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Calculate the mass of \( 139 \, \text{cm}^3 \) of Argon at STP.

Answer :

Final answer:

The mass of 139 cm^3 of argon at STP is calculated using the molar volume and molar mass of argon, resulting in approximately 0.2479 grams.

Explanation:

To calculate the mass of 139 cm3 of argon at STP (standard temperature and pressure, defined as 0°C and 1 atm), you first use the molar volume of a gas at STP. This is known to be 22.4 liters (or 22,400 cm3) per mole. Since the molar mass of argon (Ar) is approximately 39.948 g/mol, you can find out how many moles of argon are in 139 cm3 and then calculate the mass.

To begin with, determine the number of moles:

№ moles of Ar = volume of Ar / molar volume = 139 cm3 / 22,400 cm3/mol

Then, calculate the mass:

Mass of Ar = № moles of Ar × molar mass of Ar = (139 cm3 / 22,400 cm3/mol) × 39.948 g/mol

After doing the calculations, we find that the mass of 139 cm3 of argon at STP is approximately:

Mass of Ar = (139 / 22,400) × 39.948 g ≈ 0.2479 g

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Rewritten by : Barada

Volume in liters:

139 cm³ / 1000 = 0.139 L

molar mass Argon = 39.95 g/mol

1 mole -------- 22.4 L ( at STP )
? mole ------- 0.139 L

moles of argon :

0.139 * 1 / 22.4 = 0.00620 moles

Mass of argon :

0.00620 * 39.95 = 0.24769 g

hope this helps!