You have 41.6 g of o2 gas in a container with twice the volume as one with co2 gas in another container. the pressure and temperature of both containers are the same. calculate the mass of carbon dioxide gas you have in the container.

The mass of carbon dioxide is 28.6 grams

Explanation:

Step 1: Data given

Mass of O2 = 41.6 grams

Volume of the O2 container = 2V

Volume of the CO2 container = V

Pressure and temperature are the same

Step 2: Ideal gas law

The ideal gas law = p*V=nRT

For O2: p*2V = n(O2)*R*T

For CO2: p*V = n(CO2)*R*T

n(O2)*R*T / P*2V = n(CO2)*R*T / P*V

Since P, R and T are contstant, we can simplify this to:

n(O2)/2 = n(CO2)

Step 3:  Calculate moles of O2

Moles O2 = mass O2/ Molar mass O2

Moles O2 = 41.6 grams / 32 g/mol

Moles O2 = 1.3 mol O2

The number of moles CO2 = 0.65 mol

Mass of CO2 = Moles CO2 * Molar Mass CO2

Mass of CO2 = 0.65 mol * 44.01 g/mol

Mass of CO2 = 28.6 grams

The mass of carbon dioxide is 28.6 grams

i believe you are right for all except the 3rd ( look at sqdancefan his answer is much better)

what is the question?