I need help solving this question.. An aqueous solution of ethylene glycol (C2H6O2) IS 40% ethylene glycol by mass, and has a density of 1.05g/ml. what are the molarity, molality fraction of the solution?

A gas occupies 10 liters at standard conditions. what volume will it occupy at 20 C and 700 torr?

I don't know what you mean by molality fraction.

mass of 1,000 mL = 1.05 g/mL x 1000 = 1050 gram. That is 40% ethylene glycol; therefore,
1050 x 0.40 = 420 g ethylene glycol and 420 g is 420/molar mass ethylene glycol. That will give you moles/L which is M.

To find molality,
1050 grams soln - mass ethylene glycol (420 g) = 630 g water.
molality = moles/kg soln. Convert 420 to moles ethylene glycol and divide by 0.630 = ?? molal

For the gas problem use PV = nRT.

To find the molarity and molality fraction of the solution, we need to gather some information and use the appropriate formulas.

First, let's define the terms:

- Molarity (M): It is the amount of solute (in moles) divided by the volume of the solution (in liters). It is given by the formula: M = moles of solute / volume of solution (in liters).

- Molality (m): It is the amount of solute (in moles) divided by the mass of the solvent (in kilograms). It is given by the formula: m = moles of solute / mass of solvent (in kg).

- Mass fraction: It is the mass of the solute divided by the total mass of the solution.

Now, let's solve the problem step-by-step:

Step 1: Determine the mass of solute (ethylene glycol):
Since the aqueous solution is 40% ethylene glycol by mass, we can assume that 100g of the solution contains 40g of ethylene glycol.

Step 2: Determine the volume of the solution:
Given the density of the solution is 1.05g/ml, we can assume that the mass of 100ml (or 100g) of the solution is 100g.

Step 3: Convert the mass of solute to moles:
To convert the mass of solute (ethylene glycol) to moles, we need to know its molar mass. The molar mass of ethylene glycol (C2H6O2) can be calculated by adding up the atomic masses of the atoms in its chemical formula:
Molar Mass of C2H6O2 = (2 * Atomic Mass of C) + (6 * Atomic Mass of H) + (2 * Atomic Mass of O)

Step 4: Calculate the molarity:
Substitute the values into the formula:
Molarity (M) = moles of solute / volume of solution (in liters)
Volume of solution = 100ml = 100/1000 = 0.1L

Step 5: Calculate the molality fraction:
Molality (m) = moles of solute / mass of solvent (in kg)
The mass of the solvent can be calculated by subtracting the mass of the solute from the total mass of the solution.

Step 6: Calculate the mass fraction:
Mass Fraction = mass of solute / total mass of solution.

By following these steps, you should be able to calculate the molarity, molality fraction, and mass fraction of the given aqueous solution of ethylene glycol.