Answer:
0.437 g
Step-by-step explanation:
From the question we have;
Pressure of the gas as 0.2829
Volume of the gas as 1.35 L
Temperature of the gas as 25°C
But, K = °C + 273.15
Therefore, temperature of the gas is equivalent to 298.15 K
We are required to calculate the mass of the gas
Step 1: Number of moles of the gas
Using the ideal gas equation, PV = nRT , we can determine the number of moles.
R is the ideal gas constant, 0.082057 L.atm/mol.K
Therefore, rearranging the formula;
n = PV ÷ RT
= (0.2829 atm × 1.35 L) ÷ (0.082057 × 298.15 K)
= 0.0156 mole
Therefore, the number of moles of the gas is 0.0156 mole
Step 2: Mass of the gas
We know that mass of a compound is the product of moles and the molar mass.
Mass = Moles × Molar mass
Molar mass of the gas is 28.0134 g/mol
Therefore;
= 0.0156 mole × 28.0134 g/mol
= 0.437 g
Thus, the mass of the gas is 0.437 g