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Chapter 6: Problem 137

The gas with the greatest density at STP is (a) \(\mathrm{N}_{2} \mathrm{O}\) (b) \(\mathrm{Kr} ;\) (c) \(\mathrm{SO}_{3} ;\) (d) \(\mathrm{Cl}_{2}\).

Short Answer

Expert verified
The gas with the greatest density at Standard Temperature and Pressure (STP) is \(Kr\).

Step by step solution

01

Calculate The Molar Mass Of \(N_2O\)

The molar mass of a molecule is the sum of the molar masses of its atoms. Nitrogen's molar mass is 14.01 g/mol and Oxygen's molar mass is 16.00 g/mol. The \(N_2O\) molecule has 2 Nitrogen atoms and 1 Oxygen atom, thus the molar mass of \(N_2O\) is \(2*14.01 g/mol + 16.00 g/mol = 44.02 g/mol\).
02

Calculate The Molar Mass Of \(Kr\)

The Kr is a noble gas. Its atomic mass is 83.80 g/mol which is same as molar mass because it is monoatomic. So the molar mass of \(Kr\) is 83.80 g/mol.
03

Calculate The Molar Mass Of \(SO_3\)

Similar to step 1, the molar mass of \(SO_3\) is \(1*32.07 g/mol + 3*16.00 g/mol = 80.07 g/mol\).
04

Calculate The Molar Mass Of \(Cl_2\)

The \(Cl_2\) molecule has 2 Chlorine atoms. As the molar mass of Chlorine is 35.45 g/mol, the molar mass of \(Cl_2\) is \(2 * 35.45 g/mol = 70.90 g/mol\).
05

Compare The Molar Mass Of All four Gases

After comparing all the molar masses calculated above, it appears that \(Kr\) has the highest molar mass (83.80 g/mol). Therefore, \(Kr\) is the densest gas at STP.

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Most popular questions from this chapter

Under which conditions is \(\mathrm{Cl}_{2}\) most likely to behave like an ideal gas? Explain. (a) \(100^{\circ} \mathrm{C}\) and \(10.0 \mathrm{atm}\) (b) \(0^{\circ} \mathrm{C}\) and 0.50 atm; \((\mathrm{c}) 200^{\circ} \mathrm{C}\) and \(0.50 \mathrm{atm}\) (d) \(400^{\circ} \mathrm{C}\) and \(10.0 \mathrm{atm}\).

Calculate \(u_{\mathrm{rms}},\) in meters per second, for \(\mathrm{Cl}_{2}(\mathrm{g})\) molecules at \(30^{\circ} \mathrm{C}\)

To establish a pressure of 2.00 atm in a 2.24 L cylinder containing \(1.60 \mathrm{g} \mathrm{O}_{2}(\mathrm{g})\) at \(0^{\circ} \mathrm{C},\) (a) add \(1.60 \mathrm{g} \mathrm{O}_{2} ;(\mathrm{b})\) add \(0.60 \mathrm{g} \mathrm{He}(\mathrm{g}) ;(\mathrm{c})\) add \(2.00 \mathrm{g} \mathrm{He}(\mathrm{g})\) (d) release \(0.80 \mathrm{g} \mathrm{O}_{2}(\mathrm{g})\)

What is the partial pressure of \(\mathrm{Cl}_{2}(\mathrm{g}),\) in millimeters of mercury, at \(0.00^{\circ} \mathrm{C}\) and 1.00 atm in a gaseous mixture that consists of \(46.5 \% \mathrm{N}_{2}, 12.7 \% \mathrm{Ne},\) and \(40.8 \%\) \(\mathrm{Cl}_{2},\) by mass?

What is the pressure (in \(\mathrm{mmHg}\) ) of the gas inside the apparatus below if \(P_{\text {bar. }}=740 \mathrm{mm} \mathrm{Hg}, h_{1}=30 \mathrm{mm}\) and \(h_{2}=50 \mathrm{mm} ?\)
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