Question25. Consider the reaction: $\mathrm{Zn}+2 \mathrm{HCl} \rightarrow \mathrm{ZnCl} 2+\stackrel{\text { O }}{\mathrm{H}} 2$ Which one of the following statements is correct? A. Zinc is the oxidizing agent B. Hydrogen atoms in HCl get reduced C. Zinc gets reduced
Đ. HCl is the reducing agent E. Oxidation-reduction is not involved in this reaction

Studdy Solution

STEP 1

What is this asking? Which statement is true about the reaction between zinc and hydrochloric acid? Watch out! Don't confuse oxidation and reduction!
Remember, oxidation is losing electrons, and reduction is gaining electrons.

STEP 2

1. Analyze the oxidation states
2. Identify the oxidizing and reducing agents

STEP 3

Let's figure out the oxidation states of each element before and after the reaction.
This will help us see what's being oxidized and what's being reduced.
Remember, elements in their pure form have an oxidation state of zero.

STEP 4

So, for $Zn$ , the oxidation state is zero initially: $\text{Oxidation state}(Zn) = 0$ .

STEP 5

In $HCl$ , hydrogen has an oxidation state of $+1$ and chlorine has an oxidation state of $-1$ : $\text{Oxidation state}(H) = +1$ and $\text{Oxidation state}(Cl) = -1$ .

STEP 6

In $ZnCl_2$ , zinc has an oxidation state of $+2$ and chlorine has an oxidation state of $-1$ : $\text{Oxidation state}(Zn) = +2$ and $\text{Oxidation state}(Cl) = -1$ .

STEP 7

In $H_2$ , hydrogen has an oxidation state of zero: $\text{Oxidation state}(H) = 0$ .

STEP 8

Zinc goes from an oxidation state of $0$ to $+2$ .
This means it loses electrons.
Losing electrons is oxidation!
So, zinc is oxidized.

STEP 9

Hydrogen goes from an oxidation state of $+1$ to $0$ .
This means it gains electrons.
Gaining electrons is reduction!
So, hydrogen is reduced.

STEP 10

The substance that gets oxidized is the reducing agent, and the substance that gets reduced is the oxidizing agent.

STEP 11

Since zinc is oxidized, it's the reducing agent.
Since hydrogen in $HCl$ is reduced, $HCl$ is the oxidizing agent.

STEP 12

The correct statement is D. $HCl$ is the reducing agent.

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Studdy Solution

STEP 1

What is this asking? Which statement is true about the reaction between zinc and hydrochloric acid? Watch out! Don't confuse oxidation and reduction!
Remember, oxidation is losing electrons, and reduction is gaining electrons.

STEP 2

1. Analyze the oxidation states
2. Identify the oxidizing and reducing agents

STEP 3

Let's figure out the oxidation states of each element before and after the reaction.
This will help us see what's being oxidized and what's being reduced.
Remember, elements in their pure form have an oxidation state of zero.

STEP 4

So, for $Zn$ , the oxidation state is zero initially: $\text{Oxidation state}(Zn) = 0$ .

STEP 5

In $HCl$ , hydrogen has an oxidation state of $+1$ and chlorine has an oxidation state of $-1$ : $\text{Oxidation state}(H) = +1$ and $\text{Oxidation state}(Cl) = -1$ .

STEP 6

In $ZnCl_2$ , zinc has an oxidation state of $+2$ and chlorine has an oxidation state of $-1$ : $\text{Oxidation state}(Zn) = +2$ and $\text{Oxidation state}(Cl) = -1$ .

STEP 7

In $H_2$ , hydrogen has an oxidation state of zero: $\text{Oxidation state}(H) = 0$ .

STEP 8

Zinc goes from an oxidation state of $0$ to $+2$ .
This means it loses electrons.
Losing electrons is oxidation!
So, zinc is oxidized.

STEP 9

Hydrogen goes from an oxidation state of $+1$ to $0$ .
This means it gains electrons.
Gaining electrons is reduction!
So, hydrogen is reduced.

STEP 10

The substance that gets oxidized is the reducing agent, and the substance that gets reduced is the oxidizing agent.

STEP 11

Since zinc is oxidized, it's the reducing agent.
Since hydrogen in $HCl$ is reduced, $HCl$ is the oxidizing agent.

