   Chapter 13, Problem 56QAP ### Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425

#### Solutions

Chapter
Section ### Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425
Textbook Problem
3 views

# Suppose that a 1 . 25 − g sample of neon gas is confined in a 1 0. 1 − L container at 25  ° C . What will be the pressure in the container? Suppose the temperature is then raised 5 0   ° C . What will me new pressure he after the temperature is increased?

Interpretation Introduction

Interpretation:

The initial and final pressure of the container if temperature is increased should be calculated.

Concept Introduction:

According to ideal gas equation:

PV=nRT

Here, P is pressure, V is volume, n is number of moles, R is Universal gas constant and T is temperature.

The value of Universal gas constant can be taken as 0.082 L atm K1 mol1.

Mass of gas can be calculated from number of moles and molar mass as follows:

m=n×M

Here, n is number of moles, m is mass and M is molar mass.

Explanation

Given information:

The mass of neon gas sample is 1.25 g, volume of container is 10.1 L and temperature of gas is 25 C. The temperature is increased to 50 C

To calculate the pressure, first calculate the number of moles of gas as follows:

n=mM

Molar mass of neon gas is 20.18 g/mol.

Putting the values,

n=1.25 g20.18 g/mol=0.062 mol

Using the ideal gas equation, pressure can be calculated as follows:

P=nRTV

Convert the temperature from K to C as follows:

0 C=273.15 K

Thus,

25 C=(25+273.15) K=298.15 K

Putting the value,

P=(0.062 mol)(0.082 L atm K1 mol1)(298

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