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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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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Volume Conversion
When dealing with gas calculations, understanding how to convert between different volume units is essential, especially from milliliters (mL) to liters (L). This is because gases under Standard Temperature and Pressure (STP) conditions are often measured in liters. Volume conversion is straightforward; you simply divide the volume in milliliters by 1000 to get the volume in liters.
For example, if you have a volume of 75.0 mL, converting it to liters involves the simple calculation:
  • Divide by 1000:
    \(75.0 \text{ mL} = \frac{75.0}{1000} = 0.075 \text{ L}\).
This step ensures that such volumes align with the commonly used literature and scientific calculations when working with gases at STP.
Molar Volume
The concept of molar volume is fundamental when working with gases. At Standard Temperature and Pressure (STP), which is defined as 0掳C (273.15 K) and 1 atm pressure, one mole of any ideal gas occupies the same volume, which is 22.4 liters.
The molar volume makes it possible to calculate the amount of substance (in moles) from a gas's measured volume. If you know the volume of a gas at STP, the relationship can be defined as:
  • The formula for finding moles from volume:
    \[ n = \frac{V}{V_m} \]
    where \(n\) is the number of moles, \(V\) is the gas volume, and \(V_m\) is the molar volume (22.4 L/mol at STP).
Understanding molar volume helps in converting between the volume of a gas measured at STP and the number of moles, thereby connecting macroscopic quantities with microscopic chemical identities.
Molar Mass of Argon
Argon, a noble gas, is an element with atomic number 18 and commonly found in the Earth's atmosphere. The molar mass of an element refers to the mass of one mole of its atoms. For argon, the molar mass is roughly 40 g/mol. This value is derived from the atomic mass because each mole contains Avogadro's number of atoms.
To find the mass of a specific quantity of argon, such as in a gas sample, you multiply the number of moles by the molar mass:
  • The formula used:
    \[ m = n \times M \]
    where \(m\) is the mass, \(n\) is the number of moles, and \(M\) is the molar mass of argon (40 g/mol).
Knowing the molar mass is crucial for calculating how much argon is in a given set of conditions, thus facilitating various scientific and industrial applications.

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Most popular questions from this chapter

A 132.10 mL glass vessel weighs 56.1035 g when evacuated and \(56.2445 \mathrm{g}\) when filled with the gaseous hydrocarbon acetylene at \(749.3 \mathrm{mmHg}\) and \(20.02^{\circ} \mathrm{C}\) What is the molar mass of acetylene? What conclusion can you draw about its molecular formula?

A gaseous hydrocarbon that is \(82.7 \%\) C and \(17.3 \%\) H by mass has a density of \(2.35 \mathrm{g} / \mathrm{L}\) at \(25^{\circ} \mathrm{C}\) and 752 Torr. What is the molecular formula of this hydrocarbon?

A 4.0 L sample of \(\mathrm{O}_{2}\) gas has a pressure of 1.0 atm. A 2.0 L sample of \(\mathrm{N}_{2}\) gas has a pressure of 2.0 atm. If these two samples are mixed and then compressed in a 2.0 L vessel, what is the final pressure of the mixture? Assume that the temperature remains unchanged.

A particular coal sample contains \(3.28 \%\) S by mass. When the coal is burned, the sulfur is converted to \(\mathrm{SO}_{2}(\mathrm{g}) .\) What volume of \(\mathrm{SO}_{2}(\mathrm{g}),\) measured at \(23^{\circ} \mathrm{C}\) and \(738 \mathrm{mm} \mathrm{Hg},\) is produced by burning \(1.2 \times 10^{6} \mathrm{kg}\) of this coal?

Hydrogen peroxide, \(\mathrm{H}_{2} \mathrm{O}_{2},\) is used to disinfect contact lenses. How many milliliters of \(\mathrm{O}_{2}(\mathrm{g})\) at \(22^{\circ} \mathrm{C}\) and \(752 \mathrm{mmHg}\) can be liberated from \(10.0 \mathrm{mL}\) of an aqueous solution containing \(3.00 \% \mathrm{H}_{2} \mathrm{O}_{2}\) by mass? The density of the aqueous solution of \(\mathrm{H}_{2} \mathrm{O}_{2}\) is \(1.01 \mathrm{g} / \mathrm{mL}\) $$2 \mathrm{H}_{2} \mathrm{O}_{2}(\mathrm{aq}) \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}(1)+\mathrm{O}_{2}(\mathrm{g})$$
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