What is the temperature if the osmotic pressure of a solution is 2.07 atm, and t

Chemistry
Tutor: None Selected Time limit: 1 Day

What is the temperature if the osmotic pressure of a solution is 2.07 atm, and the solution is made by adding 128 grams of a protein of molar mass 2,805 g/mol to enough water to make 1500.0 ml of solution?

STEP BY STEP EXPLANATION PLEASE!!!!!

May 19th, 2015

Hello!

Here you're going to use pi=MRT

pi = osmotic pressure = 2.07atm

M = molar concentration of dissolved protein = mol/liter

M = 0.456mol/1.5L = 0.0304mol/L......see below how to find V and n

V = 1.5Liters

n = solve for, given the protein information

n = (1mol/2.805kg)*.128kg = .0456mol

R = 0.08206 (L*atm)/(K*mol)

pi = MRT....solve for T

T = pi/(MR)

T = (2.07)/(0.0304*.08206)

T=830K

Let me know if you have any questions :)

May 19th, 2015

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