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KiRa [710]
3 years ago
7

if you make a solution by dissolving 1.0 mol of Fecl3 into 1 kg of water how would the osmotic pressure of this solution compare

with the osmotic pressure of a solution that is made from 1.0 mol of glucose in 1 kg of water
Chemistry
2 answers:
zubka84 [21]3 years ago
5 0
The osmotic pressure is greater in the FeCl3 solution. The FeCl3 is an ionic compound, so it dissociates into Fe3+ and 3Cl-, creating 4 overall particles, while the glucose remains as 1 particle. The water increases in the FeCl3 to compensate for that added particle concentration. 
IceJOKER [234]3 years ago
4 0

Explanation:

Osmotic pressure is defined as the minimum pressure which has to applied on the solution to prevent the entry of the solvent in the solution through a semi-permeable membrane.

It is a type of colligative property which means it depends on the amount of the solution. More the amount, more will be the osmotic pressure.

Mathematically,

\pi =icRT

\pi = Osmotic pressure

i = Vant's Hoff factor which is 1 for non-electrolyte solutions

c = Concentration of solution

R = Solution constant

T = temperature

  • For FeCl_3

As Ferric chloride is an electrolyte, so it will completely dissociate into its ions.

1 mole of ferric chloride will dissociate into 1 Fe^{3+} ion and 3 Cl^- ions.

FeCl_3\rightarrow Fe^{3+}+3Cl^-

Here, value of i = 4

  • For Glucose

Glucose is a non-electrolyte and hence will not dissociate into the respective ions. So, value of i = 1

Osmotic pressure will be high for high value of 'i'. Therefore, osmotic pressure of FeCl_3 will be high as compared to the glucose in same amount of water.

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2. A sample of neon gas has a volume of 87.6 L at STP. How many moles are present?
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Answer:

                      3.91 moles of Neon

Explanation:

According to Avogadro's Law, same volume of any gas at standard temperature (273.15 K or O °C) and pressure (1 atm) will occupy same volume. And one mole of any Ideal gas occupies 22.4 dm³ (1 dm³ = 1 L).

Data Given:

                 n = moles = <u>???</u>

                 V = Volume = 87.6 L

Solution:

               As 22.4 L volume is occupied by one mole of gas then the 16.8 L of this gas will contain....

                          = ( 1 mole × 87.6 L) ÷ 22.4 L

                          = 3.91 moles

<h3>2nd Method:</h3>

                     Assuming that the gas is acting ideally, hence, applying ideal gas equation.

                              P V  =  n R T      ∴  R  =  0.08205 L⋅atm⋅K⁻¹⋅mol⁻¹

Solving for n,

                              n  =  P V / R T

Putting values,

                              n  =  (1 atm × 87.6 L)/(0.08205 L⋅atm⋅K⁻¹⋅mol⁻¹ × 273.15K)

                              n  =  3.91 moles

Result:

          87.6 L of Neon gas will contain 3.91 moles at standard temperature and pressure.

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P . V = n . R . T

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760 Torr are 1 atm

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Mass / Molar mass = Moles → That's why the 1.06 g / MM

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1.06g/0.0195 mol = MM →  54.3 g/m

Now, let's use the composition

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