The osmotic pressure of a decimolar solution of urea at $27^{0} C$ is:

2.49

bar

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5

bar

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3.4

bar

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1.25

bar

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Solution

The correct option is A $2.49$ bar
Molarity, $M = \frac{1}{10} M$

$= 0.1 M$

$T = 300 K$

$π = M R T$

$= 0.1 \times 0.0821 \times 300$

$π = 2.463 a t m$

and we know $1 a t m = 1.01325 b a r$

so $π = 2.463 \times 1.01325$

$= 2.49 b a r$

Hence, the correct option is $A$

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The osmotic pressure of a decimolar solution of urea at 270C is:

The correct option is A 2.49 barMolarity, M=110M =0.1M T=300Kπ=MRT=0.1×0.0821×300π=2.463 atmand we know 1 atm=1.01325 barso π=2.463×1.01325=2.49 barHence, the correct option is A

The osmotic pressure of a decimolar solution of urea at $27^{0} C$ is:

The correct option is A $2.49$ bar
Molarity, $M = \frac{1}{10} M$

$= 0.1 M$

$T = 300 K$

$π = M R T$

$= 0.1 \times 0.0821 \times 300$

$π = 2.463 a t m$

and we know $1 a t m = 1.01325 b a r$

so $π = 2.463 \times 1.01325$

$= 2.49 b a r$

Hence, the correct option is $A$