The osmotic pressure of solution containing 4 g of the solute per litre of the solution is 0.41 atm at 27. What is the molecular weight of the solute?
pressure=MRT
convert temps to kelvins
M=4/MW
R= .0826 mol-atm-L/kelvin
https://www.chem.purdue.edu/gchelp/howtosolveit/Solutions/osmoticpressure.html
Muhammad
The answer
Please answer the question i ask
To calculate the molecular weight of the solute, we need to use the formula for osmotic pressure.
The formula for osmotic pressure (π) is given by:
π = MRT
where:
π = osmotic pressure
M = molar concentration of the solute
R = ideal gas constant (0.0821 L·atm·K^-1·mol^-1)
T = temperature in Kelvin (K)
In this case, we are given the osmotic pressure (0.41 atm), the molar concentration of the solute (4 g/L), and the temperature (27°C). We need to convert the temperature to Kelvin.
To convert the temperature from Celsius to Kelvin, we use the formula:
T(K) = T(°C) + 273.15
T(K) = 27 + 273.15 = 300.15 K
Now we can substitute the values into the osmotic pressure formula:
0.41 atm = (4 g/L) (RT)
Since we want to find the molecular weight (M), we rearrange the formula:
M = (0.41 atm) / [(4 g/L) (RT)]
Now let's substitute the known values:
R = 0.0821 L·atm·K^-1·mol^-1
T = 300.15 K
M = (0.41 atm) / [(4 g/L) (0.0821 L·atm·K^-1·mol^-1) (300.15 K)]
Now, calculate the molecular weight:
M ≈ (0.41 / (4 * 0.0821 * 300.15))
M ≈ (0.41 / 9.936) ≈ 0.04132 mol/L
Therefore, the molecular weight of the solute is approximately 0.04132 g/mol.