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xxMikexx [17]
3 years ago
13

What is the vapor pressure of an aqueous solution made up of 60.0g of urea (CH4N2O) in 180g of water? the vapor pressure of wate

r at this temperature is 0.038atm.
please answer truthfully and explain how you got this answer because i dont know and my head hurts.
also the choices are
0.020atm
0.0025atm
0.035atm
0.00055atm
Chemistry
1 answer:
djyliett [7]3 years ago
7 0
To get the answer you use the Law of Raoult.


Raoult's law states that the decrease of the vapor pressure of a liquid is proportional to the molar fraction of the solute.


ΔP = Pa * Xa


Here Pa = 0.038 atm


And Xa = N a / (Na + Nb), where Na is number of moles of A and Nb is number of moles of b


Na = mass of urea / molar mass of urea =  60 g / (molar mass of CH4N2O)


molar mass of CH4N2O = 12 g/mol + 4*1g/mol + 2*14 g/mol + 16 g/mol = 60 g/mol


Na = 60 g / 60 g/mol = 1 mol


Nb = mass of water / molar mass of water = 180g / 18g/mol = 10 mol


Xa = 1 mol / (10 mol + 1 mol) = 1/11 =0.09091


ΔP = Pb * Xa = 0.038 atm * 0.09091 =  0.0035 atm


Then, the final vapor pressure of water is Pb - ΔP = 0.038atm - 0.0035atm = 0.035 atm.


 Answer: 0.035 atm
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