Questions: A chemistry student needs 25.0 g of ethanolamine for an experiment. By consulting the CRC Handbook of Chemistry and Physics, the student discovers that the density of ethanolamine is 1.02 g/cm^(-3). Calculate the volume of ethanolamine the student should pour out.

A chemistry student needs 25.0 g of ethanolamine for an experiment. By consulting the CRC Handbook of Chemistry and Physics, the student discovers that the density of ethanolamine is 1.02 g/cm^(-3). Calculate the volume of ethanolamine the student should pour out.

Transcript text: A chemistry student needs 25.0 g of ethanolamine for an experiment. By consulting the CRC Handbook of Chemistry and Physics, the student discovers that the density of ethanolamine is $1.02 \mathrm{~g} \cdot \mathrm{~cm}^{-3}$. Calculate the volume of ethanolamine the student should pour out. Be sure your answer has the correct number of significant digits.

Solution

Solution Steps

Step 1: Identify Given Values

Mass of ethanolamine: $ 25.0 \, \text{g} $
Density of ethanolamine: $ 1.02 \, \text{g/cm}^3 $

Step 2: Use the Density Formula

The formula to find volume using density is: \[ \text{Density} = \frac{\text{Mass}}{\text{Volume}} \] Rearrange to solve for volume: \[ \text{Volume} = \frac{\text{Mass}}{\text{Density}} \]

Step 3: Substitute the Given Values

Substitute the given mass and density into the formula: \[ \text{Volume} = \frac{25.0 \, \text{g}}{1.02 \, \text{g/cm}^3} \]

Step 4: Calculate the Volume

Perform the division to find the volume: \[ \text{Volume} = 24.5098 \, \text{cm}^3 \]

Step 5: Round to Correct Significant Digits

The given values have 3 significant digits, so round the volume to 3 significant digits: \[ \text{Volume} = 24.5 \, \text{cm}^3 \]