A dilute aqueous solution of an organic compound soluble in water is formed by dissolving 2.35 g of the compound in water to form 0.250 L solution. The resulting solution has an osmotic pressure of 0.605 atm at 25 Celsius.

Question

A dilute aqueous solution of an organic compound soluble in water is formed by dissolving 2.35 g of the compound in water to form 0.250 L solution. The resulting solution has an osmotic pressure of 0.605 atm at 25 Celsius.

Assuming that the organic compound is a nonelectrolyte, what is its molar mass?

Please explain in depth all steps. I am very confused.

Answer 1

GIve me the solution

Answer 2

To find the molar mass of the organic compound, we need to use the formula relating osmotic pressure, molarity, and gas constant:

π = MRT

Where:
π is the osmotic pressure,
M is the molarity,
R is the gas constant (0.0821 L·atm/(mol·K)),
T is the temperature in Kelvin.

Step 1: Convert the temperature from Celsius to Kelvin.
The given temperature is 25 Celsius. To convert it to Kelvin, add 273.15.

T = 25 + 273.15 = 298.15 K

Step 2: Calculate the molarity of the solution.
Molarity is the number of moles of solute in one liter of solution.

We are given:
Mass of the compound = 2.35 g
Volume of the solution = 0.250 L

Molarity (M) = moles of solute / volume of solution (L)

First, we need to calculate the number of moles of the compound.
To do that, we use the formula:

moles = mass / molar mass

Step 3: Determine the number of moles.
We need the molar mass of the compound to find the number of moles.
Assuming the compound is a nonelectrolyte, it will be equal to the molar mass of the compound.

Let's say the molar mass of the compound is M.

moles = mass / molar mass
moles = 2.35 g / M

Step 4: Substitute the given values into the molarity equation.
Molarity (M) = moles / volume (L)
Molarity (M) = (2.35 g / M) / 0.250 L

Now we can substitute this expression for molarity (M) into the osmotic pressure formula.

π = MRT
0.605 atm = [(2.35 g / M) / 0.250 L] * (0.0821 L·atm/(mol·K)) * (298.15 K)

Step 5: Solve the equation for the molar mass (M).
Rearrange the equation to solve for M:

M = (2.35 g / (0.250 L * 0.0821 L·atm/(mol·K) * 298.15 K)) / 0.605 atm

Now we can plug in the values and calculate the molar mass.

Answer 3

To find the molar mass of the organic compound, we need to use the equation for osmotic pressure:

π = MRT

Where:
π is the osmotic pressure,
M is the molarity (mol/L),
R is the ideal gas constant (0.0821 L.atm/mol.K),
T is the temperature in Kelvin.

We are given:
π = 0.605 atm
T = 25°C = 298 K
V = 0.250 L

First, we need to calculate the molarity of the solution using the given mass of the compound and the volume of the solution:

M = moles of solute / volume of solution

The number of moles can be found using the formula:

moles of solute = mass of solute / molar mass

In this case, we are given the mass of the solute as 2.35 g.

Now, let's calculate the molarity:

M = (2.35 g / molar mass) / 0.250 L

Next, we can substitute the values we know into the osmotic pressure equation to solve for the molar mass:

0.605 atm = (2.35 g / molar mass) / 0.250 L * 0.0821 L.atm/mol.K * 298 K

Simplifying the equation:

0.605 atm * 0.0821 L.atm/mol.K * 298 K = 2.35 g / molar mass

(0.605 * 0.0821 * 298) = 2.35 g / molar mass

Using this equation, we can solve for the molar mass of the compound:

molar mass = 2.35 g / (0.605 * 0.0821 * 298)

molar mass ≈ 99.5814 g/mol

Therefore, the molar mass of the organic compound is approximately 99.5814 g/mol.

Answer 4

pi = MRT

You know pi, R, T. Solve for M = moles/L
You now know M and L, solve for moles.
Then moles = grams/molar mass. You know moles and grams, solve fo molar mass.