Carbon dioxide (CO2) is a gas at room temperature and pressure. However, carbon dioxide can be put under pressure to become a "supercritical fluid" that is a much safer dry-cleaning agent than tetrachloroethylene. At a certain pressure, the density of supercritical CO2 is 0.469 g/cm3 . What is the mass of a 25.0-mL sample of supercritical CO2 at this pressure?
mass = volume x density
You know density and volume, solve for mass.
To determine the mass of a 25.0-mL sample of supercritical CO2 at the given pressure, we need to use the density of the supercritical CO2.
Density is defined as mass divided by volume. Therefore, we can rearrange the equation to solve for mass:
Mass = Density × Volume
First, we need to convert the volume from mL to cm3, since the density is given in g/cm3.
1 mL = 1 cm3
So, the volume of the sample is already in cm3. We can directly substitute it into the equation.
Mass = 0.469 g/cm3 × 25.0 cm3
Now we can calculate the mass:
Mass = 11.725 g
Therefore, the mass of a 25.0-mL sample of supercritical CO2 at the given pressure is 11.725 grams.