Answered: A high-altitude balloon contains…

Introduction to Chemical Engineering Thermodynamics

8th Edition

ISBN:9781259696527

Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart

Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart

Chapter1: Introduction

Section: Chapter Questions

Problem 1.1P

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Question

A high-altitude balloon contains helium, whose molar mass is 4.00 g/mol. At the
balloon’s maximum altitude, its volume is 792 m3 and the outside temperature
and pressure are -53.0 °C and 5.00 kPa, respectively. Assume that the helium in the
balloon is in equilibrium with the outside air temperature and pressure.
(a) Use the ideal gas law to find the amount of helium in the balloon at maximum
altitude.
(b) Assuming no loss of helium, what would be the volume of the balloon when it
was launched from the ground, where the air temperature and pressure are 20.0
°C and 101 kPa, respectively?
(c) If the volume of the balloon when it was launched was 65.0 m3, how many moles
of helium were lost during the balloon’s ascent?

Definition Definition Law that is the combined form of Boyle's Law, Charles's Law, and Avogadro's Law. This law is obeyed by all ideal gas. Boyle's Law states that pressure is inversely proportional to volume. Charles's Law states that volume is in direct relation to temperature. Avogadro's Law shows that volume is in direct relation to the number of moles in the gas. The mathematical equation for the ideal gas law equation has been formulated by taking all the equations into account: PV=nRT Where P = pressure of the ideal gas V = volume of the ideal gas n = amount of ideal gas measured in moles R = universal gas constant and its value is 8.314 J.K-1mol-1 T = temperature

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