   # A large balloon contains 65.0 L of helium gas at 25 °C and a pressure of 745 mm Hg. The balloon ascends to 3000 m, at which the external pressure has decreased by 30.%. What would be the volume of the balloon, assuming it expands so that the internal and external pressures are equal? (Assume the temperature is still 25 °C.) ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

#### Solutions

Chapter
Section ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 10.2, Problem 1CYU
Textbook Problem
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## A large balloon contains 65.0 L of helium gas at 25 °C and a pressure of 745 mm Hg. The balloon ascends to 3000 m, at which the external pressure has decreased by 30.%. What would be the volume of the balloon, assuming it expands so that the internal and external pressures are equal? (Assume the temperature is still 25 °C.)

Interpretation Introduction

Interpretation:

The volume of a gas in a balloon when it expands should be calculated and the initial volume is given.

Concept Introduction:

Boyle’s law:

At fixed temperature, the volume of a fixed amount of gas is inversely proportional to the pressure exerted by the gas.

Pµ1V(n,Twillbeconstant)PV=constantP1V1=P2V2

### Explanation of Solution

Given:

The volume of the gas inside the balloon using the concept of Boyle’s law

V1=65L=65×103mlP1=745mmHgP2=pressuredecreasedby30%(giventhatinternalandexternalpressuresareequal)V2=?

The pressure has decreased by 30%

P2=521

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