   Chapter 15, Problem 40CR ### 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
5 views

# 40. In an open flask, 20.0 ml. of an aqueous solution (density of solution = 1.103 g/mL) is combined with 13.5 g of a solid, and a chemical reaction takes place. One of the reaction products is 1.473 L of gas with density = 1.798 g/L. What is the mass of the mixture remaining in the flask? (Hint: Think about how the law of conservation of mass applies in this situation.)

Interpretation Introduction

Interpretation:

The mass of the mixture remaining in the flask is to be calculated.

Concept Introduction:

The atomic mass of an element is defined as the sum of number of protons and number of neutrons. Molar mass of an element is determined from atomic mass of an element.

The formula to calculate the number of moles is,

Moles=MassgMolarmass

The mass of any substance is calculated by the formula,

Mass=Volume×Density.

Explanation

It is given that 20.0mL of an aqueous solution is combined with 13.5g of solid.

The density of an aqueous solution is given to be 1.103g/mL.

The mass of an aqueous solution is calculated by the formula,

Mass=Volume×Density (1)

Substitute the values of volume and density of an aqueous solution in the equation (1).

Mass=20.0mL×1.103g/mL=22.06g

The total mass of the solution is calculated as shown below.

Totalmassofsolution=Massofanaqueoussolution+Massofsolid (2)

Substitute the values of masses of an aqueous solution and solid in the equation (2).

Totalmassofsolution=22.06g+13.5g=35

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