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Chapter 5: Problem 12

Why do astronauts have to wear protective suits when they are on the surface of the moon?

Short Answer

Expert verified
Astronauts have to wear protective suits on the moon because these suits protect them against the moon's extreme temperatures, provide a supply of oxygen, shield them from harmful solar radiation, and help them survive in the vacuum of space.

Step by step solution

01

Understand the Environment of the Moon

To answer this question, it is first important to understand the environment of the moon. The moon is a place with extreme temperatures, no breathable air and is exposed to solar radiation. It also has no atmospheric pressure.
02

Identify the protection needed

Given the moon's environment, astronauts need protection against these harsh conditions. They need to have controlled temperatures, a supply of oxygen, protection against radiation and be able to survive under no pressure conditions.
03

Connect the Conditions with the Suit’s Features

The astronaut protective suit, also known as a space suit, is designed to protect against these conditions. It is insulated to handle extreme temperatures, it has a self-contained oxygen supply for breathing, it is lined with radiation-reflecting materials, and it is built to withstand the vacuum of space.

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Most popular questions from this chapter

Discuss the following phenomena in terms of the gas laws: (a) the pressure in an automobile tire increasing on a hot day, (b) the "popping" of a paper bag, (c) the expansion of a weather balloon as it rises in the air, (d) the loud noise heard when a lightbulb shatters.

A \(36.4-\mathrm{L}\) volume of methane gas is heated from \(25^{\circ} \mathrm{C}\) to \(88^{\circ} \mathrm{C}\) at constant pressure. What is the final volume of the gas?

Helium is mixed with oxygen gas for deep sea divers. Calculate the percent by volume of oxygen gas in the mixture if the diver has to submerge to a depth where the total pressure is \(4.2 \mathrm{~atm} .\) The partial pressure of oxygen is maintained at 0.20 atm at this depth.

The boiling point of liquid nitrogen is \(-196^{\circ} \mathrm{C}\). On the basis of this information alone, do you think nitrogen is an ideal gas?

A volume of \(0.280 \mathrm{~L}\) of a gas at STP weighs \(0.400 \mathrm{~g}\). Calculate the molar mass of the gas.
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