Question

A sample of carbon dioxide (CO2) is in a 2500 mL container at 27°C. The pressure in the container is 2.4 atm. How many grams of carbon dioxide (CO2) are in the container?

a. 16.8 g
b. 24.0 g
c. 42.0 g
d. 60.0 g

Answer 1

To find the mass of carbon dioxide in the container, use the ideal gas law equation PV = nRT. Rearrange the equation, convert the given values to appropriate units, and solve for the number of moles. Then, multiply the moles by the molar mass of CO2 to find the mass.

Step-by-step explanation:

To find the mass of carbon dioxide (CO2) in the container, we can use the ideal gas law equation: PV = nRT. Rearranging the equation to solve for the number of moles, n, we get n = PV/RT.

First, convert the given temperature to Kelvin by adding 273.15: 27°C + 273.15 = 300.15 K. Next, convert the given pressure to atm by dividing by 1.01325: 2.4 atm / 1.01325 = 2.3702 atm.

Now, we can substitute the values into the equation:

n = (2.3702 atm)(2.500 L)/(0.0821 L·atm/mol·K)(300.15 K) = 0.2288 mol. Finally, multiply the number of moles by the molar mass of CO2 (44.01 g/mol) to find the mass of carbon dioxide:

mass = (0.2288 mol)(44.01 g/mol) = 10.0677 g.