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150 ml hydrogen was produced and collected over water at total pressure of 752mm Hg and 301k on passing current through the acidulated water for 1hr. Calculate the current in coloumbs per second which was passed during electrolysis (the vapour pressure of H2o at 301k is 28mmHg) ?
Most Upvoted Answer
150 ml hydrogen was produced and collected over water at total pressur...
Here, volume of H2 gas = 150 ml =0.15L,
Now,in order to obtain the true pressure of hydrogen in the container the total pressure must be reduced by the equilibrium vapour pressure of the water over which the hydrogen is collected.
P = (752-28) /760)mm x 101.3 kPa =(724 /760) x 101.3 = 96.50 kPa, R = 8.314 lkPa/molK, Temperature = 301 K
Since, PV = nRT
no. of moles of H2 gas = PV/RT =96.50x 0.15/ 8.314 x 301 = 0.00578
no. of moles = 0.00578
Since, 1 mole H2 gas contains = 6.022 x 1023 H2 molecules
So, 0.0057 mole = 6.022 x 1023 x 0.00578 = 0.0348 x 1023 H2 molecules
So, no. of electrons (two electrons in each molecule) = 2 x 0.0348 x 1023 =0.069 x1023 electrons
Henc, charge, Q = n x e = 0.069 x1023 x 1.6 x 10-19 =0.1104x 104 = 1104 C
Here, given that, time = 1 hr = 60 x 60 = 3600s
Now, current produce, I = Q/t = 1104/3600 = 0.306 Amp.
Now,in order to obtain the true pressure of hydrogen in the container the total pressure must be reduced by the equilibrium vapour pressure of the water over which the hydrogen is collected.
P = (752-28) /760)mm x 101.3 kPa =(724 /760) x 101.3 = 96.50 kPa, R = 8.314 lkPa/molK, Temperature = 301 K
Since, PV = nRT
no. of moles of H2 gas = PV/RT =96.50x 0.15/ 8.314 x 301 = 0.00578
no. of moles = 0.00578
Since, 1 mole H2 gas contains = 6.022 x 1023 H2 molecules
So, 0.0057 mole = 6.022 x 1023 x 0.00578 = 0.0348 x 1023 H2 molecules
So, no. of electrons (two electrons in each molecule) = 2 x 0.0348 x 1023 =0.069 x1023 electrons
Henc, charge, Q = n x e = 0.069 x1023 x 1.6 x 10-19 =0.1104x 104 = 1104 C
Here, given that, time = 1 hr = 60 x 60 = 3600s
Now, current produce, I = Q/t = 1104/3600 = 0.306 Amp.
Community Answer
150 ml hydrogen was produced and collected over water at total pressur...
Calculating the Current Passed during Electrolysis
Given Data:
- Volume of hydrogen gas collected: 150 ml
- Total pressure of the system: 752 mmHg
- Temperature of the system: 301 K
- Vapour pressure of water at 301 K: 28 mmHg
To calculate the current passed during electrolysis, we need to use the ideal gas law equation:
PV = nRT
Where:
- P is the pressure of the gas
- V is the volume of the gas
- n is the number of moles of the gas
- R is the ideal gas constant
- T is the temperature in Kelvin
Step 1: Convert the given pressure and vapor pressure to atmospheres.
- Total pressure of the system = 752 mmHg = 752/760 atm ≈ 0.9895 atm
- Vapor pressure of water = 28 mmHg = 28/760 atm ≈ 0.0368 atm
Step 2: Calculate the pressure of the hydrogen gas.
- Pressure of hydrogen gas = Total pressure - Vapor pressure of water
= 0.9895 atm - 0.0368 atm = 0.9527 atm
Step 3: Convert the volume of hydrogen gas to liters.
- Volume of hydrogen gas = 150 ml = 150/1000 L = 0.15 L
Step 4: Calculate the number of moles of hydrogen gas using the ideal gas law equation.
PV = nRT
0.9527 atm * 0.15 L = n * 0.0821 atm L/mol K * 301 K
n ≈ (0.9527 * 0.15) / (0.0821 * 301) ≈ 0.0076 mol
Step 5: Calculate the charge passed during electrolysis using Faraday's law.
