   # A balloon holds 30.0 kg of helium. What is the volume of the balloon if its pressure is 1.20 atm and the temperature is 22 °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, Problem 18PS
Textbook Problem
64 views

## A balloon holds 30.0 kg of helium. What is the volume of the balloon if its pressure is 1.20 atm and the temperature is 22 °C?

Interpretation Introduction

Interpretation:

The volume of the balloon should be calculated using the given temperature, amount of gas and pressure.

Concept Introduction:

Different laws have been put forward to introduce properties of gases:

Boyle’s law:

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

P1V(n,Twillbeconstant)

Charles’s law: States that volume is directly proportional to temperature when the gas is held

at constant pressure and number of molecules.

VT

General Gas Law: Combining Charles’s law and Boyle’s law we get the General gas law or combined gas law.

P1V1T1=P2V2T2

• To relate the amount of gas and the volume.
• VnatconstantTandP

Combining all these together ideal gas law is introduced:

PV=nRT

### Explanation of Solution

Ideal gas law: PV=nRT

R=0.0827L.atmK.molTshouldbeexpressedinKPshouldbeexpressedinatm

Given data:

P=1atmT=22°C=22+273=295Km=30kg=30×103gV=?

In-order to calculate the number of moles we can use the equation:

No.ofmoles=massmolarmass=30×10

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