Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 5: Problem 36

A gauge on a compressed gas cylinder reads 2200 psi (pounds per square inch; 1 atm \(=14.7\) psi). Express this pressure in each of the following units. a. standard atmospheres b. megapascals (MPa) c. torr

Short Answer

Expert verified
The pressure of 2200 psi is approximately equal to 149.66 atm, 15.167 MPa, and 113,713 torr.

Step by step solution

01

Convert psi to atmospheres

Given the pressure gauge reading as 2200 psi, we will first convert it to standard atmospheres using the given conversion factor (1 atm = 14.7 psi). \(Number\ of\ atmospheres = \frac{Pressure\ in\ psi}{Conversion\ factor}\)
02

Calculate atmospheres

Now we will plug in the values and find the number of atmospheres. \(Number\ of\ atmospheres = \frac{2200}{14.7}\) \(Number\ of\ atmospheres ≈ 149.66\) Therefore, the pressure in standard atmospheres is approximately 149.66 atm.
03

Convert psi to megapascals (MPa)

Next, we need to convert the pressure in psi to megapascals (MPa). To do this, we will use the conversion factor 1 psi = 0.00689476 MPa. \(Pressure\ in\ MPa = Pressure\ in\ psi × Conversion\ factor\)
04

Calculate megapascals

Now we will plug in the values and find the pressure in MPa. \(Pressure\ in\ MPa = 2200 × 0.00689476\) \(Pressure\ in\ MPa ≈ 15.167\) Therefore, the pressure in megapascals is approximately 15.167 MPa.
05

Convert psi to torr

Lastly, we need to convert the pressure in psi to torr. To do this, we will use the conversion factor 1 psi = 51.7149 torr. \(Pressure\ in\ torr = Pressure\ in\ psi × Conversion\ factor\)
06

Calculate torr

Now we will plug in the values and find the pressure in torr. \(Pressure\ in\ torr = 2200 × 51.7149\) \(Pressure\ in\ torr ≈ 113713\) Therefore, the pressure in torr is approximately 113,713 torr.

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.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

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

Consider the following reaction: $$ 4 \mathrm{Al}(s)+3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{Al}_{2} \mathrm{O}_{3}(s) $$ It takes \(2.00 \mathrm{~L}\) pure oxygen gas at STP to react completely with a certain sample of aluminum. What is the mass of aluminum reacted?

From the values in Table \(5.3\) for the van der Waals constant \(a\) for the gases \(\mathrm{H}_{2}, \mathrm{CO}_{2}, \mathrm{~N}_{2}\), and \(\mathrm{CH}_{4}\), predict which of these gas molecules show the strongest intermolecular attractions.

A gas sample containing \(1.50 \mathrm{~mol}\) at \(25^{\circ} \mathrm{C}\) exerts a pressure of 400 . torr. Some gas is added to the same container and the temperature is increased to \(50 .{ }^{\circ} \mathrm{C}\). If the pressure increases to 800 . torr, how many moles of gas were added to the container? Assume a constant-volume container.

At STP, \(1.0 \mathrm{~L} \mathrm{Br}_{2}\) reacts completely with \(3.0 \mathrm{~L} \mathrm{~F}_{2}\), producing 2.0 L of a product. What is the formula of the product? (All substances are gases.)

As \(\mathrm{NH}_{3}(g)\) is decomposed into nitrogen gas and hydrogen gas at constant pressure and temperature, the volume of the product gases collected is twice the volume of \(\mathrm{NH}_{3}\) reacted. Explain. As \(\mathrm{NH}_{3}(g)\) is decomposed into nitrogen gas and hydrogen gas at constant volume and temperature, the total pressure increases by some factor. Why the increase in pressure and by what factor does the total pressure increase when reactants are completely converted into products? How do the partial pressures of the product gases compare to each other and to the initial pressure of \(\mathrm{NH}_{3}\) ?
See all solutions

Recommended explanations on Chemistry Textbooks

Organic Chemistry

Read Explanation

Chemical Analysis

Read Explanation

The Earths Atmosphere

Read Explanation

Inorganic Chemistry

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Making Measurements

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.

Sign-up for free