   Chapter 13, Problem 94QAP ### 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
1 views

# Consider the following unbalanced chemical equation in which element X is unknown:msp;  X ( s ) + F 2 ( g )   XF 3 ( s ) 9 . 15 g of element X ( s ) is completely reacted with 4 .00  L of fluorine gas at 25 0   ° C and 2 . 5 0 am, what is the identity of X ?

Interpretation Introduction

Interpretation:

The element X should be identified.

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 element X is 9.15 g, volume of fluorine gas is 4.00 L, temperature is 250 C and pressure is 2.50 atm.

Calculation:

The unbalanced chemical equation is as follows:

X(s)+F2(g)XF3(s)

To balanced the above reaction, give coefficient 2 to X, 3 to F2 and 2 to XF3 thus,

2X(s)+3F2(g)2XF3(s)

To identify the element X, its molar mass should be calculated.

First calculate the number of moles of fluorine gas from given temperature and pressure values as follows:

n=PVRT

Convert the given temperature from C to K:

0 C=273.15 K

Thus,

250 C=(250+273.15) K=523.15 K

Putting the values,

n=(2.50 atm)(4

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