BuyFindarrow_forward

College Physics

11th Edition
Raymond A. Serway + 1 other
ISBN: 9781305952300

Solutions

Chapter
Section
BuyFindarrow_forward

College Physics

11th Edition
Raymond A. Serway + 1 other
ISBN: 9781305952300
Textbook Problem

An ideal diatomic gas expands adiabatically from 0.750 m3 to 1.50 m3. If the initial pressure and temperature are 1.50 × 105 Pa and 325 K, respectively, find (a) the number of moles in the gas, (b) the final gas pressure, (c) the final gas temperature, and (d) the work done on the gas.

(a)

To determine
The number of moles in the gas.

Explanation

Given Info:

The initial volume of the gas is 0.750m3 .

The final volume of the gas is 1.50m3 .

Initial pressure of the gas is 1.50×105Pa .

The initial temperature of the gas is 325K

Formula to calculate the number of moles in the gas is

n=PVRT

  • P is the pressure of the gas
  • V is the volume of the gas
  • R is the universal gas constant
  • T is absolute temperature

For the initial conditions,

n=PiViRTi

Substitute 1.50×105Pa for Pi , 0

(b)

To determine
the final gas pressure.

(c)

To determine
The finial gas temperature of the gas.

(d)

To determine
the work done on the gas.

Still sussing out bartleby?

Check out a sample textbook solution.

See a sample solution

The Solution to Your Study Problems

Bartleby provides explanations to thousands of textbook problems written by our experts, many with advanced degrees!

Get Started

Additional Science Solutions

Find more solutions based on key concepts

Show solutions add

A diet too low in carbohydrate brings about responses that are similar to fasting.

Nutrition: Concepts and Controversies - Standalone book (MindTap Course List)

What is the monomer of a nucleic acid macromolecule?

Biology: The Dynamic Science (MindTap Course List)