To calculate the osmotic pressure, we can use the formula:

Π = nRT/V

where:
Π is the osmotic pressure,
n is the number of moles of the solute,
R is the ideal gas constant,
T is the temperature in Kelvin,
V is the volume in liters.

Given:
n = 0.100 M (Molarity is moles/liter, so this is also the number of moles in 1 liter),
R = 0.08206 L × atm × mol⁻¹ × K⁻¹,
T = 25°C = 298.15 K (converted from Celsius to Kelvin by adding 273.15),
V = 1 L (since we're considering a 1 liter solution).

Substituting these values into the formula gives:

Π = (0.100 mol) × (0.08206 L × atm × mol⁻¹ × K⁻¹) × (298.15 K) / 1 L

Solving this gives Π ≈ 2.45 atm. So, the osmotic pressure of the solution is approximately 2.45 atmospheres.

Question

To calculate the osmotic pressure, we can use the formula:

Π = nRT/V

where:
Π is the osmotic pressure,
n is the number of moles of the solute,
R is the ideal gas constant,
T is the temperature in Kelvin,
V is the volume in liters.

Given:
n = 0.100 M (Molarity is moles/liter, so this is also the number of moles in 1 liter),
R = 0.08206 L × atm × mol⁻¹ × K⁻¹,
T = 25°C = 298.15 K (converted from Celsius to Kelvin by adding 273.15),
V = 1 L (since we're considering a 1 liter solution).

Substituting these values into the formula gives:

Π = (0.100 mol) × (0.08206 L × atm × mol⁻¹ × K⁻¹) × (298.15 K) / 1 L

Solving this gives Π ≈ 2.45 atm. So, the osmotic pressure of the solution is approximately 2.45 atmospheres.

Knowee AI · Accepted Answer

To calculate the osmotic pressure, we can use the formula:

Π = nRT/V

where:
Π is the osmotic pressure,
n is the number of moles of the solute,
R is the ideal gas constant,
T is the temperature in Kelvin,
V is the volume in liters.

Given:
n = 0.100 M (Molarity is moles/liter, so this is also the number of moles in 1 liter),
R = 0.08206 L × atm × mol⁻¹ × K⁻¹,
T = 25°C = 298.15 K (converted from Celsius to Kelvin by adding 273.15),
V = 1 L (since we're considering a 1 liter solution).

Substituting these values into the formula gives:

Π = (0.100 mol) × (0.08206 L × atm × mol⁻¹ × K⁻¹) × (298.15 K) / 1 L

Solving this gives Π ≈ 2.45 atm. So, the osmotic pressure of the solution is approximately 2.45 atmospheres.

What is the osmotic pressure of a 0.100 M aqueous solution of urea at25oC?for pressure in atmospheres, R = 0.08206 L × atm × mol -1 × K-1 Question 9Select one:246 atm3.82 atm24.4 atm2.45 atm

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