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Answer:
The molecular weight of the unknown compound is 267.7 g/mol
Explanation:
Lowering vapor pressure → Colligative property where the vapor pressure of solution is lower than vapor pressure of pure solvent
ΔP = P° . Xm
0.526 atm - 0.501 atm = 0.025atm
0.025 atm = 0.526 atm . Xm
Xm = 0.025 atm / 0.526 atm → 0.0475 (mole fraction)
Mole fraction = Moles of solute / Total moles (solute + solvent)
0.0475 = Moles of solute / Moles of solute + Moles of solvent
We determine the moles of solvent → 116.2 g . 1mol / 58 g = 2 moles
0.0475 = Moles of solute / Moles of solute + 2
0.0475 moles of solute + 0.095 = Moles of solute
0.095 = Moles of solute - 0.0475 moles of solute
0.095 / 0.9525 = Moles of solute → 0.0997 moles
Molas mass = g/mol → 26.7 g / 0.0997 mol = 267.7 g/mol
The volume (in mL) of methylergonovine the nurse should draw up in the syringeis is 0.25 mL
<h3>What is density? </h3>
The density of a substance is simply defined as the mass of the subtance per unit volume of the substance. Mathematically, it can be expressed as
Density = mass / volume
With the concept of density, we can obtain the volume of methylergonovine. Details below
<h3>How to determine the volume </h3>
The following data were obtained from the question:
- Mass of methylergonovine = 0.2 mg
- Density of methylergonovine = 0.8 mg/mL
- Volume of methylergonovine =?
Density = mass / volume
Cross multiply
Density × volume = mass
Divide both sides by density
Volume = mass / density
Volume = 0.2 / 0.8
Volume of methylergonovine = 0.25 mL
Learn more about density:
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