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Chapter 4: Q3 E (page 214)

Balance the following equations:

\(\begin{array}{l}\;(a)\;PC{l_5}\left( s \right) + {H_2}O\left( l \right) \to POC{l_3}\left( l \right) + HCl\left( {aq} \right)\\\left( b \right)\,Cu\left( s \right) + HN{O_3}\left( {aq} \right) \to Cu{\left( {N{O_3}} \right)_2}\left( {aq} \right) + {H_2}O\left( l \right) + NO\left( g \right)\\\left( c \right){H_2}\left( g \right) + {I_2}\left( g \right) \to HI\left( s \right)\\\left( d \right)\,Fe\left( s \right) + {O_2}\left( g \right) \to F{e_2}{O_3}\left( s \right)\\\left( e \right)\,Na\left( s \right) + {H_2}O\left( l \right) \to NaOH\left( {aq} \right) + {H_2}\left( g \right)\\\left( f \right)\,{\left( {N{H_4}} \right)_2}C{r_2}{O_7}\left( s \right) \to C{r_2}{O_3}\left( s \right) + {N_2}\left( g \right) + {H_2}O\left( g \right)\\\left( g \right){P_4}\left( s \right) + C{l_2}\left( g \right) \to PC{l_3}\left( l \right)\\\left( h \right)PtC{l_4}\left( s \right) \to Pt\left( s \right) + C{l_2}\left( g \right)\end{array}\)

Short Answer

Expert verified

\(\begin{array}{l}\;\left( a \right)\;PC{l_5}\left( s \right) + {H_2}O\left( l \right) \to POC{l_3}\left( l \right) + 2HCl\left( {aq} \right)\\\left( b \right)\,3Cu\left( s \right) + 8HN{O_3}\left( {aq} \right) \to 3Cu{\left( {N{O_3}} \right)_2}\left( {aq} \right) + 4{H_2}O\left( l \right) + 2NO\left( g \right)\\\left( c \right){H_2}\left( g \right) + {I_2}\left( g \right) \to HI\left( s \right)\\\left( d \right)\,4Fe\left( s \right) + 3{O_2}\left( g \right) \to 2F{e_2}{O_3}\left( s \right)\\\left( e \right)\,2Na\left( s \right) + 2{H_2}O\left( l \right) \to 2NaOH\left( {aq} \right) + {H_2}\left( g \right)\\\left( f \right)\,{\left( {N{H_4}} \right)_2}C{r_2}{O_7}\left( s \right) \to C{r_2}{O_3}\left( s \right) + {N_2}\left( g \right) + 4{H_2}O\left( g \right)\\\left( g \right){P_4}\left( s \right) + 6C{l_2}\left( g \right) \to 4PC{l_3}\left( l \right)\\\left( h \right)PtC{l_4}\left( s \right) \to Pt\left( s \right) + 2C{l_2}\left( g \right)\end{array}\)

Step by step solution

01

Balance equation of part (a)

\(\left( a \right){\rm{\;PC}}{{\rm{l}}_5}\left( s \right) + {{\rm{H}}_2}{\rm{O}}\left( l \right) \to POC{l_3}\left( l \right) + 2HCl\left( {aq} \right)\)

First balance phosphorous and chlorine followed by hydrogen and oxygen

Draw balancing table for the equation:

Element

Reactant

Product

Balanced? yes

P

1×1

1×1

1=1

Cl

1×5

1×3+2×1

5=5

H

1×2

2×1

2=2

O

1×1

1×1

1=1

02

Balance equation of part (b)

\(\left( b \right)\,3Cu\left( s \right) + 8HN{O_3}\left( {aq} \right) \to 3Cu{\left( {N{O_3}} \right)_2}\left( {aq} \right) + 4{H_2}O\left( l \right) + 2NO\left( g \right)\)

First balance copper, nitrogen followed by hydrogen and oxygen

Draw balancing table for the equation:

Element

Reactant

Product

Balanced? yes

Cu

3×1

3×1

3=3

N

8×1

3×2+2×1

8=8

H

8×1

4×2

2=2

O

8×3

3×6+4×1+2×1

24=24

03

Balance equation of part (c)

\(\left( c \right){H_2}\left( g \right) + {I_2}\left( g \right) \to HI\left( s \right)\)

First balance iodine and hydrogen

Draw balancing table for the equation:

