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rosijanka [135]
3 years ago
14

5.00 g of an unknown compound was dissolved in 250.0 mL of water. The unknown compound was found to be a non-electrolyte and the

osmotic pressure of the solution was determined to 14.5 atm at 298 K. Calculate the molar mass of the unknown compound (in units of g/mol). R= 0.08206 (L atm)/(mol K)
Chemistry
1 answer:
Zielflug [23.3K]3 years ago
4 0

Answer:

This unknown compound has a molar mass of 33.74g/mole

Explanation:

<u>Step 1:</u> Given data

The formula for the osmotic pressure is:

π = MRT = 14.5 atm

⇒ with M = Concentration of the solution

⇒ with R = gas constant = 0.08206 L atm / mol K

⇒ with T = absolute temperature (in Kelvin) = 298K

<u>Step 2:</u> Calculate concentration

M = π/ RT

M = 14.5 / (0.08206 * 298)

M = 0.593 M this is 0.593 moles per L

<u>Step 3:</u> Calculate number of moles

Since the volume is only 0.250 L, the amount of moles is:

0.593 * 0.250 L = 0.1482 moles

<u>Step 4:</u> Calculate molar mass

The molar mass is : mass / moles

Molar mass of this unknown compund = 5g / 0.1482 moles = 33.74 g/mole

This unknown compound has a molar mass of 33.74g/ mole

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