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Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425

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BuyFindarrow_forward

Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425
Textbook Problem
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. In each of the following reactions, identify which element is being oxidized and which is being reduced by assigning oxidation numbers.

a. Fe ( s ) + CuSO 4 ( aq ) FeSO 4 ( aq ) + Cu ( s )    b. Cl 2 ( g ) + 2NaBr ( aq ) 2NaCl ( aq ) + Br 2 ( l )    c. 3CuS ( s ) + 8HNO 3 ( aq ) 3CuSO 4 ( aq ) + 8NO ( g ) + 4H 2 O ( l ) .

d. 2Zn ( s ) + O 2 ( g ) 2ZnO ( s )

Interpretation Introduction

Interpretation:

The element being oxidized and reduced in the given reaction should be determined.

Concept Introduction:

The oxidation state is defined as the charge(s) that an atom would have when electron(s) were transferred completely from a molecule or ion.

The element being oxidized is the one whose oxidation increases in the reaction whereas the reduced element is the one whose oxidation number decreases in the reaction.

Explanation

Given:

Fe(s) + CuSO4(aq)  FeSO4(aq) + Cu(s)

The oxidation state is defined as the charge(s) that an atom would have when electron(s) were transferred completely from a molecule or ion.

While determining the oxidation state of compound, the element with greater electronegativity is assigned with negative value of oxidation state which is equal to the charge as an anion in ionic compounds and element whose oxidation states are fixed are assigned. For compounds with no charge, the sum of oxidation states is zero.

The oxidation states are determined as:

Since, Fe and Cu are in its stable elemental state so, the oxidation state of each is zero for CuSO4 and FeSO4 the oxidation are determined as:

For CuSO4 :

The oxidation state of SO4 is assigned as -2 and the oxidation state of Cu is assigned as x:

Since, CuSO4 has no charge so; the sum of oxidation state must be zero

Interpretation Introduction

Interpretation:

The element being oxidized and reduced in the given reaction should be determined.

Concept Introduction:

The oxidation state is defined as the charge(s) that an atom would have when electron(s) were transferred completely from a molecule or ion.

The element being oxidized is the one whose oxidation increases in the reaction whereas the reduced element is the one whose oxidation number decreases in the reaction.

Interpretation Introduction

Interpretation:

The element being oxidized and reduced in the given reaction should be determined.

Concept Introduction:

The oxidation state is defined as the charge(s) that an atom would have when electron(s) were transferred completely from a molecule or ion.

The element being oxidized is the one whose oxidation increases in the reaction whereas the reduced element is the one whose oxidation number decreases in the reaction.

Interpretation Introduction

Interpretation:

The element being oxidized and reduced in the given reaction should be determined.

Concept Introduction:

The oxidation state is defined as the charge(s) that an atom would have when electron(s) were transferred completely from a molecule or ion.

The element being oxidized is the one whose oxidation increases in the reaction whereas the reduced element is the one whose oxidation number decreases in the reaction.

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