NEET Exam > NEET Questions > A solution of urea (mol. mass 56 g mol-l) boi...
Start Learning for Free
A solution of urea (mol. mass 56 g mol-l) boils at 100.18°C at the atmospheric pressure
If Kf and Kb for water are 1.86 and 0.52 K kg mol-1 respectively, the above solution will freeze at
- a)-6.54°C
- b)654°C
- c)0.654°C
- d)-0.654T
Correct answer is option 'D'. Can you explain this answer?
Most Upvoted Answer
A solution of urea (mol. mass 56 g mol-l) boils at 100.18°C at the...
∆Tb=∆Tb-∆Tbo= 100.18-100=018Celsius,
∆Tb =Kb×nb/v,
∆Tb= 0.52 × wb/56,
(0.18×56)/.52 = Wb
Wb=19.38g
∆Tf = ∆Tfo- ∆Tf,
0- Tf =1.86× 19.38/56,
-Tf=0.6436,
Tf= -0.6436~ -0.65
∆Tb =Kb×nb/v,
∆Tb= 0.52 × wb/56,
(0.18×56)/.52 = Wb
Wb=19.38g
∆Tf = ∆Tfo- ∆Tf,
0- Tf =1.86× 19.38/56,
-Tf=0.6436,
Tf= -0.6436~ -0.65
Free Test
FREE
| Start Free Test |
Community Answer
A solution of urea (mol. mass 56 g mol-l) boils at 100.18°C at the...
To determine the boiling point of a solution, we need to consider the boiling point elevation, which is given by the equation:
ΔTb = Kb * m
Where:
ΔTb = boiling point elevation
Kb = molal boiling point elevation constant
m = molality of the solution
First, we need to calculate the molality (m) of the solution. Molality is defined as the number of moles of solute per kilogram of solvent.
Given that the molecular mass of urea is 56 g/mol, we need to convert the mass of urea to moles:
Mass of urea = 56 g/mol
Now, we need to calculate the molality (m):
m = moles of solute / mass of solvent (in kg)
Since the solvent is not specified, we cannot calculate the exact molality without additional information. However, we can assume that the solution is water-based, which is a common solvent. In this case, we can assume a typical concentration of urea in water.
For example, if we assume a 1 molal solution, then the molality (m) would be 1 mol/kg.
Now, let's calculate the boiling point elevation (ΔTb) using the equation:
ΔTb = Kb * m
The molal boiling point elevation constant (Kb) for water is approximately 0.512 °C/m.
If we assume a molality (m) of 1 mol/kg, then:
ΔTb = 0.512 °C/m * 1 mol/kg
ΔTb = 0.512 °C
To find the boiling point of the solution, we add the boiling point elevation (ΔTb) to the boiling point of pure water (100 °C):
Boiling point of solution = 100 °C + 0.512 °C
Boiling point of solution = 100.512 °C
Therefore, assuming a molality of 1 mol/kg, the boiling point of the urea solution would be approximately 100.512 °C.
ΔTb = Kb * m
Where:
ΔTb = boiling point elevation
Kb = molal boiling point elevation constant
m = molality of the solution
First, we need to calculate the molality (m) of the solution. Molality is defined as the number of moles of solute per kilogram of solvent.
Given that the molecular mass of urea is 56 g/mol, we need to convert the mass of urea to moles:
Mass of urea = 56 g/mol
Now, we need to calculate the molality (m):
m = moles of solute / mass of solvent (in kg)
Since the solvent is not specified, we cannot calculate the exact molality without additional information. However, we can assume that the solution is water-based, which is a common solvent. In this case, we can assume a typical concentration of urea in water.
For example, if we assume a 1 molal solution, then the molality (m) would be 1 mol/kg.
Now, let's calculate the boiling point elevation (ΔTb) using the equation:
ΔTb = Kb * m
The molal boiling point elevation constant (Kb) for water is approximately 0.512 °C/m.
If we assume a molality (m) of 1 mol/kg, then:
ΔTb = 0.512 °C/m * 1 mol/kg
ΔTb = 0.512 °C
To find the boiling point of the solution, we add the boiling point elevation (ΔTb) to the boiling point of pure water (100 °C):
Boiling point of solution = 100 °C + 0.512 °C
Boiling point of solution = 100.512 °C
Therefore, assuming a molality of 1 mol/kg, the boiling point of the urea solution would be approximately 100.512 °C.
