You have 30.4 g of O2 gas in a container with twice the volume as one with CO2 gas. The pressure and temperature of both containers are the same. Calculate the mass of carbon dioxide gas you have in the container.

mass of CO2 = 20.9 g

Explanation:

Given that:

mass of O2= 30.4 g

molar mass O2 = 32

number of moles of O2 = 30.4 / 32

number of moles of O2 = 0.95 moles

The Volume of O2 = 2V

Using ideal gas equation:

PV = nRT

P × (2V) = 0.95 × R × T

PV = 0.475 RT  ----- (1)

For CO2;

The volume = V

Using ideal gas equation:

PV = nRT ---- (2)

Equating equation (1) and (2) together, we get:

0.475 RT = nRT

Dividing both sides by RT

(0.475 RT)/RT = (nRT)/RT

0.475 = n

Thus, the number of moles of CO2 = 0.475

Since mass = number of moles × molar mass

mass of CO2 = 0.475 × 44

mass of CO2 = 20.9 g