Chapter 13, Problem 13E

(a)

To determine

The single-replacement reaction will occur or will not occur in the given reaction: $\text{Na}+\text{KCl}\left(\text{aq}\right)\to \text{K}+\text{NaCl}\left(\text{aq}\right)$

Answer to Problem 13E

The single-replacement reaction will not occur in the given reaction:

$\text{Na}+\text{KCl}\left(\text{aq}\right)\to \text{K}+\text{NaCl}\left(\text{aq}\right)$

Explanation of Solution

Given info: Refer to the table 13.5 in the textbook.

Explanation:

The loss of electrons from an atom or ion is called oxidation. The gain of electrons from an atom is called reduction. When oxidation and reduction reaction occurs simultaneously. The process is called redox reaction.

The activity of metal is determined by its tendency to lose electrons to form ions as compared to another metal or to hydrogen ions.

If an element X is placed above element Y in the activity series, then element X is more active than element Y and will replace Y from compound YZ. This process is called single-replacement reaction.

The reaction between $\text{KCl}$ and $\text{Na}$ is written as,

$\text{Na}+\text{KCl}\left(\text{aq}\right)\to \text{K}+\text{NaCl}\left(\text{aq}\right)$

In the above reaction, an element $\text{K}$ is placed above an element $\text{Na}$ in the activity series, and then $\text{K}$ is more active than $\text{Na}$. Therefore, $\text{Na}$ atom will not replace $\text{K}$ atom from $\text{KCl}$. Therefore, the above reaction will not occur.

Conclusion:

Therefore, The single-replacement reaction will not occur in the given reaction:

$\text{Na}+\text{KCl}\left(\text{aq}\right)\to \text{K}+\text{NaCl}\left(\text{aq}\right)$

(b)

To determine

The single-replacement reaction will occur or will not occur in the given reaction: $\text{Ni}+{\text{CuBr}}_{\text{2}}\left(\text{aq}\right)\to \text{Cu}+{\text{NiBr}}_2\left(\text{aq}\right)$

Answer to Problem 13E

The single-replacement reaction will occur in the given reaction:

$\text{Ni}+{\text{CuBr}}_{\text{2}}\left(\text{aq}\right)\to \text{Cu}+{\text{NiBr}}_2\left(\text{aq}\right)$

Explanation of Solution

Given info: Refer to the table 13.5 in the textbook.

Explanation:

The loss of electrons from an atom or ion is called oxidation. The gain of electrons from an atom is called reduction. When oxidation and reduction reaction occurs simultaneously. The process is called redox reaction.

The activity of metal is determined by its tendency to lose electrons to form ions as compared to another metal or to hydrogen ions.

If an element X is placed above element Y in the activity series, then element X is more active than element Y and will replace Y from compound YZ. This process is called single-replacement reaction.

The reaction between ${\text{CuBr}}_{\text{2}}$ and $\text{Ni}$ is written as,

$\text{Ni}+{\text{CuBr}}_{\text{2}}\left(\text{aq}\right)\to \text{Cu}+{\text{NiBr}}_2\left(\text{aq}\right)$

In the above reaction, an element $\text{Ni}$ is placed above an element $\text{Cu}$ in the activity series, then $\text{Ni}$ is more active than $\text{Cu}$ and replace $\text{Cu}$ from ${\text{CuBr}}_{\text{2}}$. Therefore, the above reaction will occur.

Conclusion:

Therefore, the single-replacement reaction will occur in the given reaction: $\text{Ni}+{\text{CuBr}}_{\text{2}}\left(\text{aq}\right)\to \text{Cu}+{\text{NiBr}}_2\left(\text{aq}\right)$

(c)

To determine

The single-replacement reaction will occur or will not occur in the given reaction: $2\text{Al}+6\text{HCl}\left(\text{aq}\right)\to 3{\text{H}}_{\text{2}}+2{\text{AlCl}}_{\text{3}}\left(\text{aq}\right)$

Answer to Problem 13E

The single-replacement reaction will occur in the given reaction:

$2\text{Al}+6\text{HCl}\left(\text{aq}\right)\to 3{\text{H}}_{\text{2}}+2{\text{AlCl}}_{\text{3}}\left(\text{aq}\right)$

Explanation of Solution

Given info: Refer to the table 13.5 in the textbook.

Explanation:

The loss of electrons from an atom or ion is called oxidation. The gain of electrons from an atom is called reduction. When oxidation and reduction reaction occurs simultaneously. The process is called redox reaction.

The activity of metal is determined by its tendency to lose electrons to form ions as compared to another metal or to hydrogen ions.

If an element X is placed above element Y in the activity series, then element X is more active than element Y and will replace Y from compound YZ. This process is called single-replacement reaction.

The reaction between $\text{HCl}$ and $\text{Al}$ is written as,

$2\text{Al}+6\text{HCl}\left(\text{aq}\right)\to 3{\text{H}}_{\text{2}}+2{\text{AlCl}}_{\text{3}}\left(\text{aq}\right)$

In the above reaction, an element $\text{Al}$ is placed above an element $\text{H}$ in the activity series, then $\text{Al}$ is more active than $\text{H}$ and replace $\text{H}$ from $\text{HCl}$. Therefore, the above reaction will occur.

Conclusion:

Therefore, the single-replacement reaction will occur in the given reaction:

$2\text{Al}+6\text{HCl}\left(\text{aq}\right)\to 3{\text{H}}_{\text{2}}+2{\text{AlCl}}_{\text{3}}\left(\text{aq}\right)$