   Chapter 9, Problem 47QAP ### 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
19 views

# For each of the following unbalanced chemical equations, suppose 10.0 g of each reactant is taken. Show by calculation which reactant is the limiting reagent. Calculate the mass of each product that is expected.msp;  C 3 H 8 ( g ) + O 2 ( g ) → CO 2 ( g ) + H 2 O ( g ) msp;  Al ( s ) + Cl 2 ( g ) → AlCl 3 ( s ) msp;  NaOH ( s ) + CO 2 ( g ) → Na 2 CO 3 ( s ) + H 2 O ( l ) msp;  NaHCO 3 ( s ) + HCl ( a q ) → NaCl ( a q ) + H 2 O ( l ) + CO 2 ( g )

Interpretation Introduction

(a)

Interpretation:

Chemical equations have to be correctly balanced and molar ratios of the reactants have to be determined. By finding the number of moles of the reactants available along with molar ratios of the reactants, limiting regent can be determined. From the balanced chemical equation, moles of the products can be determined. According to the balanced chemical equation of this reaction, C3 H8 (g) and O2 (g) reacts in a molar ratio of 1:5.

Concept Introduction:

Number of moles of a given mass of a substance can be determined using the molar masses of the compounds. Reactants undergo chemical reactions in a proper molar ratio, which can be determined by balancing the chemical equations.

Explanation

Given information:

The masses of the reactants are given with the unbalanced equations.

moles=MassMM

MM = molar mass

Reaction 1

C3 H8 (g) + 5 O2 (g) ( 3 CO2 (g) + 4 H2 O(g)

Molar mass of C3 H8

= (12×3)+(1×8)

= 44 g/mol

Molar mass of O2

= 16×2

= 32 g/mol

Molar mass of CO2

= (12×1)+(16×2)

= 44 g/mol

Molar mass of H2 O

= (1*2)+16

= 18 g/mol

C3 H8 moles

= 1044

= 0

Interpretation Introduction

(b)

Interpretation:

Chemical equations have to be correctly balanced and molar ratios of the reactants have to be determined. By finding the number of moles of the reactants available along with molar ratios of the reactants, limiting regent can be determined. From the balanced chemical equation, moles of the products can be determined. According to the balanced chemical equation of this reaction, Al(s) and Cl2 (g) reacts in a molar ratio of 2:3.

Concept Introduction:

Number of moles of a given mass of a substance can be determined using the molar masses of the compounds. Reactants undergo chemical reactions in a proper molar ratio, which can be determined by balancing the chemical equations.

Interpretation Introduction

(c)

Interpretation:

Chemical equations have to be correctly balanced and molar ratios of the reactants have to be determined. By finding the number of moles of the reactants available along with molar ratios of the reactants, limiting regent can be determined. From the balanced chemical equation, moles of the products can be determined. According to the balanced chemical equation of this reaction, NaOH(s) and CO2 (g) reacts in a molar ratio of 2:1.

Concept Introduction:

Number of moles of a given mass of a substance can be determined using the molar masses of the compounds. Reactants undergo chemical reactions in a proper molar ratio, which can be determined by balancing the chemical equations.

Interpretation Introduction

(d)

Interpretation:

Chemical equations have to be correctly balanced and molar ratios of the reactants have to be determined. By finding the number of moles of the reactants available along with molar ratios of the reactants, limiting regent can be determined. From the balanced chemical equation, moles of the products can be determined. According to the balanced chemical equation of this reaction, NaHCO3 (s) and HCl(aq) reacts in a molar ratio of 1:1.

Concept Introduction:

Number of moles of a given mass of a substance can be determined using the molar masses of the compounds. Reactants undergo chemical reactions in a proper molar ratio, which can be determined by balancing the chemical equations.

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