Problem: What mass of ethylene glycol (assume non-volatile), when mixed with 225 g H2O, will reduce the equilibrium vapor pressure of H2O from 1.00 atm to 0.800 atm at 100 °C? The molar masses of water and ethylene glycol are 18.02 g/mol and 62.07 g/mol, respectively. Assume ideal behavior for the solution.a. 275 gb. 89.1 gc. 194 gd. 106 ge. 134 g

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We’re being asked to determine the mass of ethylene glycol in water when the equilibrium vapor pressure is lowered to 0.80 atm from 1 atm


Recall that the vapor pressure of a solution can be given by Raoult’s Law:


Psolution = P°solventχsolvent


where P˚ = vapor pressure of solvent/water and χ = mole fraction of solvent. Mole fraction is given by:

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Problem Details

What mass of ethylene glycol (assume non-volatile), when mixed with 225 g H2O, will reduce the equilibrium vapor pressure of H2O from 1.00 atm to 0.800 atm at 100 °C? The molar masses of water and ethylene glycol are 18.02 g/mol and 62.07 g/mol, respectively. Assume ideal behavior for the solution.

a. 275 g

b. 89.1 g

c. 194 g

d. 106 g

e. 134 g

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