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Chapter 6: Problem 17

What is the mass of argon gas in a \(75.0 \mathrm{mL}\) volume at STP?

Short Answer

Expert verified
The mass of argon gas in a \(75.0 \mathrm{mL}\) volume at STP is approximately \(0.134 \mathrm{g}\).

Step by step solution

01

Convert the volume to liters

To start, convert the volume given in milliliters (mL) to liters (L) because STP conditions are usually expressed in liters. This is done by dividing the volume by 1000 as follows: \(75.0 \mathrm{mL} = 75.0/1000 = 0.075 \mathrm{L}\) .
02

Calculate the number of moles of the gas

Next, use the volume and the molar volume at STP to calculate the number of moles of the gas. The molar volume at STP is typically given as \(22.4 \mathrm{L/mol}\) . Therefore the number of moles can be calculated using the formula \( n = V/V_m = 0.075 \mathrm{L} /22.4 \mathrm{L/mol} = 0.00335 \mathrm{mol}\).
03

Calculate the mass of the gas

Finally, use the number of moles and the molar mass of argon to calculate the mass of the gas. The molar mass of argon is around \(40 g/mol\) . The formula is \( m = n \cdot M = 0.00335 \mathrm{mol} \cdot 40 \mathrm{g/mol} = 0.134 \mathrm{g}\).

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