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An aqueous solution containing 288 g of a non–volatile compound having the stoichiometric composit ion CxH2xOx in 90 g water boils at 101.24ºC at 1 atmospheric pressure. What is the value of x? (Given that: Kb(H2O) = 0.512 K Kg mol–1):
Correct answer is '44'. Can you explain this answer?
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An aqueous solution containing 288 g of a non–volatile compound ...
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An aqueous solution containing 288 g of a non–volatile compound ...
Given:
- Mass of nonvolatile compound = 288 g
- Mass of water = 90 g
- Boiling point of solution = 101.24 °C
- Pressure = 1 atm
- Kb(H2O) = 0.512 K kg mol^-1
To Find:
Value of x in the stoichiometric composition CxH2xOx
Solution:
Molality (m) is defined as the moles of solute per kilogram of solvent.
Molar mass of water (H2O) = 2 * 1 + 16 = 18 g/mol
Number of moles of water = Mass of water / Molar mass of water
= 90 g / 18 g/mol
= 5 mol
Molality (m) = (Number of moles of solute) / (Mass of solvent in kg)
= (288 g / Molar mass of solute) / (90 g / 1000)
= (288 / Molar mass of solute) / 0.09
= 3.2 / Molar mass of solute
∆Tb = Kb * m
= 0.512 K kg mol^-1 * (3.2 / Molar mass of solute)
∆T = Boiling point of solution - Boiling point of pure solvent
= 101.24 °C - 100 °C
= 1.24 °C
∆T = Kb * m
1.24 °C = 0.512 K kg mol^-1 * (3.2 / Molar mass of solute)
Molar mass of solute = (0.512 K kg mol^-1 * 3.2) / 1.24 °C
= 1.315 K kg mol^-1
Given:
CxH2xOx has a stoichiometric composition
Molar mass of carbon (C) = 12 g/mol
Molar mass of hydrogen (H) = 1 g/mol
Molar mass of oxygen (O) = 16 g/mol
Molar mass of CxH2xOx = (12x + 1x + 16x) g/mol
= 29x g/mol
Molar mass of solute = 1.315 K kg mol^-1 = 29x g/mol
29x = 1.315 * 1000
x = 44
Therefore, the value of x in the stoichiometric composition CxH2xOx is 44.
- Mass of nonvolatile compound = 288 g
- Mass of water = 90 g
- Boiling point of solution = 101.24 °C
- Pressure = 1 atm
- Kb(H2O) = 0.512 K kg mol^-1
To Find:
Value of x in the stoichiometric composition CxH2xOx
Solution:
1. Calculate the molality (m) of the solution:
Molality (m) is defined as the moles of solute per kilogram of solvent.
Molar mass of water (H2O) = 2 * 1 + 16 = 18 g/mol
Number of moles of water = Mass of water / Molar mass of water
= 90 g / 18 g/mol
= 5 mol
Molality (m) = (Number of moles of solute) / (Mass of solvent in kg)
= (288 g / Molar mass of solute) / (90 g / 1000)
= (288 / Molar mass of solute) / 0.09
= 3.2 / Molar mass of solute
2. Calculate the change in boiling point (∆Tb) of the solution:
∆Tb = Kb * m
= 0.512 K kg mol^-1 * (3.2 / Molar mass of solute)
3. Calculate the boiling point elevation (∆T) of the solution:
∆T = Boiling point of solution - Boiling point of pure solvent
= 101.24 °C - 100 °C
= 1.24 °C
4. Calculate the molar mass of the solute:
∆T = Kb * m
1.24 °C = 0.512 K kg mol^-1 * (3.2 / Molar mass of solute)
Molar mass of solute = (0.512 K kg mol^-1 * 3.2) / 1.24 °C
= 1.315 K kg mol^-1
Given:
CxH2xOx has a stoichiometric composition
Molar mass of carbon (C) = 12 g/mol
Molar mass of hydrogen (H) = 1 g/mol
Molar mass of oxygen (O) = 16 g/mol
Molar mass of CxH2xOx = (12x + 1x + 16x) g/mol
= 29x g/mol
Molar mass of solute = 1.315 K kg mol^-1 = 29x g/mol
29x = 1.315 * 1000
x = 44
Therefore, the value of x in the stoichiometric composition CxH2xOx is 44.
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An aqueous solution containing 288 g of a non–volatile compound having the stoichiometric composit ion CxH2xOx in 90 g water boils at 101.24ºC at 1 atmospheric pressure. What is the value of x? (Given that: Kb(H2O) = 0.512 K Kg mol–1):Correct answer is '44'. Can you explain this answer?
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An aqueous solution containing 288 g of a non–volatile compound having the stoichiometric composit ion CxH2xOx in 90 g water boils at 101.24ºC at 1 atmospheric pressure. What is the value of x? (Given that: Kb(H2O) = 0.512 K Kg mol–1):Correct answer is '44'. Can you explain this answer? for Chemistry 2024 is part of Chemistry preparation. The Question and answers have been prepared according to the Chemistry exam syllabus. Information about An aqueous solution containing 288 g of a non–volatile compound having the stoichiometric composit ion CxH2xOx in 90 g water boils at 101.24ºC at 1 atmospheric pressure. What is the value of x? (Given that: Kb(H2O) = 0.512 K Kg mol–1):Correct answer is '44'. Can you explain this answer? covers all topics & solutions for Chemistry 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for An aqueous solution containing 288 g of a non–volatile compound having the stoichiometric composit ion CxH2xOx in 90 g water boils at 101.24ºC at 1 atmospheric pressure. What is the value of x? (Given that: Kb(H2O) = 0.512 K Kg mol–1):Correct answer is '44'. Can you explain this answer?.
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