what volume of glycerine C3H8O3, with a density of 1.26 g/mL should be taken to obtain 2.50 ml of glycerine?

Answer to this question

Given number of moles to be 2.5mol, we can use it and the molar mass of glycerine which is 92.11g/mol to determine it's mass. That is,

m=nMr
m=2.50mol*92.11g/mol
m=230g
Density is s ratio of the mass and the volume, so we use this relationship to find the volume to obtain 2.5mol,C3H8O3
V=m/D
V=230g/1.26g/ml
V=183ml

what volume of glycerine CHO with 1.26 must be taken to obtain 2.50 mole of glycerine

To calculate the volume of glycerine needed, we can use the given density and the desired volume.

Step 1: Convert the given density from grams per milliliter (g/mL) to grams per cubic centimeter (g/cm³).

Density of glycerine = 1.26 g/mL

Since 1 mL is equal to 1 cm³, the density remains the same.

Density of glycerine = 1.26 g/cm³

Step 2: Use the formula density = mass/volume to find the mass of glycerine required.

Density of glycerine = Mass/Volume

Rearranging the formula, we have:

Mass = Density × Volume

Volume = 2.50 mL (given)

Mass = 1.26 g/cm³ × 2.50 mL

Note: To ensure the units are consistent, it's important to convert 2.50 mL to cubic centimeters (cm³) since 1 mL = 1 cm³.

Step 3: Calculate the mass of glycerine:

Mass = 1.26 g/cm³ × 2.50 cm³

Mass = 3.15 grams

Therefore, the volume of glycerine needed to obtain 2.50 mL is 3.15 grams.