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Chapter 5: Problem 70

A mixture of helium and neon gases is collected over water at \(28.0^{\circ} \mathrm{C}\) and \(745 \mathrm{mmHg} .\) If the partial pressure of helium is \(368 \mathrm{mmHg}\), what is the partial pressure of neon? (Vapor pressure of water at \(28^{\circ} \mathrm{C}=\) \(28.3 \mathrm{mmHg} .\) )

Short Answer

Expert verified
The partial pressure of neon is \(348.7 \, \mathrm{mmHg}\).

Step by step solution

01

Identify Given Variables

The total pressure in the system is given as \(745 \, \mathrm{mmHg}\). The partial pressure of helium in the system is given as \(368 \, \mathrm{mmHg}\). The pressure of water in the system is given as \(28.3 \, \mathrm{mmHg}\).
02

Apply Dalton's Law of Partial Pressures

According to Dalton's Law of Partial Pressures, the total pressure is equal to the sum of the partial pressures of individual gases. In this case, the total pressure will be the sum of the pressure of helium, neon, and water. With the given data, the equation can be formed as: \(745 = 368 + P_{Ne} + 28.3\) where \(P_{Ne}\) denotes the pressure of neon.
03

Solve for Neon's Partial Pressure

Reorder the equation to solve for \(P_{Ne}\) which gives: \(P_{Ne} = 745 - 368 - 28.3\).
04

Perform the Calculation

By solving, the value of \(P_{Ne}\) will be: \(P_{Ne} = 348.7 \, \mathrm{mmHg}\).

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Most popular questions from this chapter

An equimolar mixture of \(\mathrm{H}_{2}\) and \(\mathrm{D}_{2}\) effuses through an orifice (small hole) at a certain temperature. Calculate the composition (in mole fractions) of the gases that pass through the orifice. The molar mass of \(\mathrm{D}_{2}\) is \(2.014 \mathrm{~g} / \mathrm{mol}\)

Two vessels are labeled A and B. Vessel A contains \(\mathrm{NH}_{3}\) gas at \(70^{\circ} \mathrm{C},\) and vessel \(\mathrm{B}\) contains \(\mathrm{Ne}\) gas at the same temperature. If the average kinetic energy of \(\mathrm{NH}_{3}\) is \(7.1 \times 10^{-21} \mathrm{~J} / \mathrm{molecule},\) calculate the rootmean- square speed of Ne atoms.

Apply your knowledge of the kinetic theory of gases to the following situations. (a) Two flasks of volumes \(V_{1}\) and \(V_{2}\left(V_{2}>V_{1}\right)\) contain the same number of helium atoms at the same temperature. (i) Compare the root-mean-square (rms) speeds and average kinetic energies of the helium (He) atoms in the flasks. (ii) Compare the frequency and the force with which the He atoms collide with the walls of their containers. (b) Equal numbers of He atoms are placed in two flasks of the same volume at temperatures \(T_{1}\) and \(T_{2}\left(T_{2}>T_{1}\right) .\) (i) Compare the rms speeds of the atoms in the two flasks. (ii) Compare the frequency and the force with which the He atoms collide with the walls of their containers. (c) Equal numbers of He and neon (Ne) atoms are placed in two flasks of the same volume, and the temperature of both gases is \(74^{\circ} \mathrm{C}\). Comment on the validity of the following statements: (i) The rms speed of He is equal to that of Ne. (ii) The average kinetic energies of the two gases are equal. (iii) The rms speed of each He atom is \(1.47 \times 10^{3} \mathrm{~m} / \mathrm{s}\)

The density of a mixture of fluorine and chlorine gases is \(1.77 \mathrm{~g} / \mathrm{L}\) at \(14^{\circ} \mathrm{C}\) and 0.893 atm. Calculate the mass percent of the gases.

Ethanol \(\left(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\right)\) burns in air: $$ \mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}(l)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l) $$ Balance the equation and determine the volume of air in liters at \(35.0^{\circ} \mathrm{C}\) and \(790 \mathrm{mmHg}\) required to burn \(227 \mathrm{~g}\) of ethanol. Assume that air is 21.0 percent \(\mathrm{O}_{2}\) by volume.
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