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Chapter 8: Problem 25

Which noble gas has the smallest density at STP? Explain.

Short Answer

Expert verified
Helium (He) has the smallest density among the noble gases at standard temperature and pressure (STP) because it has the lowest molar mass (4.0026 g/mol) compared to other noble gases. At STP, the density of a gas is directly proportional to its molar mass, and since helium has the smallest molar mass, it also has the smallest density.

Step by step solution

01

Identify the noble gases

Noble gases are found in Group 18 of the periodic table. These elements are known for their low reactivity due to their stable electron configurations. The noble gases are: helium (He), neon (Ne), argon (Ar), krypton (Kr), xenon (Xe), and radon (Rn).
02

Understand the relationship between molar mass and density at STP

Density (\( \rho \)) is defined as mass per unit volume. At standard temperature and pressure, the density of a gas can be calculated using the formula: \[ \rho = \frac{molar~mass}{molar~volume} \] where molar mass is given in grams per mole and molar volume is typically represented as 22.4 L/mol for any ideal gas at STP.
03

Compare the molar masses of the noble gases

The molar masses of the noble gases are as follows: - Helium (He): 4.0026 g/mol - Neon (Ne): 20.1797 g/mol - Argon (Ar): 39.948 g/mol - Krypton (Kr): 83.798 g/mol - Xenon (Xe): 131.293 g/mol - Radon (Rn): 222 g/mol
04

Determine the noble gas with the smallest density at STP

Comparing the molar masses of the noble gases, we can see that helium (He) has the smallest molar mass. Since the molar volume at STP is the same for all ideal gases, a smaller molar mass will result in a smaller density. Therefore, helium (He) has the smallest density among the noble gases at standard temperature and pressure.

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Most popular questions from this chapter

A spherical glass container of unknown volume contains helium gas at \(25^{\circ} \mathrm{C}\) and \(1.960\) atm. When a portion of the helium is withdrawn and adjusted to 1.00 atm at \(25^{\circ} \mathrm{C},\) it is found to have a volume of \(1.75 \mathrm{cm}^{3} .\) The gas remaining in the first container shows a pressure of \(1.710 \) atm. Calculate the volume of the spherical container.

The average lung capacity of a human is \(6.0 \mathrm{~L}\). How many moles of air are in your lungs when you are in the following situations? a. At sea level \((T=298 \mathrm{~K}, P=1.00 \mathrm{~atm})\). b. \(10 . \mathrm{m}\) below water \((T=298 \mathrm{~K}, P=1.97 \mathrm{~atm})\). c. At the top of Mount Everest \((T=200 . \mathrm{K}, P=0.296 \mathrm{~atm})\).

A particular balloon is designed by its manufacturer to be inflated to a volume of no more than 2.5 L. If the balloon is filled with 2.0 L helium at sea level, is released, and rises to an altitude at which the atmospheric pressure is only \(500 . \mathrm{mm}\) Hg, will the balloon burst? (Assume temperature is constant.)

Calculate the pressure exerted by \(0.5000\) mole of \(\mathrm{N}_{2}\) in a \(1.0000-\mathrm{L}\) container at \(25.0^{\circ} \mathrm{C}\) a. using the ideal gas law. b. using the van der Waals equation. c. Compare the results.

A \(20.0\) -\(\mathrm{L}\) stainless steel container at \(25^{\circ} \mathrm{C}\) was charged with \(2.00\) atm of hydrogen gas and \(3.00\) atm of oxygen gas. A spark ignited the mixture, producing water. What is the pressure in the tank at \(25^{\circ} \mathrm{C} ?\) If the exact same experiment were performed, but the temperature was \(125^{\circ} \mathrm{C}\) instead of \(25^{\circ} \mathrm{C},\) what would be the pressure in the tank?
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