/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 12 Why do astronauts have to wear p... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

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鈥檚 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.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with 91影视!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Based on your knowledge of the kinetic theory of gases, derive Graham's law of diffusion [Equation ( 5.17 )]

A sample of air contains only nitrogen and oxygen gases whose partial pressures are 0.80 atm and 0.20 atm, respectively. Calculate the total pressure and the mole fractions of the gases.

Dry air near sea level has the following composition by volume: \(\mathrm{N}_{2}, 78.08\) percent; \(\mathrm{O}_{2}, 20.94\) percent; \(\mathrm{Ar},\) 0.93 percent; \(\mathrm{CO}_{2}, 0.05\) percent. The atmospheric pressure is \(1.00 \mathrm{~atm} .\) Calculate (a) the partial pressure of each gas in atm and (b) the concentration of each gas in moles per liter at \(0^{\circ} \mathrm{C}\).

At a certain temperature the speeds of six gaseous molecules in a container are \(2.0 \mathrm{~m} / \mathrm{s}, 2.2 \mathrm{~m} / \mathrm{s}, 2.6 \mathrm{~m} / \mathrm{s}\) \(2.7 \mathrm{~m} / \mathrm{s}, 3.3 \mathrm{~m} / \mathrm{s},\) and \(3.5 \mathrm{~m} / \mathrm{s} .\) Calculate the root- mean-square speed and the average speed of the molecules. These two average values are close to each other, but the root-mean-square value is always the larger of the two. Why?

Define Dalton's law of partial pressures and mole fraction. Does mole fraction have units?
See all solutions

Recommended explanations on Chemistry Textbooks

Inorganic Chemistry

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Organic Chemistry

Read Explanation

Nuclear Chemistry

Read Explanation

Chemical Analysis

Read Explanation

Chemical Reactions

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.