Chemistry, asked by HMurmu301, 1 year ago

The relationship between osmotic pressure at 273 k when 10g glucose, 10g urea and 10g sucrose are dissolved in 250 ml of water is

Answers

Answered by BarrettArcher
65

Solution : Given,

Temperature = 273 K

Mass of glucose = 10g

Mass of urea = 10g

Mass of sucrose = 10g

Volume of solvent (water) = 250 ml

Molar mass of glucose = 180.156 g/mole

Molar mass of urea = 60.06 g/mole

Molar mass of sucrose = 342.296 g/mole

The formula used for osmotic pressure is,

\pi=\frac{w\times R\times T}{M\times V}

where,

\pi = osmotic pressure

w = given mass

R = gas constant

T = temperature

M = molar mass

V = volume of solvent

From the formula, we conclude that the Osmotic pressure is inversely proportional to the Molar mass, since other values are same for all three compounds.

\pi\propto \frac{1}{M}

Osmotic pressure of glucose, urea and sucrose is represented as \pi_1, \pi_2 and \pi_3 respectively.

This means that the lower the molar mass of the compound, the higher will be the osmotic pressure of compound.

So, the relationship between the osmotic pressure of glucose, urea and sucrose is,

\pi_2> \pi_1> \pi_3



Answered by sara200408
1

Explanation:

The osmotic pressure is inversely proportional to the molecular weight.

The increasing order of molecular weights is urea < glucose < sucrose.

Hence, the decreasing order of osmotic pressure is P

urea > glucose > sucrose.

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