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Chapter 4: Q6 E (page 214)

Write a balanced equation describing each of the following chemical reactions.

(a) Solid potassium chlorate, KClO3 decomposes to form solid potassium chloride and diatomic oxygen gas

(b) Solid aluminium metal reacts with solid diatomic iodine to form solid Al2I6

(c) When solid sodium chloride is added to aqueous sulfuric acid, hydrogen chloride gas and aqueous sodium sulfate are produced.

(d) Aqueous solutions of phosphoric acid and potassium hydroxide react to produce aqueous potassium dihydrogen phosphate and liquid water.

Short Answer

Expert verified

The balanced equations for the chemical reactions are as follows:

(a) \(2KCl{O_3}\left( s \right) \to 2KCl\left( s \right) + 3{O_2}\left( g \right)\)

(b) \(2Al\left( s \right) + 3{I_2}\left( s \right) \to A{l_2}{I_6}\left( s \right)\)

(c) \(2NaCl\left( s \right) + {H_2}S{O_4}(aq) \to 2HCl\left( g \right) + N{a_2}S{O_4}\left( {aq} \right)\)

(d) \({H_3}P{O_4}\left( {aq} \right) + KOH\left( {aq} \right) \to K{H_2}P{O_4}\left( {aq} \right) + {H_2}O\left( l \right)\)

Step by step solution

01

Balanced equation for decomposition of potassium chlorate

The balanced equation is as represented below:

\(2KCl{O_3}\left( s \right) \to 2KCl\left( s \right) + 3{O_2}\left( g \right)\)

Draw the balancing table using the coefficients and subscripts of the formulae.

Element

Reactant

Product

Balanced? yes

K

2×1

2×1

2=2

Cl

2×1

2×1

2=2

O

2×3

3×2

6=6

02

Balanced equation for reaction of aluminium with iodine

The balanced equation is as represented below:

\(2Al\left( s \right) + 3{I_2}\left( s \right) \to A{l_2}{I_6}\left( s \right)\)

Draw the balancing table using the coefficients and subscripts of the reaction formulae.

Element

Reactant

Product

Balanced? yes

Al

2×1

1×2

2=2

I

3×2

1×6

6=6

03

Balanced equation for reaction of sodium chloride with sulfuric acid

The balanced reaction is as given below:

\(2NaCl\left( s \right) + {H_2}S{O_4}(aq) \to 2HCl\left( g \right) + N{a_2}S{O_4}\left( {aq} \right)\)

Draw the balancing table using the coefficients and subscripts of the reaction formulae.

Element

Reactant

Product

Balanced? yes

Na

2×1

1×2

2=2

Cl

2×1

2×1

2=2

S

1×1

1×1

1=1

H

1×2

2×1

2=2

O

1×4

1×4

4=4

04

Balanced equation for reaction of phosphoric acid with potassium hydroxide

The balanced reaction is as given below:

\({H_3}P{O_4}\left( {aq} \right) + KOH\left( {aq} \right) \to K{H_2}P{O_4}\left( {aq} \right) + {H_2}O\left( l \right)\)

Draw the balancing table using the coefficients and subscripts of the reaction formulae.

Element

Reactant

Product

Balanced? yes

K

1×1

1×1

1=1

P

1×1

1×1

1=1

H

1×3+1×1

1×2+1×2

4=4

O

1×4+1×1

1×4+1×1

5=5

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Most popular questions from this chapter

How many molecules of C2H4Cl2 can be prepared from 15 C2H4molecules and 8 Cl2molecules?

Write a balanced molecular equation describing each of the following chemical reactions.

(a) Solid calcium carbonate is heated and decomposes to solid calcium oxide and carbon dioxide gas

(b)Gaseous butane reacts with diatomic oxygen gas to yield gaseous carbon dioxide and water vapor

(c)Aqueous solution of magnesium chloride and sodium hydroxide react to produce solid magnesium hydroxide and aqueous sodium chloride

(d) Water vapor reacts with sodium metal to produce solid sodium hydroxide and hydrogen gas.

What volume of 0.600 M HCl is required to react completely with 2.50 g of sodium hydrogen carbonate?

\({\rm{NaHC}}{{\rm{O}}_{3(aq)}}{\rm{ + HC}}{{\rm{l}}_{(aq)}}{\rm{ }} \to {\rm{ NaC}}{{\rm{l}}_{(aq)}}{\rm{ + C}}{{\rm{O}}_{2(aq)}}{\rm{ + }}{{\rm{H}}_2}{{\rm{O}}_{({\rm{l}})}}\)

Complete and balance the following acid-base equations:

(a) A solution ofHClO4 is added to a solution of LiOH

(b) AqueousH2SO4 reacts withNaOH

(c)Ba(OH)2reacts withHF gas.

Balance the following equations:

\(\begin{array}{l}\left( a \right)\,Ag\left( s \right) + {H_2}S\left( g \right) + {O_2}\left( g \right) \to A{g_2}S\left( s \right) + {H_2}O\left( l \right)\\\left( b \right)\,{P_4}\left( s \right) + {O_2}\left( g \right) \to {P_4}{O_{10}}\left( s \right)\\\left( c \right)\,Pb\left( s \right) + {H_2}O\left( l \right) + {O_2}\left( g \right) \to Pb{\left( {OH} \right)_2}\left( s \right)\\\left( d \right)\,Fe\left( s \right) + {H_2}O\left( l \right) \to F{e_3}{O_4}\left( s \right) + {H_2}\left( g \right)\\\left( e \right)\,S{c_2}{O_3}\left( s \right) + S{O_3}\left( g \right) \to S{c_2}{\left( {S{O_4}} \right)_3}\left( s \right)\\\left( f \right)\,C{a_3}{\left( {P{O_4}} \right)_2}\left( {aq} \right) + {H_3}P{O_4}\left( {aq} \right) \to Ca{\left( {{H_2}P{O_4}} \right)_2}\left( {aq} \right)\\\left( g \right)\,Al\left( s \right) + {H_2}S{O_4}\left( {aq} \right) \to A{l_2}{\left( {S{O_4}} \right)_3}\left( s \right) + {H_2}\left( g \right)\\\left( h \right)\,TiC{l_4}\left( s \right) + {H_2}O\left( g \right) \to Ti{O_2}\left( s \right) + HCl\left( g \right)\end{array}\)
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