   Chapter 13, Problem 91QAP ### 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

# Many transition metal salts are hydrates: they contain a fixed number of water molecules bound per formula unit of the salt. For example, copped(II) sulfate most commonly exists as the pentahydrate, CuSO 4 .  5H 2 O .  If 5 .00  g of CuSO 4 . 5H 2 O is heated strongly so as to drive off all of the waters of hydration as water vapor, what volume will this water vapor occupy at 35 0.   ° C and a pressure of 1 .0 4 atm?

Interpretation Introduction

Interpretation:

The volume of water vapour at 350 C and 1.04 atm 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: Mass of hydrated copper (II) sulfate CuSO4.5H2O is 5.00 g.

Calculation:

The balanced chemical reaction is as follows:

CuSO4.5H2OΔCuSO4+5H2O

From the balanced chemical reaction, 1 mol of CuSO4.5H2O produced 5 mol of H2O. To calculate the volume of water vapour, first calculate the number of moles of CuSO4.5H2O and water vapour as follows:

n=mM

Molar mass of CuSO4.5H2O is 249.72 g/mol thus,

n=5 g249.72 g/mol=0.02 mol

Thus, number of moles of water vapour produced will be 0

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