1 mole of electrons = 1 Faraday = 96,485 C
0.0076 mol of electrons = 0.0076 * 96,485 C ≈ 732.76 C
Step 6: Calculate the current passed per second.
1 hour = 3600 seconds
Current = Charge / Time
Current = 732.76 C / 3600 s ≈ 0.203 A ≈ 203 mA
Therefore, the current passed during electrolysis is approximately 203 mA.
Given Data:
- Volume of hydrogen gas collected: 150 ml
- Total pressure of the system: 752 mmHg
- Temperature of the system: 301 K
- Vapour pressure of water at 301 K: 28 mmHg
To calculate the current passed during electrolysis, we need to use the ideal gas law equation:
PV = nRT
Where:
- P is the pressure of the gas
- V is the volume of the gas
- n is the number of moles of the gas
- R is the ideal gas constant
- T is the temperature in Kelvin
Step 1: Convert the given pressure and vapor pressure to atmospheres.
- Total pressure of the system = 752 mmHg = 752/760 atm ≈ 0.9895 atm
- Vapor pressure of water = 28 mmHg = 28/760 atm ≈ 0.0368 atm
Step 2: Calculate the pressure of the hydrogen gas.
- Pressure of hydrogen gas = Total pressure - Vapor pressure of water
= 0.9895 atm - 0.0368 atm = 0.9527 atm
Step 3: Convert the volume of hydrogen gas to liters.
- Volume of hydrogen gas = 150 ml = 150/1000 L = 0.15 L
Step 4: Calculate the number of moles of hydrogen gas using the ideal gas law equation.
PV = nRT
0.9527 atm * 0.15 L = n * 0.0821 atm L/mol K * 301 K
n ≈ (0.9527 * 0.15) / (0.0821 * 301) ≈ 0.0076 mol
Step 5: Calculate the charge passed during electrolysis using Faraday's law.
1 mole of electrons = 1 Faraday = 96,485 C
0.0076 mol of electrons = 0.0076 * 96,485 C ≈ 732.76 C
Step 6: Calculate the current passed per second.
1 hour = 3600 seconds
Current = Charge / Time
Current = 732.76 C / 3600 s ≈ 0.203 A ≈ 203 mA
Therefore, the current passed during electrolysis is approximately 203 mA.
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150 ml hydrogen was produced and collected over water at total pressure of 752mm Hg and 301k on passing current through the acidulated water for 1hr. Calculate the current in coloumbs per second which was passed during electrolysis (the vapour pressure of H2o at 301k is 28mmHg) ?
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150 ml hydrogen was produced and collected over water at total pressure of 752mm Hg and 301k on passing current through the acidulated water for 1hr. Calculate the current in coloumbs per second which was passed during electrolysis (the vapour pressure of H2o at 301k is 28mmHg) ? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about 150 ml hydrogen was produced and collected over water at total pressure of 752mm Hg and 301k on passing current through the acidulated water for 1hr. Calculate the current in coloumbs per second which was passed during electrolysis (the vapour pressure of H2o at 301k is 28mmHg) ? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 150 ml hydrogen was produced and collected over water at total pressure of 752mm Hg and 301k on passing current through the acidulated water for 1hr. Calculate the current in coloumbs per second which was passed during electrolysis (the vapour pressure of H2o at 301k is 28mmHg) ?.
150 ml hydrogen was produced and collected over water at total pressure of 752mm Hg and 301k on passing current through the acidulated water for 1hr. Calculate the current in coloumbs per second which was passed during electrolysis (the vapour pressure of H2o at 301k is 28mmHg) ? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about 150 ml hydrogen was produced and collected over water at total pressure of 752mm Hg and 301k on passing current through the acidulated water for 1hr. Calculate the current in coloumbs per second which was passed during electrolysis (the vapour pressure of H2o at 301k is 28mmHg) ? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 150 ml hydrogen was produced and collected over water at total pressure of 752mm Hg and 301k on passing current through the acidulated water for 1hr. Calculate the current in coloumbs per second which was passed during electrolysis (the vapour pressure of H2o at 301k is 28mmHg) ?.
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