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Chapter 4: Q20E (page 217)

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

Short Answer

Expert verified

(a) Mg is oxidised and Ni is reduced,change in oxidation state -Mg (0 to +2) andNi (+2 to 0), Mg is reducing agent and Ni is oxidising agent.

(b) P is oxidised and Cl is reduced, change in oxidation state - P (+3 to +5) and Cl (0 to -1), P is reducing agent and Cl is oxidising agent

(c) C is oxidised and O is reduced, change in oxidation state- C (-2 to +4) and O (0 to -2), C is reducing agent and O is oxidising agent.

(d) Zn is oxidised and H is reduced, change in oxidation state-Zn(0 to +2)and H(+1 to 0), Zn is reducing agent and H is oxidising agent

(e) S is oxidised and I is reduced,change in oxidation state- S(+2 to +2.5) and I (0 to -2), S is reducing agent and I is oxidising agent

(f) Cu is oxidised and N is reduced, change in oxidation state-Cu (0 to +2) and N (+5 to +3), Cu is reducing agent and N is oxidising agent

Step by step solution

01

Consider the reaction (a)

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

Here magnesium is oxidised, hence it is the reducing agent, whereas nickel is reduced, making it the oxidising agent. The change in oxidation state of magnesium is from 0 to +2 and nickel is from +2 to 0.

02

Consider the reaction (b)

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

Here phosphorus is oxidised, hence it is the reducing agent, while chlorine is reduced, making it the oxidising agent.The change in oxidation state of phosphorus is from +3 to +5 and chlorine is from 0 to -1.

03

Consider the reaction (c)

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

Here carbon is oxidised, hence it is the reducing agent, while oxygen is reduced, making it the oxidising agent.The change in oxidation state of carbon is from -2 to +4 and oxygen is from 0 to -2.

04

Consider the reaction (d)

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

Here zinc is oxidised, hence it is the reducing agent, while hydrogen is reduced, making it the oxidising agent.The change in oxidation state of zinc is from 0 to +2 and hydrogen is from +1 to 0.

05

Consider the reaction (e)

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

Here sulfur is oxidised, hence it is the reducing agent, while iodine is reduced, making it the oxidising agent.The change in oxidation state of sulphur is from +2 to +2.5 and iodine is from 0 to -2.

06

Consider the reaction (f)

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

Here copper is oxidised, hence it is the reducing agent, while nitrogen is reduced, making it the oxidising agent.The change in oxidation state of copper is from 0 to +2 and nitrogen is from +5 to +3.

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Most popular questions from this chapter

What volume of a 0.00945 M solution of potassium hydroxide would be required to titrate 50.00 mL of a sample of acid rain with a H2SO4 concentration of 1.23×10-4M

\({{\rm{H}}_2}{\rm{S}}{{\rm{O}}_{4({\rm{aq}})}}{\rm{ + 2KO}}{{\rm{H}}_{({\rm{aq}})}}{\rm{ }} \to {\rm{ }}{{\rm{K}}_2}{\rm{S}}{{\rm{O}}_{4({\rm{aq}})}}{\rm{ + 2}}{{\rm{H}}_2}{{\rm{O}}_{{\rm{(l)}}}}\)

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\(Na{C_2}{O_4} + U{O_2}{\left( {N{O_3}} \right)_2} + 3{H_2}O \to U{O_2}\left( {{C_2}{O_4}} \right) \cdot 3{H_2}O + 2NaN{O_3}\)

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.

Balance the following equations:

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