Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 5: Problem 42

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. mega pascals (MPa) c. torr

Short Answer

Expert verified
The pressure can be expressed in the following units: a. \(149.660\) atm, b. \(15.158\) MPa, and c. \(113661.6\) torr.

Step by step solution

01

Convert psi to atm

Given pressure = 2200 psi We know that 1 atm = 14.7 psi Therefore, to convert 2200 psi to atm, we'll use the following formula: Pressure in atm = (Pressure in psi) / (Conversion factor) Pressure in atm = 2200 psi / 14.7 psi/atm = 149.660 atm a. The pressure in standard atmospheres is approximately 149.660 atm.
02

Convert atm to MPa

Now, we will convert the pressure from atm to MPa. We know that: 1 atm = 101.325 kPa, and 1 MPa = 1000 kPa Therefore, to convert the pressure from atm to MPa, we'll follow these steps: 1. Convert atm to kPa Pressure in kPa = (Pressure in atm) × (Conversion factor) Pressure in kPa = 149.660 atm × 101.325 kPa/atm ≈ 15158.31 kPa 2. Convert kPa to MPa Pressure in MPa = (Pressure in kPa) / 1000 Pressure in MPa = 15158.31 kPa / 1000 = 15.158 MPa b. The pressure in mega pascals is approximately 15.158 MPa.
03

Convert atm to torr

Lastly, we will convert the pressure from atm to torr. We know that: 1 atm = 760 torr To convert the pressure from atm to torr, we'll use the following formula: Pressure in torr = (Pressure in atm) × (Conversion factor) Pressure in torr = 149.660 atm × 760 torr/atm ≈ 113661.6 torr c. The pressure in torr is approximately 113661.6 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 a sample of a hydrocarbon (a compound consisting of only carbon and hydrogen) at 0.959 atm and 298 \(\mathrm{K}\). Upon combusting the entire sample in oxygen, you collect a mixture of gaseous carbon dioxide and water vapor at 1.51 atm and 375 \(\mathrm{K}\). This mixture has a density of 1.391 g/L and occupies a volume four times as large as that of the pure hydrocarbon. Determine the molecular formula of the hydrocarbon

You have a gas in a container fitted with a piston and you change one of the conditions of the gas such that a change takes place, as shown below: State three distinct changes you can make to accomplish this, and explain why each would work.

Atmospheric scientists often use mixing ratios to express the concentrations of trace compounds in air. Mixing ratios are often expressed as ppmv (parts per million volume): $${\text {ppmv of}} \ X=\frac{\text { vol of } X \text { at STP }}{\text { total vol of air at STP }} \times 10^{6}$$ On a certain November day, the concentration of carbon monoxide in the air in downtown Denver, Colorado, reached \(3.0 \times 10^{2}\) ppmv. The atmospheric pressure at that time was 628 torr and the temperature was $0^{\circ} \mathrm{C}$ . a. What was the partial pressure of CO? b. What was the concentration of CO in molecules per cubic meter? c. What was the concentration of CO in molecules per cubic centimeter?

A \(1.0-\mathrm{L}\) sample of air is collected at \(25^{\circ} \mathrm{C}\) at sea level \((1.00 \mathrm{atm}) .\) Estimate the volume this sample of air would have at an altitude of 15 \(\mathrm{km}\) ( see Fig.5.30) .At \(15 \mathrm{km},\) the pressure is about 0.1 \(\mathrm{atm} .\)

A bicycle tire is filled with air to a pressure of 75 psi at a temperature of \(19^{\circ} \mathrm{C}\) . Riding the bike on asphalt on a hot day increases the temperature of the tire to \(58^{\circ} \mathrm{C}\) . The volume of the tire increases by 4.0\(\%\) . What is the new pressure in the bicycle tire?
See all solutions

Recommended explanations on Chemistry Textbooks

The Earths Atmosphere

Read Explanation

Organic Chemistry

Read Explanation

Chemistry Branches

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Chemical Reactions

Read Explanation

Kinetics

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