You have 32.8 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 gas in container = 22.56 g

Explanation:

Molar mass of = 32 g/mol

So, 32.8 g of = moles of = 1.025 moles of

Let's assume both and inside container behaves ideally

So, for both of them, PV = nRT

Where, P is pressure, V is volume of container, n is number of moles, R is gas constant and T is temperature in kelvin scale

So,

As P, R and T are constant for both and therefore ratio for both and will also remain constant

As gas container has twice the volume of gas container therefore number of moles of gas inside container will be twice the number of moles of gas inside container

Number of moles of gas present inside container = 1.025 moles

So, Number of moles of gas present inside container = moles = 0.5125 moles

Molar mass of = 44.01 g/mol

So, mass of gas inside container = g = 22.56 g

pv=nrt

explanation:

5.6⋅10−^19  j

do you need the explaination?