Answer:
a) 0.046 mol/L
b) 0.016 mol
c) 271.58 g/mol
Explanation:
A nonelectrolyte solute is a solute that, when dissolved in a solvent, will not make the solution a conductor, and so the electricity will not pass through it. The osmotic pressure is a colligative property, and it's the pressure difference needed to stop the flow of a solution across a semipermeable membrane. It can be calculated by:
π = MRT
Where π is the osmotic pressure, M is the molarity of the solute (mol/L), R is the ideal gas constant, and T is the temperature (in K). For a pressure in torr, R = 62.3637 torr.L/(mol.K).
a) π = MRT , T = 25°C = 298 K
851 = M*62.3637*298
18584.3826M = 851
M = 0.046 mol/L
b) The number of moles of the solute (n) is the molar concentration (molarity) multiplied by the volume. So, for a solution of 345 mL = 0.345 L,
n = 0.046 * 0.345
n = 0.016 mol
c) The molar mass (MM) is the mass divided by the number of moles:
MM = 4.31/0.016
MM = 271.58 g/mol
Avogadro's number tells you how many atoms are in 1 mol of every element.
So,
1 mol : 6.022x10^23 atoms = 0.450 moles : x atoms
There are 2.7099x10^23 atoms in 0.450 moles
Answer:
V₂ = 1070 mL or 1.07 L
Solution:
Data Given;
P₁ = 1170 mmHg
V₁ = 915 mL
T₁ = 24 °C + 273 K = 297 K
P₂ = 842 mmHg
V₂ = ?
T₂ = - 23 °C + 273 K = 250 K
According to Ideal gas equation,
P₁ V₁ / T₁ = P₂ V₂ / T₂
Solving for V₂,
V₂ = P₁ V₁ T₂ / P₂ T₁
Putting Values,
V₂ = (1170 mmHg × 915 mL × 250 K) ÷ (842 mmHg × 297 K)
V₂ = 1070 mL or 1.07 L
