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

i dont know

explanation:

we can conclude that the melting point of table salt is above room temperature (it's actually 801 deg c). the melting point of mercury must be below room temperature (- 39 deg c).