|
Explore Courses for NEET exam
|
|
Top Courses for NEETView all
Question Description
A solution of urea (mol. mass 56 g mol-l) boils at 100.18°C at the atmospheric pressureIf Kfand Kbfor water are 1.86 and 0.52 K kg mol-1respectively, the above solution will freeze ata)-6.54°Cb)654°Cc)0.654°Cd)-0.654TCorrect answer is option 'D'. Can you explain this answer? for NEET 2025 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about A solution of urea (mol. mass 56 g mol-l) boils at 100.18°C at the atmospheric pressureIf Kfand Kbfor water are 1.86 and 0.52 K kg mol-1respectively, the above solution will freeze ata)-6.54°Cb)654°Cc)0.654°Cd)-0.654TCorrect answer is option 'D'. Can you explain this answer? covers all topics & solutions for NEET 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for A solution of urea (mol. mass 56 g mol-l) boils at 100.18°C at the atmospheric pressureIf Kfand Kbfor water are 1.86 and 0.52 K kg mol-1respectively, the above solution will freeze ata)-6.54°Cb)654°Cc)0.654°Cd)-0.654TCorrect answer is option 'D'. Can you explain this answer?.
A solution of urea (mol. mass 56 g mol-l) boils at 100.18°C at the atmospheric pressureIf Kfand Kbfor water are 1.86 and 0.52 K kg mol-1respectively, the above solution will freeze ata)-6.54°Cb)654°Cc)0.654°Cd)-0.654TCorrect answer is option 'D'. Can you explain this answer? for NEET 2025 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about A solution of urea (mol. mass 56 g mol-l) boils at 100.18°C at the atmospheric pressureIf Kfand Kbfor water are 1.86 and 0.52 K kg mol-1respectively, the above solution will freeze ata)-6.54°Cb)654°Cc)0.654°Cd)-0.654TCorrect answer is option 'D'. Can you explain this answer? covers all topics & solutions for NEET 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for A solution of urea (mol. mass 56 g mol-l) boils at 100.18°C at the atmospheric pressureIf Kfand Kbfor water are 1.86 and 0.52 K kg mol-1respectively, the above solution will freeze ata)-6.54°Cb)654°Cc)0.654°Cd)-0.654TCorrect answer is option 'D'. Can you explain this answer?.
Solutions for A solution of urea (mol. mass 56 g mol-l) boils at 100.18°C at the atmospheric pressureIf Kfand Kbfor water are 1.86 and 0.52 K kg mol-1respectively, the above solution will freeze ata)-6.54°Cb)654°Cc)0.654°Cd)-0.654TCorrect answer is option 'D'. Can you explain this answer? in English & in Hindi are available as part of our courses for NEET.
Download more important topics, notes, lectures and mock test series for NEET Exam by signing up for free.
Here you can find the meaning of A solution of urea (mol. mass 56 g mol-l) boils at 100.18°C at the atmospheric pressureIf Kfand Kbfor water are 1.86 and 0.52 K kg mol-1respectively, the above solution will freeze ata)-6.54°Cb)654°Cc)0.654°Cd)-0.654TCorrect answer is option 'D'. Can you explain this answer? defined & explained in the simplest way possible. Besides giving the explanation of
A solution of urea (mol. mass 56 g mol-l) boils at 100.18°C at the atmospheric pressureIf Kfand Kbfor water are 1.86 and 0.52 K kg mol-1respectively, the above solution will freeze ata)-6.54°Cb)654°Cc)0.654°Cd)-0.654TCorrect answer is option 'D'. Can you explain this answer?, a detailed solution for A solution of urea (mol. mass 56 g mol-l) boils at 100.18°C at the atmospheric pressureIf Kfand Kbfor water are 1.86 and 0.52 K kg mol-1respectively, the above solution will freeze ata)-6.54°Cb)654°Cc)0.654°Cd)-0.654TCorrect answer is option 'D'. Can you explain this answer? has been provided alongside types of A solution of urea (mol. mass 56 g mol-l) boils at 100.18°C at the atmospheric pressureIf Kfand Kbfor water are 1.86 and 0.52 K kg mol-1respectively, the above solution will freeze ata)-6.54°Cb)654°Cc)0.654°Cd)-0.654TCorrect answer is option 'D'. Can you explain this answer? theory, EduRev gives you an
ample number of questions to practice A solution of urea (mol. mass 56 g mol-l) boils at 100.18°C at the atmospheric pressureIf Kfand Kbfor water are 1.86 and 0.52 K kg mol-1respectively, the above solution will freeze ata)-6.54°Cb)654°Cc)0.654°Cd)-0.654TCorrect answer is option 'D'. Can you explain this answer? tests, examples and also practice NEET tests.
|
|
Explore Courses for NEET exam
|
|
Signup for Free!
Signup to see your scores go up within 7 days! Learn & Practice with 1000+ FREE Notes, Videos & Tests.
|
© EduRev
|
Education Revolution
|
|
Signup on EduRev and stay on top of your study goals
10M+ students crushing their study goals daily