Answer:
The mass of the air is 6920.71g
Explanation:
Step 1:
Data obtained from the question. This includes the following:
Volume (V) = 5.0x10^3 L
Molar Mass of air (M) = 28.98 g/mol
Temperature (T) = 0.2°C
Pressure (P) = 1.07 atm
mass air (m) =?
Number of mole (n) =?
Recall:
Gas constant (R) = 0.082atm.L/Kmol
Step 2:
Conversion of celsius temperature to Kelvin temperature.
K = °C + 273
°C = 0.2°C
K = °C + 273
K = 0.2°C + 273
K = 273.2 K
Therefore, the temperature (T) = 273.2 K
Step 3:
Determination of the number of mole of air.
Applying the ideal gas equation PV = nRT, the number of mole n, can be obtained as follow:
PV = nRT
1.07 x 5.0x10^3 = n x 0.082 x 273.2
Divide both side by 0.082 x 273.2
n = (1.07 x 5.0x10^3)/(0.082 x 273.2)
n = 238.81 moles
Step 4:
Determination of the mass of air. This is illustrated below:
Number of mole of air = 238.81 moles
Molar Mass of air = 28.98 g/mol
Mass of air =.?
Mass = number of mole x molar Mass
Mass of air = 238.81 x 28.98
Mass of air = 6920.71g
