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In a cylinder of pressure 1 bar, there is the hydrogen of 20 grams and neon of 50 grams, what is a partial pressure of hydrogen?
- a)0.2
- b)0.8
- c)0.4
- d)0.6
Correct answer is option 'B'. Can you explain this answer?
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In a cylinder of pressure 1 bar, there is the hydrogen of 20 grams and...
Partial Pressure of Hydrogen in a Cylinder
Given:
Pressure of the cylinder = 1 bar
Mass of hydrogen = 20 grams
Mass of neon = 50 grams
To find: Partial pressure of hydrogen
Partial Pressure Formula:
Partial pressure is the pressure exerted by an individual gas component in a mixture. It can be calculated using the formula:
Partial Pressure = (Mole Fraction) x (Total Pressure)
1. Calculate the Mole Fraction of Hydrogen:
The mole fraction of a gas component is the ratio of the number of moles of that gas to the total number of moles in the mixture. It can be calculated using the formula:
Mole Fraction = (Number of Moles of Hydrogen) / (Total Number of Moles)
To calculate the number of moles of hydrogen, we need to know the molar mass of hydrogen. The molar mass of hydrogen is approximately 2 g/mol.
Number of Moles of Hydrogen = (Mass of Hydrogen) / (Molar Mass of Hydrogen)
= 20 g / 2 g/mol
= 10 moles
To calculate the total number of moles, we need to know the molar masses of hydrogen and neon.
Molar Mass of Neon = 20 g/mol
Number of Moles of Neon = (Mass of Neon) / (Molar Mass of Neon)
= 50 g / 20 g/mol
= 2.5 moles
Total Number of Moles = Number of Moles of Hydrogen + Number of Moles of Neon
= 10 moles + 2.5 moles
= 12.5 moles
Mole Fraction of Hydrogen = (Number of Moles of Hydrogen) / (Total Number of Moles)
= 10 moles / 12.5 moles
= 0.8
2. Calculate the Partial Pressure of Hydrogen:
Using the formula for partial pressure:
Partial Pressure of Hydrogen = (Mole Fraction of Hydrogen) x (Total Pressure)
= 0.8 x 1 bar
= 0.8 bar
Therefore, the partial pressure of hydrogen in the cylinder is 0.8 bar, which corresponds to option B.
Given:
Pressure of the cylinder = 1 bar
Mass of hydrogen = 20 grams
Mass of neon = 50 grams
To find: Partial pressure of hydrogen
Partial Pressure Formula:
Partial pressure is the pressure exerted by an individual gas component in a mixture. It can be calculated using the formula:
Partial Pressure = (Mole Fraction) x (Total Pressure)
1. Calculate the Mole Fraction of Hydrogen:
The mole fraction of a gas component is the ratio of the number of moles of that gas to the total number of moles in the mixture. It can be calculated using the formula:
Mole Fraction = (Number of Moles of Hydrogen) / (Total Number of Moles)
To calculate the number of moles of hydrogen, we need to know the molar mass of hydrogen. The molar mass of hydrogen is approximately 2 g/mol.
Number of Moles of Hydrogen = (Mass of Hydrogen) / (Molar Mass of Hydrogen)
= 20 g / 2 g/mol
= 10 moles
To calculate the total number of moles, we need to know the molar masses of hydrogen and neon.
Molar Mass of Neon = 20 g/mol
Number of Moles of Neon = (Mass of Neon) / (Molar Mass of Neon)
= 50 g / 20 g/mol
= 2.5 moles
Total Number of Moles = Number of Moles of Hydrogen + Number of Moles of Neon
= 10 moles + 2.5 moles
= 12.5 moles
Mole Fraction of Hydrogen = (Number of Moles of Hydrogen) / (Total Number of Moles)
= 10 moles / 12.5 moles
= 0.8
2. Calculate the Partial Pressure of Hydrogen:
Using the formula for partial pressure:
Partial Pressure of Hydrogen = (Mole Fraction of Hydrogen) x (Total Pressure)
= 0.8 x 1 bar
= 0.8 bar
Therefore, the partial pressure of hydrogen in the cylinder is 0.8 bar, which corresponds to option B.
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In a cylinder of pressure 1 bar, there is the hydrogen of 20 grams and...
As we know that the partial pressure of a gas is the product of its mole fraction and the total pressure of the gases present, so here the partial pressure of hydrogen is 10/10 + 2.5 = 0.8. Mole fraction is given by the number of moles of required as per the total number of the gas moles.
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In a cylinder of pressure 1 bar, there is the hydrogen of 20 grams and neon of 50 grams, what is a partial pressure of hydrogen?a)0.2b)0.8c)0.4d)0.6Correct answer is option 'B'. Can you explain this answer?
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