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6 grams of urea is dissolved in 16.2 grams of water at 25oC . What is the vapour pressure (in mm) of the resultant solution? The vapour of water at 25oC is 24 mm
- a)2.4
- b)21.6
- c)23.6
- d)18
Correct answer is option 'B'. Can you explain this answer?
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6 grams of urea is dissolved in 16.2 grams of water at 25oC . What is ...
Given:
Mass of urea (m1) = 6 g
Mass of water (m2) = 16.2 g
Temperature (T) = 25°C = 298 K
Vapour pressure of water (P°) = 24 mm
To find: Vapour pressure of the resultant solution
We can use Raoult’s law to calculate the vapour pressure of the solution:
P = P°X
Where P is the vapour pressure of the solution,
P° is the vapour pressure of the pure solvent, and
X is the mole fraction of the solvent in the solution.
First, we need to calculate the mole fraction of water in the solution:
Molar mass of urea (M1) = 60 g/mol
Molar mass of water (M2) = 18 g/mol
Number of moles of urea (n1) = m1/M1 = 6/60 = 0.1 mol
Number of moles of water (n2) = m2/M2 = 16.2/18 = 0.9 mol
Total number of moles in the solution (n) = n1 + n2 = 1 mol
Mole fraction of water (X2) = n2/n = 0.9/1 = 0.9
Now, we can calculate the vapour pressure of the solution:
P = P°X2 = 24 x 0.9 = 21.6 mm
Therefore, the vapour pressure of the resultant solution is 21.6 mm, which is option (b).
Mass of urea (m1) = 6 g
Mass of water (m2) = 16.2 g
Temperature (T) = 25°C = 298 K
Vapour pressure of water (P°) = 24 mm
To find: Vapour pressure of the resultant solution
We can use Raoult’s law to calculate the vapour pressure of the solution:
P = P°X
Where P is the vapour pressure of the solution,
P° is the vapour pressure of the pure solvent, and
X is the mole fraction of the solvent in the solution.
First, we need to calculate the mole fraction of water in the solution:
Molar mass of urea (M1) = 60 g/mol
Molar mass of water (M2) = 18 g/mol
Number of moles of urea (n1) = m1/M1 = 6/60 = 0.1 mol
Number of moles of water (n2) = m2/M2 = 16.2/18 = 0.9 mol
Total number of moles in the solution (n) = n1 + n2 = 1 mol
Mole fraction of water (X2) = n2/n = 0.9/1 = 0.9
Now, we can calculate the vapour pressure of the solution:
P = P°X2 = 24 x 0.9 = 21.6 mm
Therefore, the vapour pressure of the resultant solution is 21.6 mm, which is option (b).
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