Respuesta :
The mole fraction is calculated using the formula:
mole fraction of component A = # of moles of component A / # of total moles of the solution.
A) number of moles of ethanol
To calculate the number of moles of ethanol, you need its density, which will permit you to determine the mass of the 10.00 ml, and then convert into moles using the molar mass of ethanol.
The normal density of ethanol is 0.789 g/ml
density = mass / volume => mass = density * volume = 0.789 g/ml * 10.00 ml = 7.890 g
Molar mass of ethanol = 46.07 g/mol
number of moles = mass / molar mass = 7.890g / 46.07 g/mol = 0.1713 mol
B) number of moles of water
density of water = 1.00 g/mol
mass of water = density * volume = 1.00 g/mol * 2.00 ml = 2.00 g
number of moles of water = mass / molar mass = 2.00 g / 18.0 g/mol = 0.111 mol
C) mole fraction
mole fraction of ethanol = number of moles of ethanol / number of moles of solution
number of moles of ethanol = 0.1713 / (0.1713 + 0.111) = 0.1713 / 0.2824 = 0.607
Answer: 0.607
The volume of the final solution may be calculated by adding the volume of the two components. This is 10.00 ml of ethanol + 2.00 ml of water makes 12.00 ml of solution.
It is not clear what the second question is meant for. Some context is missing. If you know density and you know maqss (or can calculate the mass from other data) you do not need to measure the volume.
mole fraction of component A = # of moles of component A / # of total moles of the solution.
A) number of moles of ethanol
To calculate the number of moles of ethanol, you need its density, which will permit you to determine the mass of the 10.00 ml, and then convert into moles using the molar mass of ethanol.
The normal density of ethanol is 0.789 g/ml
density = mass / volume => mass = density * volume = 0.789 g/ml * 10.00 ml = 7.890 g
Molar mass of ethanol = 46.07 g/mol
number of moles = mass / molar mass = 7.890g / 46.07 g/mol = 0.1713 mol
B) number of moles of water
density of water = 1.00 g/mol
mass of water = density * volume = 1.00 g/mol * 2.00 ml = 2.00 g
number of moles of water = mass / molar mass = 2.00 g / 18.0 g/mol = 0.111 mol
C) mole fraction
mole fraction of ethanol = number of moles of ethanol / number of moles of solution
number of moles of ethanol = 0.1713 / (0.1713 + 0.111) = 0.1713 / 0.2824 = 0.607
Answer: 0.607
The volume of the final solution may be calculated by adding the volume of the two components. This is 10.00 ml of ethanol + 2.00 ml of water makes 12.00 ml of solution.
It is not clear what the second question is meant for. Some context is missing. If you know density and you know maqss (or can calculate the mass from other data) you do not need to measure the volume.
The mole fraction of ethanol in the solution is 0.599.
Moles of solute : Ethanol :
Density = [tex]\rm \dfrac{mass}{volume}[/tex]
density of ethanol = 0.789 g/ml
mass of Ethanol = Density [tex]\times[/tex] Volume
mass of Ethanol =0.789 [tex]\times[/tex] 10
mass of Ethanol = 7.89 grams
[tex]\rm Moles\;of\;Ethanol\;=\;\dfrac{weight}{molecular\;weight}[/tex]
[tex]\rm Moles\;of\;Ethanol\;=\;\dfrac{7.89}{46.07}[/tex]
Moles of Ethanol = 0.16 moles
Density of water = 0.97 g/ml
Mass of Water = 0.97 [tex]\times[/tex] 2 g
Mass of Water = 1.94 grams.
[tex]\rm Moles\;of\;Water\;=\;\dfrac{1.94}{18.0153}[/tex]
Moles of water = 0.107 moles
Total moles of solution = Moles of Ethanol + moles of water
Total moles of solution = 0.16 + 0.107
Total moles of solution = 0.267 moles.
Mole fraction of ethanol :
= [tex]\rm \dfrac{0.16}{0.267}[/tex]
= 0.599 .
The mole fraction of ethanol in the solution is 0.599.
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