Respuesta :
Explanation:
As we know that density is the amount of mass present in a liter of solution.
Mathematically, density = [tex]\frac{mass}{volume}[/tex]
As it is given that density of water is 1 g/ml and volume is 175 mL. So, mass of water will be calculated as follows.
density = [tex]\frac{mass}{volume}[/tex]
1 g/ml = [tex]\frac{mass}{175 ml}[/tex]
mass = 175 g
It is known that 18 g of water contains 1 mole of water. Hence, number of moles present in 175 g of water will be calculated as follows.
No. of moles = [tex]\frac{mass}{\text{molar mass}}[/tex]
= [tex]\frac{175 g}{18 g/mol}[/tex]
= 9.72 mol
This means that we have 9.72 moles of ethanol also.
Hence, volume of ethanol present in 175 ml of water will be as follows.
No. of moles of ethanol = [tex]\frac{density \times Volume}{\text{molar mass of ethanol}}[/tex]
9.72 mol = [tex]\frac{0.789 g/ml \times Volume}{46 g/mol}[/tex]
Volume = 566.69 ml
Thus, we can conclude that 566.69 ml volume of ethanol contains the same number of molecules as are present in 175 ml of [tex]H_{2}O[/tex].
Answer: 566.7 ml
Explanation:-
[tex]Density=\frac{mass}{Volume}[/tex]
Density of the water= [tex]1g/ml[/tex]
volume of water = 175 ml
Putting in the values we get:
[tex]1g/ml=\frac{mass}{175ml}[/tex]
mass of water = 175 g
According to avogadro's law, 1 mole of every substance occupies 22.4 L at STP and contains avogadro's number [tex]6.023\times 10^{23}[/tex] of particles.
tex]\text{Number of moles of water}=\frac{175g}{18g/mol}=9.72moles[/tex]
Thus 9.72 moles of ethanol are required.
Mass of ethanol=[tex]moles\times {\text {Molar mass}}=9.72\times 46=447.12g[/tex]
[tex]Density=\frac{mass}{Volume}[/tex]
Density of ethanol= [tex]0.789g/ml[/tex]
volume of ethanol= ?
Putting in the values we get:
[tex]0.789g/ml=\frac{447.12g}{Volume}[/tex]
[tex]Volume=566.7ml[/tex]
Thus volume of ethanol that contains the same number of molecules as are present in 175 ml of water is 566.7 ml.
