Question

1a.) Calculate the osmotic pressure of a solution that contains 95.0 g of the nonelectrolyte urea, CH₄N₂O, per 500 mL of solution at 25°C.

a.) 75.4 atm,

b.) 69.8 atm,

c.) 84.4 atm,

d.) 77.4 atm

1b.) Calculate the osmotic pressure of a 0.060M glucose solution at 27°C.

a.) 3.4 atm,

b.) 1.2 atm,

c.) 5.8 atm,

d.) 1.5 atm

PLEASE CIRCLE THE ANSWERS.

Answer 1

a)

Molar mass of CH4N2O = 1*MM(C) + 4*MM(H) + 2*MM(N) + 1*MM(O)

= 1*12.01 + 4*1.008 + 2*14.01 + 1*16.0

= 60.062 g/mol

mass of CH4N2O = 95.0 g

we have below equation to be used:

number of mol of CH4N2O,

n = mass of CH4N2O/molar mass of CH4N2O

=(95.0 g)/(60.062 g/mol)

= 1.582 mol

volume , V = 500 mL

= 0.5 L

we have below equation to be used:

Molarity,

M = number of mol / volume in L

= 1.582/0.5

= 3.163 M

T= 25.0 oC

= (25.0+273) K

= 298 K

we have below equation to be used:

P = C*R*T

P = 3.1633978222503414*0.0821*298.0

P =77.4 atm

Answer: d

b)

T= 27.0 oC

= (27.0+273) K

= 300 K

we have below equation to be used:

P = C*R*T

P = 0.06*0.0821*300.0

P =1.5 atm

Answer: d