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Chapter 5: Problem 32

Without looking at a table of values, which of the following gases would you expect to have the largest value of the van der Waals constant \(b: \mathrm{H}_{2}, \mathrm{~N}_{2}, \mathrm{CH}_{4}, \mathrm{C}_{2} \mathrm{H}_{6}\), or \(\mathrm{C}_{3} \mathrm{H}_{8}\) ?

Short Answer

Expert verified
The gas with the largest value of the van der Waals constant \(b\) would be C3H8 (Propane), as it has the largest molecular weight (\(44.096 \, amu\)) among the given gases. This is because molecular weight plays a significant role in determining the van der Waals constant \(b\).

Step by step solution

01

Analyzing the molecular weight

To determine which gas would have the largest value of the van der Waals constant b, we'll need to consider the molecular weight of each gas. Remember that the molecular weight is determined by the sum of the atomic weights of the atoms in the molecule.
02

Evaluating each gas's molecular weight

Let's evaluate the molecular weight of each gas: 1. H2 (Hydrogen gas): Its molecular weight is 2(1.008) = \(2.016 \, amu\) 2. N2 (Nitrogen gas): Its molecular weight is 2(14.007) = \(28.014 \, amu\) 3. CH4 (Methane): Its molecular weight is 12.011 + 4(1.008) = \(16.043 \, amu\) 4. C2H6 (Ethane): Its molecular weight is 2(12.011) + 6(1.008) = \(30.069 \, amu\) 5. C3H8 (Propane): Its molecular weight is 3(12.011) + 8(1.008) = \(44.096 \, amu\)
03

Identifying the gas with the largest molecular weight

Comparing the molecular weight of each gas, we can see that C3H8 (Propane) has the largest molecular weight of \(44.096 \, amu\).
04

Determining the gas with the largest value of the van der Waals constant b

Since molecular weight plays a significant role in determining the van der Waals constant b, we can conclude that C3H8 (Propane) would have the largest value of the van der Waals constant b among the given gases due to its largest molecular weight.

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Most popular questions from this chapter

As weather balloons rise from the earth's surface, the pressure of the atmosphere becomes less, tending to cause the volume of the balloons to expand. However, the temperature is much lower in the upper atmosphere than at sea level. Would this temperature effect tend to make such a balloon expand or contract? Weather balloons do, in fact, expand as they rise. What does this tell you?

A 20.0-L stainless steel container at \(25^{\circ} \mathrm{C}\) was charged with \(2.00\) atm of hydrogen gas and \(3.00 \mathrm{~atm}\) of oxygen gas. A spark ignited the mixture, producing water. What is the pressure in the tank at \(25^{\circ} \mathrm{C}\) ? If the 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?

A gauge on a compressed gas cylinder reads 2200 psi (pounds per square inch; 1 atm \(=14.7\) psi). Express this pressure in each of the following units. a. standard atmospheres b. megapascals (MPa) c. torr

Calculate the pressure exerted by \(0.5000 \mathrm{~mol} \mathrm{~N}_{2}\) in a \(10.000-\mathrm{L}\) container at \(25.0^{\circ} \mathrm{C}\) a. using the ideal gas law. b. using the van der Waals equation. c. Compare the results. d. Compare the results with those in Exercise 107 .

Cyclopropane, a gas that when mixed with oxygen is used as a general anesthetic, is composed of \(85.7 \% \mathrm{C}\) and \(14.3 \% \mathrm{H}\) by mass. If the density of cyclopropane is \(1.88 \mathrm{~g} / \mathrm{L}\) at \(\mathrm{STP}\), what is the molecular formula of cyclopropane?
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