Answer:
3.34x10^–4 Torr
Explanation:
Step 1:
Data obtained from the question:
Mass of CO2 = 99g
Volume (V) = 1.24x10^5 m^3
Temperature (T) = 22ºC
Pressure =?
Step 2:
Determination of the number of mole of CO2.
Mass of CO2 = 99g
Molar Mass of CO2 = 12 + (2x16) = 44g/mol
Number of mole =Mass /Molar Mass
Number of mole of CO2 = 99/44
Number of mole of CO2 = 2.25 moles
Step 3:
Conversion to appropriate unit.
For Volume :
1 m^3 = 1000L
Therefore, 1.24x10^5 m^3 = 1.24x10^5 x 1000 = 1.24x10^8 L
For temperature:
T (Kelvin) = T (°C) + 273
T (°C) = 22ºC
T(Kelvin) = 22ºC + 273 = 295K
Step 4:
Determination of the pressure exerted by the gas.
The pressure can be obtained by using the ideal gas equation as follow:
Volume (V) = 1.24x10^8 L
Temperature (T) = 295K
Number of mole (n) = 2.25 moles
Gas constant (R) = 0.082atm.L/Kmol
Pressure =?
PV = nRT
Divide both side by V
P = nRT /V
P = (2.25 x 0.082 x 295) /1.24x10^8
P = 4.39x10^–7 atm.
Step 5:
Conversion of 4.39x10^–7 atm to Torr.
This is illustrated below:
1 atm = 760 Torr
Therefore, 4.39x10^–7 = 4.39x10^–7 x 760 = 3.34x10^–4 Torr
Therefore, the pressure exerted by the gass in torr is 3.34x10^–4 Torr