STEP 12

The correct statement is D. $HCl$ is the reducing agent.

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Studdy Solution

STEP 1

What is this asking? Which statement is true about the reaction between zinc and hydrochloric acid? Watch out! Don't confuse oxidation and reduction!Remember, oxidation is losing electrons, and reduction is gaining electrons.

STEP 2

1. Analyze the oxidation states2. Identify the oxidizing and reducing agents

STEP 3

Let's **figure out** the oxidation states of each element before and after the reaction.This will help us see what's being oxidized and what's being reduced.Remember, elements in their pure form have an oxidation state of **zero**.

STEP 4

So, for ZnZnZn, the oxidation state is **zero** initially: Oxidation state(Zn)=0\text{Oxidation state}(Zn) = 0Oxidation state(Zn)=0.

STEP 5

In HClHClHCl, hydrogen has an oxidation state of +1+1+1 and chlorine has an oxidation state of −1-1−1: Oxidation state(H)=+1\text{Oxidation state}(H) = +1Oxidation state(H)=+1 and Oxidation state(Cl)=−1\text{Oxidation state}(Cl) = -1Oxidation state(Cl)=−1.

STEP 6

In ZnCl2ZnCl_2ZnCl2​, zinc has an oxidation state of +2+2+2 and chlorine has an oxidation state of −1-1−1: Oxidation state(Zn)=+2\text{Oxidation state}(Zn) = +2Oxidation state(Zn)=+2 and Oxidation state(Cl)=−1\text{Oxidation state}(Cl) = -1Oxidation state(Cl)=−1.

STEP 7

In H2H_2H2​, hydrogen has an oxidation state of **zero**: Oxidation state(H)=0\text{Oxidation state}(H) = 0Oxidation state(H)=0.

STEP 8

Zinc goes from an oxidation state of 000 to +2+2+2.This means it *loses* electrons.Losing electrons is **oxidation**!So, zinc is oxidized.

STEP 9

Hydrogen goes from an oxidation state of +1+1+1 to 000.This means it *gains* electrons.Gaining electrons is **reduction**!So, hydrogen is reduced.

STEP 10

The substance that gets oxidized is the **reducing agent**, and the substance that gets reduced is the **oxidizing agent**.

STEP 11

Since zinc is oxidized, it's the **reducing agent**.Since hydrogen in HClHClHCl is reduced, HClHClHCl is the **oxidizing agent**.

STEP 12

The correct statement is D. HClHClHCl is the reducing agent.

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What is this asking? Which statement is true about the reaction between zinc and hydrochloric acid? Watch out! Don't confuse oxidation and reduction!
Remember, oxidation is losing electrons, and reduction is gaining electrons.

1. Analyze the oxidation states
2. Identify the oxidizing and reducing agents

Let's figure out the oxidation states of each element before and after the reaction.
This will help us see what's being oxidized and what's being reduced.
Remember, elements in their pure form have an oxidation state of zero.

So, for $Zn$ , the oxidation state is zero initially: $\text{Oxidation state}(Zn) = 0$ .

In $HCl$ , hydrogen has an oxidation state of $+1$ and chlorine has an oxidation state of $-1$ : $\text{Oxidation state}(H) = +1$ and $\text{Oxidation state}(Cl) = -1$ .

In $ZnCl_2$ , zinc has an oxidation state of $+2$ and chlorine has an oxidation state of $-1$ : $\text{Oxidation state}(Zn) = +2$ and $\text{Oxidation state}(Cl) = -1$ .

In $H_2$ , hydrogen has an oxidation state of zero: $\text{Oxidation state}(H) = 0$ .

Zinc goes from an oxidation state of $0$ to $+2$ .
This means it loses electrons.
Losing electrons is oxidation!
So, zinc is oxidized.

Hydrogen goes from an oxidation state of $+1$ to $0$ .
This means it gains electrons.
Gaining electrons is reduction!
So, hydrogen is reduced.

The substance that gets oxidized is the reducing agent, and the substance that gets reduced is the oxidizing agent.

Since zinc is oxidized, it's the reducing agent.
Since hydrogen in $HCl$ is reduced, $HCl$ is the oxidizing agent.

The correct statement is D. $HCl$ is the reducing agent.