When 5.00 mol of benzene is vaporized at a constant pressure of 1.00 atm and at its normal boiling point of 80.1°C, 169.5 kJ are
absorbed and PΔV for the vaporization process is equal to 14.5 kJ.
What is the change of internal energy?
What is the change of enthalpy?
Is the change in entropy positive or negative for this process?
If the pressure would be only ½ atm, what are the changes of internal energy and enthalpy during vaporization (approximately)?
How much energy is absorbed?
Write the definition of the Gibbs Free Energy.
At the lower pressure, will the boiling point be higher or lower.
What is the change of internal energy?
What is the change of enthalpy?
Is the change in entropy positive or negative for this process?
If the pressure would be only ½ atm, what are the changes of internal energy and enthalpy during vaporization (approximately)?
How much energy is absorbed?
Write the definition of the Gibbs Free Energy.
At the lower pressure, will the boiling point be higher or lower.
1 answer:
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Answer : The molar mass of the solute would be low.
Explanation :
Formula used for depression in freezing point is:
where,
= change in freezing point
= freezing point of solution
= freezing point of water
i = Van't Hoff factor
= freezing point constant
m = molality
= mass of solute
= mass of solvent
= molar mass of solute
From the formula we conclude that, when the freezing point of the solution read incorrectly that is freezing point of the solution is lower than the true freezing point then this means that change in freezing point would be high and the molar mass of the solute would be low.
Hence, the molar mass of the solute would be low.