dm^3/mol. Therefore, 4.12 dm^3 of hydrogen gas is equivalent to:
4.12 dm^3 / 22.4 dm^3/mol = 0.1836 mol
Since the balanced equation for the electrolysis of water is:
2H2O -> 2H2 + O2
We can see that 1 mol of H2 gas is produced for every 2 moles of electrons transferred. Therefore, 0.1836 mol of H2 gas produced corresponds to 0.1836 mol of electrons transferred.
Now, we need to calculate the charge (in Coulombs) that corresponds to 0.1836 mol of electrons transferred. The Faraday constant is 96485 C/mol, so:
Charge = 0.1836 mol * 96485 C/mol = 17727.66 C
Since the current (I) is defined as the rate of flow of charge, we can calculate the current flowing in the circuit by dividing the total charge by the time (3 hours = 10800 seconds):
Current (I) = 17727.66 C / 10800 s = 1.64 A
Therefore, the current flowing in the circuit during the electrolysis process is 1.64 Amperes.
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