If 22.9 g of solid carbon dioxide was placed in a similar container already containing air at 720. torr, what would be the partial pressure of carbon dioxide and the total pressure in the container after the carbon dioxide had vaporized?

ppCO2 = 1.51 atm

total pressure = 3atm

Explanation:

The reaction involved is C + O2 = CO2

I need the number of moles to be able to calculate the partial pressure of CO2 with the general equation of gases.

n = 22.9gCO2 * (1molCO2 / 44gCO2) =0.52mol

T = 20 ° + 273.15K = 293.15K

V = 22.4L

p = nRT / V = (0.52mol * (0.082 atm * L / K * mol) * 293.15K) /22.4L

ppCO2 = 0.56 atm

ppaire = 720torr * (1 atm / 760torr) = 0.95atm

total pressure = ppCO2 + ppaire = 0.56 + 0.95

total pressure =1.51atm

answer: the primary difference between a hypothesis and a theory is that b hypothesis is falsifiable, but a theory has been proven to be correct. theory is an explanation of something that is happening but hypothesis is a guess of something that can happen

explanation:

elements make up everything, and they combine to make compounds.

the answer is c