choose the solvent below that would show the greatest boiling point elevation when used to make a 0.10m non electrolyte solution
a.C6H6, Kb= 5.12 degree C/m
b. CHCl3, Kb= 4.70 degree C/m
c.CCl4, Kb= 29.9degree C/m
d.CH3CH2OH, Kb= 1.99degree C/m
e.CH3CH2OCH2CH3, Kb=1.79degree C/m
delta T = Kb*m
So which will give the largest delta T?
Since m is the same it must depend on Kb?
5.66
To determine which solvent would show the greatest boiling point elevation when used to make a 0.10m non-electrolyte solution, we need to compare the boiling point elevation constants (Kb) for each solvent.
The boiling point elevation is directly proportional to the molality (m) of the solute, and the boiling point elevation constant (Kb) of the solvent. The greater the Kb value, the greater the boiling point elevation.
Comparing the Kb values:
a. C6H6, Kb= 5.12 degree C/m
b. CHCl3, Kb= 4.70 degree C/m
c. CCl4, Kb= 29.9 degree C/m
d. CH3CH2OH, Kb= 1.99 degree C/m
e. CH3CH2OCH2CH3, Kb= 1.79 degree C/m
From the provided options, the solvent with the greatest boiling point elevation would be c. CCl4, which has a Kb value of 29.9 degree C/m.
To determine the solvent that would show the greatest boiling point elevation when used to make a 0.10m non-electrolyte solution, we need to compare the values of Kb (boiling point elevation constant) for the given solvents. The solute concentration is the same for all solvents (0.10m), so the boiling point elevation will depend solely on the Kb value.
The solvent with the highest Kb value will cause the greatest boiling point elevation. So, we need to compare the Kb values for each solvent:
a. C6H6, Kb = 5.12 degree C/m
b. CHCl3, Kb = 4.70 degree C/m
c. CCl4, Kb = 29.9 degree C/m
d. CH3CH2OH, Kb = 1.99 degree C/m
e. CH3CH2OCH2CH3, Kb = 1.79 degree C/m
Comparing the Kb values, we can see that CCl4 has the highest value of 29.9 degree C/m. Therefore, CCl4 would show the greatest boiling point elevation when used to make a 0.10m non-electrolyte solution.