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Chapter 5: Problem 41

To collect a beaker of \(\mathrm{H}_{2}\) gas by displacing the air already in the beaker, would you hold the beaker upright or inverted? Why? How would you hold the beaker to collect \(\mathrm{CO}_{2}\) ?

Short Answer

Expert verified
Hold the beaker inverted for \(\text{H}_2\) and upright for \(\text{CO}_2\).

Step by step solution

01

Understand the Properties of \(\text{H}_2\) Gas

\(\text{H}_2\) gas is less dense than air, so it will rise above the air when released. Therefore, to collect \(\text{H}_2\) gas, the beaker should be held inverted to allow the gas to displace the air and fill the beaker from the bottom.
02

Understand the Properties of \(\text{CO}_2\) Gas

\(\text{CO}_2\) gas is denser than air, so it will sink below the air when released. Therefore, to collect \(\text{CO}_2\) gas, the beaker should be held upright to allow the gas to displace the air and fill the beaker from the bottom.
03

Determine the Correct Orientation for Each Gas

For collecting \(\text{H}_2\) gas, hold the beaker inverted. For collecting \(\text{CO}_2\) gas, hold the beaker upright.

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Key Concepts

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

hydrogen gas properties
Hydrogen is the lightest gas known, and it has some unique properties. It is colorless, odorless, and tasteless. Hydrogen is less dense than air, making it much lighter. Because of its low density, hydrogen gas will rise in the atmosphere when released.
When collecting hydrogen gas, its lightness plays a crucial role. If you want to gather this gas for any experiment or observation, you need to hold the collection container (like a beaker) upside down. This way, the hydrogen, being lighter, can fill up the beaker from the bottom as it displaces the air inside.
carbon dioxide gas properties
Carbon dioxide is different from hydrogen in both weight and behavior. It's also colorless and odorless but denser than air. Because it is heavier, carbon dioxide tends to sink below air when released.
When you need to catch carbon dioxide gas, consider its density. To collect it efficiently, you should hold an upright beaker. This orientation allows the heavier CO鈧� to move down, displacing the air and gradually filling the beaker from the bottom up. This method ensures that the gas does not escape and you have a successful collection.
gas density
Gas density is crucial for understanding different collection methods. Simply put, density is the mass of gas per unit volume. Gases with lower density than air, like hydrogen, rise because they are lighter. Gases heavier than air, like carbon dioxide, sink.
Here's a handy way to remember how to collect different gases:
  • For light gases like hydrogen, use an inverted container. The gas will rise and fill the space from the bottom.
  • For heavy gases like carbon dioxide, use an upright container. The gas will move down and displace the air from the bottom.
Understanding density helps you effectively capture gases and use them in your experiments or studies.

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Most popular questions from this chapter

In a certain experiment, magnesium boride \(\left(\mathrm{Mg}_{3} \mathrm{~B}_{2}\right)\) reacted with acid to form a mixture of four boron hydrides \(\left(\mathrm{B}_{x} \mathrm{H}_{y}\right),\) three as liquids (labeled I, II, and III) and one as a gas (IV). (a) When a \(0.1000-\mathrm{g}\) sample of each liquid was transferred to an evacuated \(750.0-\mathrm{mL}\) container and volatilized at \(70.00^{\circ} \mathrm{C},\) sample I had a pressure of 0.05951 atm; sample II, 0.07045 atm; and sample III, 0.05767 atm. What is the molar mass of each liquid? (b) Boron was determined to be \(85.63 \%\) by mass in sample I, \(81.10 \%\) in II, and \(82.98 \%\) in III. What is the molecular formula of each sample? (c) Sample IV was found to be \(78.14 \%\) boron. The rate of effusion for this gas was compared to that of sulfur dioxide; under identical conditions, \(350.0 \mathrm{~mL}\) of sample IV effused in \(12.00 \mathrm{~min}\) and \(250.0 \mathrm{~mL}\) of sulfur dioxide effused in 13.04 min. What is the molecular formula of sample IV?

The thermal decomposition of ethylene occurs during the compound's transit in pipelines and during the formation of polyethylene. The decomposition reaction is $$\mathrm{CH}_{2}=\mathrm{CH}_{2}(g) \longrightarrow \mathrm{CH}_{4}(g)+\mathrm{C}(\mathrm{graphite})$$ If the decomposition begins at \(10^{\circ} \mathrm{C}\) and 50.0 atm with a gas density of \(0.215 \mathrm{~g} / \mathrm{mL}\) and the temperature increases by \(950 \mathrm{~K}\), (a) What is the final pressure of the confined gas (ignore the volume of graphite and use the van der Waals equation)? (b) How does the \(P V / R T\) value of \(\mathrm{CH}_{4}\) compare to that in Figure \(5.23 ?\) Explain.

An equimolar mixture of Ne and Xe is accidentally placed in a container that has a tiny leak. After a short while, a very small proportion of the mixture has escaped. What is the mole fraction of Ne in the effusing gas?

The Hawaian volcano Kilauea emits an average of \(1.5 \times 10^{3} \mathrm{~m}^{3}\) of gas each day, when corrected to \(298 \mathrm{~K}\) and \(1.00 \mathrm{~atm} .\) The mixture contains gases that contribute to global warming and acid rain, and some are toxic. An atmospheric chemist analyzes a sample and finds the following mole fractions: \(0.4896 \mathrm{CO}_{2}, 0.0146 \mathrm{CO}, 0.3710 \mathrm{H}_{2} \mathrm{O}\) \(0.1185 \mathrm{SO}_{2}, 0.0003 \mathrm{~S}_{2}, 0.0047 \mathrm{H}_{2}, 0.0008 \mathrm{HCl},\) and \(0.0003 \mathrm{H}_{2} \mathrm{~S} .\) How many metric tons (t) of each gas are emitted per year ( \(1 \mathrm{t}=1000 \mathrm{~kg}\) )?

Many water treatment plants use chlorine gas to kill microorganisms before the water is released for residential use. A plant engineer has to maintain the chlorine pressure in a tank below the 85.0 -atm rating and, to be safe, decides to fill the tank to \(80.0 \%\) of this maximum pressure. (a) How many moles of \(\mathrm{Cl}_{2}\) gas can be kept in an \(850 .-\mathrm{L}\) tank at \(298 \mathrm{~K}\) if she uses the ideal gas law in the calculation? (b) What is the tank pressure if she uses the van der Waals equation for this amount of gas? (c) Did the engineer fill the tank to the desired pressure?
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