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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 CO₂ 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

Dilute aqueous hydrogen peroxide is used as a bleaching agent and for disinfecting surfaces and small cuts. Its concentration is sometimes given as a certain number of "volumes hydrogen peroxide," which refers to the number of volumes of \(\mathrm{O}_{2}\) gas, measured at STP, that a given volume of hydrogen peroxide solution will release when it decomposes to \(\mathrm{O}_{2}\) and liquid \(\mathrm{H}_{2} \mathrm{O}\). How many grams of hydrogen peroxide are in \(0.100 \mathrm{~L}\) of \(" 20\) volumes hydrogen peroxide" solution?

Ammonium nitrate, a common fertilizer, was used by terrorists in the tragic explosion in Oklahoma City in \(1995 .\) How many liters of gas at \(307^{\circ} \mathrm{C}\) and 1.00 atm are formed by the explosive decomposition of \(15.0 \mathrm{~kg}\) of ammonium nitrate to nitrogen, oxygen, and water vapor?

Convert each of the pressures described below to atm: (a) At the peak of Mt. Everest, atmospheric pressure is only \(2.75 \times 10^{2} \mathrm{mmHg}\) (b) A cyclist fills her bike tires to 86 psi. (c) The surface of Venus has an atmospheric pressure of \(9.15 \times 10^{6} \mathrm{~Pa}\) (d) At \(100 \mathrm{ft}\) below sea level, a scuba diver experiences a pressure of \(2.54 \times 10^{4}\) torr.

What is the ratio of effusion rates for the lightest gas, \(\mathrm{H}_{2}\), and the heaviest known gas, UF \(_{6} ?\)

An atmospheric chemist studying the pollutant \(\mathrm{SO}_{2}\) places a mixture of \(\mathrm{SO}_{2}\) and \(\mathrm{O}_{2}\) in a 2.00 -L container at \(800 . \mathrm{K}\) and \(1.90 \mathrm{~atm}\). When the reaction occurs, gaseous \(\mathrm{SO}_{3}\) forms, and the pressure falls to 1.65 atm. How many moles of \(\mathrm{SO}_{3}\) form?
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