What is the osmotic pressure at 20 c° of a solution made by dissolving 0.69 grams of sucrose, c12h22o11, in 100 ml of water?

The osmotic pressure is 0.4808 atm

Explanation:

Given:

Temperature =

Volume of sucrose = 0.69 grams

volume of water = 100 mL

To Find:

The osmotic pressure =?

Solution:

Step 1: lets find the number of moles in 0.69 grams of sucrose(

number of moles in 0.69 grams of sucrose =

=>

=>

=>0.002 moles

Step2 :Dividing  number of moles by the amount of litres in the solution

=>       [ 100 mL = 0.100L]

=> 0.02 M

Step 3: Converting the temperature to kelvin

=>20 +273

=>293 K

Step 4: Finding the value of osmotic pressure

where

M is the Molarity

R is gas constant

T is the temperature

Now substituting the values,

the mass of the cathode increases because ions from the solution get reduced to atoms and become part of the cathode.

explanation:

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