Answer:
First question: P = 2.00 atm (1520 torr)
Second question: Partial pressure of carbon dioxide: 2.00 atm (1520 torr); total pressure: 2.97 atm (2260 torr).
Explanation:
The molar mass of caron dioxide, CO₂, is:
12 g/mol of C + 2*16 g/mol of O = 44 g/mol
The number of moles is the mass divided by the molar mass:
n = 7.8/44 = 0.1773 mol
By the ideal gas law:
PV = nRT
Where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant (0.082 atm*L/mol*K), and T is the temperature (278ºC + 273 = 551 K).
So, the pressure will be:
P*4 = 0.1773*0.082*551
P = 2.00 atm = 1520 torr
If there was air in the container, the partial pressure of the carbon dioxide will still the same, 2 atm (1520 torr), because the partial pressure is the pressure the substance would have if it eas alone in the container.
The total pressure is the sum of the partial pressures, so
Pt = 740 + 1520 = 2260 torr = 2.97 atm
