   Chapter 10, Problem 20PS

Chapter
Section
Textbook Problem

A steel cylinder holds 1.50 g of ethanol, C2H5OH. What is the pressure of the ethanol vapor if the cylinder has a volume of 251 cm3 and the temperature is 250 °C? (Assume all of the ethanol is in the vapor phase at this temperature.)

Interpretation Introduction

Interpretation:

The pressure of ethanol vapour should be calculated using the given temperature, amount and volume.

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

Ideal gas law: PV=nRT

R=0.0827L.atmK.molTshouldbeexpressedinKPshouldbeexpressedinatm

Given data:

P=?T=250°C=250+273=523KV=251cm3=251ml=0.251Lm=1.50gethanol

Molecular mass of ethanol,C2H5OH=46.07g/mol

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

No.ofmoles=massmolarmass=1

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