Element

Reactant

Product

Balanced? yes

I

1×2

2×1

2=2

H

1×2

2×1

2=2

04

Balance equation of part (d)

\(\left( d \right)\,4Fe\left( s \right) + 3{O_2}\left( g \right) \to 2F{e_2}{O_3}\left( s \right)\)

First balance iron and oxygen

Draw balancing table for the equation:

Element

Reactant

Product

Balanced? yes

Fe

4×1

2×2

4=4

O

3×2

2×3

6=6

05

Balance equation of part (e)

\(\left( e \right)\,2Na\left( s \right) + 2{H_2}O\left( l \right) \to 2NaOH\left( {aq} \right) + {H_2}\left( g \right)\)

First balance sodium and hydrogen followed by oxygen

Draw balancing table for the equation:

Element

Reactant

Product

Balanced? yes

Na

2×1

2×1

2=2

H

2×2

2×1+1×2

4=4

O

2×1

2×1

2=2

06

Balance equation of part (f)

\(\left( f \right)\,{\left( {N{H_4}} \right)_2}C{r_2}{O_7}\left( s \right) \to C{r_2}{O_3}\left( s \right) + {N_2}\left( g \right) + 4{H_2}O\left( g \right)\)

First balance chromium, nitrogen followed by hydrogen and oxygen

Draw balancing table for the equation:

Element

Reactant

Product

Balanced? yes

Cr

1×2

1×2

2=2

N

1×2

1×2

2=2

H

1×8

4×2

8=8

O

1×7

1×3+4×1

7=7

07

Balance equation of part (g)

\(\left( g \right){P_4}\left( s \right) + 6C{l_2}\left( g \right) \to 4PC{l_3}\left( l \right)\)

First balance chlorine and then phosphorus

Draw balancing table for the equation:

Element

Reactant

Product

Balanced? yes

Cl

6×2

4×3

12=12

P

1×4

4×1

4 = 4

08

Balance equation of part (h) 

\(\left( h \right)PtC{l_4}\left( s \right) \to Pt\left( s \right) + 2C{l_2}\left( g \right)\)

First balance chlorine

Draw balancing table for the equation:

Element

Reactant

Product

Balanced? yes

Cl

1×4

2×2

4=4

Pt

1×1

1×1

1=1

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Most popular questions from this chapter

Identify the atoms that are oxidized and reduced, the change in the oxidation state for each, and the oxidizing and reducing agents in each of the following equations:

(a)\(Mg\left( s \right) + NiC{l_2}\left( {aq} \right) \to MgC{l_2}\left( {aq} \right) + Ni\left( s \right)\)

(b)\(PC{l_3}\left( l \right) + C{l_2}\left( g \right) \to PC{l_5}\left( s \right)\)

(c)\({C_2}{H_4}\left( g \right) + 3{O_2}\left( g \right) \to 2C{O_2}\left( g \right) + 2{H_2}O\left( g \right)\)

(d)\(Zn\left( s \right) + {H_2}S{O_4}\left( {aq} \right) \to ZnS{O_4}\left( {aq} \right) + {H_2}\left( g \right)\)

(e) \(2{K_2}{S_2}{O_3}\left( s \right) + {I_2}\left( s \right) \to {K_2}{S_4}{O_6}\left( s \right) + 2KI\left( s \right)\)

(f) \(3Cu\left( s \right) + 8HN{O_3}\left( {aq} \right) \to 3Cu{\left( {N{O_3}} \right)_2}\left( {aq} \right) + 2NO\left( g \right) + 4{H_2}O\left( l \right)\)

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.

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 mass of gallium oxide Ga2O3 can be prepared from 29 g of gallium metal? The equation for the reaction is \(4Ga + 3{O_2} \to 2G{a_2}{O_3}\)

Indicate what type or types of reaction each of the following represents:

(a) \(\)\(Ca\left( s \right) + B{r_2}\left( l \right) \to CaB{r_2}\left( s \right)\)

(b) \(Ca{\left( {OH} \right)_2} + 2HBr\left( {aq} \right) \to CaB{r_2}\left( {aq} \right) + 2{H_2}O\left( l \right)\)

(c) \({C_6}{H_{12}}\left( l \right) + 9{O_2}\left( g \right) \to 6C{O_2}\left( g \right) + 6{H_2}O\left( l \right)\)\(\)
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