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0.24 g of a volatile liquid on vaporization gives 45 ml of vapours at STP.What will be the vapour density of the substance ?(Density of H₂ = 0.089 gL⁻1)
- a)95.39
- b)39.95
- c)99.53
- d)59.93
Correct answer is option 'D'. Can you explain this answer?
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0.24 g of a volatile liquid on vaporization gives 45 ml of vapours at ...
Given:
Mass of the volatile liquid = 0.24 g
Volume of vapors at STP = 45 ml = 45 cm^3
Density of hydrogen (H2) gas = 0.089 g/L
To find: Vapour density of the substance
Vapour density is defined as the ratio of the molar mass of a substance to the molar mass of hydrogen gas.
We can calculate the molar mass of the substance using the ideal gas equation:
PV = nRT
Where:
P = Pressure (in atm)
V = Volume (in L)
n = Number of moles of the substance
R = Ideal gas constant (0.082 L.atm/mol.K)
T = Temperature (in K)
Since the volume is given at STP, we can assume the pressure to be 1 atm and the temperature to be 273 K.
Using the ideal gas equation, we can rearrange it to solve for n:
n = PV / RT
Since the volume is given in cm^3, we need to convert it to L:
Volume = 45 cm^3 = 45/1000 L = 0.045 L
Substituting the given values into the equation:
n = (1 atm) (0.045 L) / [(0.082 L.atm/mol.K) (273 K)]
n = 0.00176 mol
The molar mass of the substance can be calculated using the formula:
Molar mass = mass / number of moles
Substituting the given values into the equation:
Molar mass = 0.24 g / 0.00176 mol
Molar mass = 136.36 g/mol
The molar mass of hydrogen gas (H2) is 2 g/mol.
Finally, we can calculate the vapour density of the substance:
Vapour density = Molar mass / Molar mass of H2
Vapour density = 136.36 g/mol / 2 g/mol
Vapour density = 68.18
Since the options provided are in g/L, we need to convert the vapour density to g/L by multiplying it by the density of hydrogen gas:
Vapour density = 68.18 * 0.089 g/L
Vapour density = 6.07 g/L
Therefore, the correct answer is option 'D': 59.93 g/L.
Mass of the volatile liquid = 0.24 g
Volume of vapors at STP = 45 ml = 45 cm^3
Density of hydrogen (H2) gas = 0.089 g/L
To find: Vapour density of the substance
Vapour density is defined as the ratio of the molar mass of a substance to the molar mass of hydrogen gas.
We can calculate the molar mass of the substance using the ideal gas equation:
PV = nRT
Where:
P = Pressure (in atm)
V = Volume (in L)
n = Number of moles of the substance
R = Ideal gas constant (0.082 L.atm/mol.K)
T = Temperature (in K)
Since the volume is given at STP, we can assume the pressure to be 1 atm and the temperature to be 273 K.
Using the ideal gas equation, we can rearrange it to solve for n:
n = PV / RT
Since the volume is given in cm^3, we need to convert it to L:
Volume = 45 cm^3 = 45/1000 L = 0.045 L
Substituting the given values into the equation:
n = (1 atm) (0.045 L) / [(0.082 L.atm/mol.K) (273 K)]
n = 0.00176 mol
The molar mass of the substance can be calculated using the formula:
Molar mass = mass / number of moles
Substituting the given values into the equation:
Molar mass = 0.24 g / 0.00176 mol
Molar mass = 136.36 g/mol
The molar mass of hydrogen gas (H2) is 2 g/mol.
Finally, we can calculate the vapour density of the substance:
Vapour density = Molar mass / Molar mass of H2
Vapour density = 136.36 g/mol / 2 g/mol
Vapour density = 68.18
Since the options provided are in g/L, we need to convert the vapour density to g/L by multiplying it by the density of hydrogen gas:
Vapour density = 68.18 * 0.089 g/L
Vapour density = 6.07 g/L
Therefore, the correct answer is option 'D': 59.93 g/L.
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0.24 g of a volatile liquid on vaporization gives 45 ml of vapours at STP.What will be the vapour density of the substance ?(Density of H = 0.089 gL1)a)95.39b)39.95c)99.53d)59.93Correct answer is option 'D'. Can you explain this answer?
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0.24 g of a volatile liquid on vaporization gives 45 ml of vapours at STP.What will be the vapour density of the substance ?(Density of H = 0.089 gL1)a)95.39b)39.95c)99.53d)59.93Correct answer is option 'D'. Can you explain this answer? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about 0.24 g of a volatile liquid on vaporization gives 45 ml of vapours at STP.What will be the vapour density of the substance ?(Density of H = 0.089 gL1)a)95.39b)39.95c)99.53d)59.93Correct answer is option 'D'. Can you explain this answer? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 0.24 g of a volatile liquid on vaporization gives 45 ml of vapours at STP.What will be the vapour density of the substance ?(Density of H = 0.089 gL1)a)95.39b)39.95c)99.53d)59.93Correct answer is option 'D'. Can you explain this answer?.
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