Why the electrolysis of water is not the best method to produce hydrogen gas has to be reasoned. Concept Introduction: In any electrochemical reaction, an electron goes from one substance to another substance driven by the oxidation-reduction reaction. Electrochemical cells have two conducting electrodes, called the anode and cathode. The anode is defined as the electrode where oxidation occurs. The cathode is the electrode where reduction takes place. Standard electrode potential ( E ° c e l l ) can be calculated for both oxidation and reduction reactions. A positive value of ( E ° c e l l ) indicates that the reaction proceeds spontaneously in the forward direction whereas, a negative value of ( E ° c e l l ) indicates that the reaction proceeds spontaneously in backward direction. The standard cell potential expression is written as follows, E ° c e l l = E ° c a t h o d e + E ° a n o d e

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Answer 1

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Chapter 8, Problem 43Q

Interpretation Introduction

Interpretation:

Why the electrolysis of water is not the best method to produce hydrogen gas has to be reasoned.

Concept Introduction:

In any electrochemical reaction, an electron goes from one substance to another substance driven by the oxidation-reduction reaction. Electrochemical cells have two conducting electrodes, called the anode and cathode. The anode is defined as the electrode where oxidation occurs. The cathode is the electrode where reduction takes place. Standard electrode potential (E° cell) can be calculated for both oxidation and reduction reactions. A positive value of (E° cell) indicates that the reaction proceeds spontaneously in the forward direction whereas, a negative value of (E° cell) indicates that the reaction proceeds spontaneously in backward direction. The standard cell potential expression is written as follows,

E° cell = E° cathode + E° anode

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Answer 2

Question

Chapter 8, Problem 43Q

Interpretation Introduction

Interpretation:

Why the electrolysis of water is not the best method to produce hydrogen gas has to be reasoned.

Concept Introduction:

In any electrochemical reaction, an electron goes from one substance to another substance driven by the oxidation-reduction reaction. Electrochemical cells have two conducting electrodes, called the anode and cathode. The anode is defined as the electrode where oxidation occurs. The cathode is the electrode where reduction takes place. Standard electrode potential (E° cell) can be calculated for both oxidation and reduction reactions. A positive value of (E° cell) indicates that the reaction proceeds spontaneously in the forward direction whereas, a negative value of (E° cell) indicates that the reaction proceeds spontaneously in backward direction. The standard cell potential expression is written as follows,

E° cell = E° cathode + E° anode

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Answer 3

Question

Chapter 8, Problem 43Q

Interpretation Introduction

Interpretation:

Why the electrolysis of water is not the best method to produce hydrogen gas has to be reasoned.

Concept Introduction:

In any electrochemical reaction, an electron goes from one substance to another substance driven by the oxidation-reduction reaction. Electrochemical cells have two conducting electrodes, called the anode and cathode. The anode is defined as the electrode where oxidation occurs. The cathode is the electrode where reduction takes place. Standard electrode potential (E° cell) can be calculated for both oxidation and reduction reactions. A positive value of (E° cell) indicates that the reaction proceeds spontaneously in the forward direction whereas, a negative value of (E° cell) indicates that the reaction proceeds spontaneously in backward direction. The standard cell potential expression is written as follows,

E° cell = E° cathode + E° anode

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Answer 4

Question

Chapter 8, Problem 43Q

Interpretation Introduction

Interpretation:

Why the electrolysis of water is not the best method to produce hydrogen gas has to be reasoned.

Concept Introduction:

In any electrochemical reaction, an electron goes from one substance to another substance driven by the oxidation-reduction reaction. Electrochemical cells have two conducting electrodes, called the anode and cathode. The anode is defined as the electrode where oxidation occurs. The cathode is the electrode where reduction takes place. Standard electrode potential (E° cell) can be calculated for both oxidation and reduction reactions. A positive value of (E° cell) indicates that the reaction proceeds spontaneously in the forward direction whereas, a negative value of (E° cell) indicates that the reaction proceeds spontaneously in backward direction. The standard cell potential expression is written as follows,

E° cell = E° cathode + E° anode

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Answer 5

Chapter 8, Problem 43Q

Interpretation Introduction

Interpretation:

Why the electrolysis of water is not the best method to produce hydrogen gas has to be reasoned.

Concept Introduction:

In any electrochemical reaction, an electron goes from one substance to another substance driven by the oxidation-reduction reaction. Electrochemical cells have two conducting electrodes, called the anode and cathode. The anode is defined as the electrode where oxidation occurs. The cathode is the electrode where reduction takes place. Standard electrode potential (E° cell) can be calculated for both oxidation and reduction reactions. A positive value of (E° cell) indicates that the reaction proceeds spontaneously in the forward direction whereas, a negative value of (E° cell) indicates that the reaction proceeds spontaneously in backward direction. The standard cell potential expression is written as follows,

E° cell = E° cathode + E° anode

Answer 6

Chapter 8, Problem 43Q

Interpretation Introduction

Interpretation:

Why the electrolysis of water is not the best method to produce hydrogen gas has to be reasoned.

Concept Introduction:

In any electrochemical reaction, an electron goes from one substance to another substance driven by the oxidation-reduction reaction. Electrochemical cells have two conducting electrodes, called the anode and cathode. The anode is defined as the electrode where oxidation occurs. The cathode is the electrode where reduction takes place. Standard electrode potential (E° cell) can be calculated for both oxidation and reduction reactions. A positive value of (E° cell) indicates that the reaction proceeds spontaneously in the forward direction whereas, a negative value of (E° cell) indicates that the reaction proceeds spontaneously in backward direction. The standard cell potential expression is written as follows,

E° cell = E° cathode + E° anode

Answer 7

Chapter 8, Problem 43Q

Interpretation Introduction

Interpretation:

Why the electrolysis of water is not the best method to produce hydrogen gas has to be reasoned.

Concept Introduction:

In any electrochemical reaction, an electron goes from one substance to another substance driven by the oxidation-reduction reaction. Electrochemical cells have two conducting electrodes, called the anode and cathode. The anode is defined as the electrode where oxidation occurs. The cathode is the electrode where reduction takes place. Standard electrode potential (E° cell) can be calculated for both oxidation and reduction reactions. A positive value of (E° cell) indicates that the reaction proceeds spontaneously in the forward direction whereas, a negative value of (E° cell) indicates that the reaction proceeds spontaneously in backward direction. The standard cell potential expression is written as follows,

E° cell = E° cathode + E° anode

Answer 8

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Answer 11

Ch. 8.1 - Prob. 8.3YT Ch. 8.1 - Prob. 8.4YT Ch. 8.3 - Prob. 8.9CT Ch. 8.4 - Prob. 8.10CT Ch. 8.4 - Prob. 8.11SC Ch. 8.5 - Prob. 8.13SC Ch. 8.5 - Prob. 8.14CT Ch. 8.6 - Prob. 8.16CT Ch. 8.7 - Prob. 8.17CT Ch. 8.7 - Prob. 8.18YT

Solution Summary: The author explains why electrolysis of water is not the best method to produce hydrogen gas.

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