Chemistry, 27.08.2019 16:20 TheSmartRey

Asolution of 62.4 g of insulin in enough water to make 1.000 l of solution has an osmotic pressure of 0.305 atm at 25°c. based on these data, what is the molar mass of insulin?

Answers

Answer from: ameliaparry123p2eupk

Molecular Mass of insulin = 5004

Explanation:

Mass of insulin = 62.4 g

Volume of the solution = 1.00 L

Osmotic pressure = 0.305 L

Temperature = 25 °C = 25 + 273 = 298 K

PV = nRT

Where,

P = osmotic pressure

V = Volume of the solution

n = No. of moles

R gas constant = 0.08206 L atm K^{-1} Mol^{-1}

T = Temperature

PV = nRT

$n=\frac{PV}{RT}$

$n=\frac{(0.305 atm)(1.00 L)}{(0.08206 L atm K^{-1} Mol^{-1})(298 K)}$

n = 0.01247

No. of mol = Mass in g/molecular mass

Molecular mass = Mass in g/No. of mol

Molecular mass = 62.4/0.01247

= 5004

Answer from: Quest

i think the answer is terrae but not 100 percent sure. ▓▬▬ §

Answer from: Quest

the answer is na (sodium)

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Asolution of 62.4 g of insulin in enough water to make 1.000 l of solution has an osmotic pressure o...