The nonvolatile, nonelectrolyte DDT, C14H9Cl5 (354.50 g/mol), is soluble in diethyl ether CH3CH2OCH2CH3. Calculate the osmotic pressure generated when 10.4 grams of DDT are dissolved in 286 ml of a diethyl ether solution at 298 K. The molarity of the solution is M. The osmotic pressure of the solution is atmospheres.

2.50 atm

Explanation:

We have 10.4 g of DDT (solute), whose molar mass is 354.50 g/mol. The corresponding moles are:

10.4 g × (1 mol/354.50 g) = 0.0293 mol

The molarity of the solution is:

M = moles of solute / liters of solution

M = 0.0293 mol / 0.286 L

M = 0.102 M

We can find the osmotic pressure (π) using the following pressure.

π = M × R × T

where,

R: ideal gas constant

T: absolute temperature

π = M × R × T

π = 0.102 M × 0.0821 atm.L/mol.K × 298 K

π = 2.50 atm

c (diamond),

sio2 (quartz)

the answers would be

the first one and the second one