# What is the mass of a sample of CO2 if it is held at 24 degrees C, 0.544 atm in a 3.00L flask?

Nov 14, 2015

2.94g

#### Explanation:

Use the ideal gas law ($P V = n R T$).

Since the question asks for mass, if we find the number of moles of $C {O}_{2}$, we can multiply that by the molar mass to find the mass of the $C {O}_{2}$ gas.

If we want to solve for moles, $n = \frac{P V}{R T}$.

Plug in values: $n = \frac{0.544 \cdot 3.00}{0.08206 \cdot \left(24 + 273.15\right)}$

Remember, the temperature must be in Kelvin, not Celsius.

$n = 0.67$

$0.67 m o l$$C {O}_{2}$$\times \frac{44 g}{1 m o l} = \textcolor{b l u e}{2.94 g}$