IDNLearn.com provides a user-friendly platform for finding answers to your questions. Discover reliable and timely information on any topic from our network of experienced professionals.
Sagot :
To determine which chemical reaction is a redox reaction, we need to examine each reaction and identify if there is a change in the oxidation states of any of the elements involved. A redox reaction involves the transfer of electrons between species, leading to changes in their oxidation states.
Let's go through each of the reactions step by step:
A) [tex]\( 2 \text{HCl} + \text{CaCO}_3 \rightarrow \text{CaCl}_2 + \text{CO}_2 + \text{H}_2\text{O} \)[/tex]
- H in HCl: Oxidation state +1
- Cl in HCl: Oxidation state -1
- Ca in CaCO[tex]\(_3\)[/tex]: Oxidation state +2
- C in CaCO[tex]\(_3\)[/tex]: Oxidation state +4
- O in CaCO[tex]\(_3\)[/tex]: Oxidation state -2
In the products:
- Ca in CaCl[tex]\(_2\)[/tex]: Oxidation state +2
- Cl in CaCl[tex]\(_2\)[/tex]: Oxidation state -1
- C in CO[tex]\(_2\)[/tex]: Oxidation state +4
- O in CO[tex]\(_2\)[/tex]: Oxidation state -2
- H in H[tex]\(_2\text{O}\)[/tex]: Oxidation state +1
- O in H[tex]\(_2\text{O}\)[/tex]: Oxidation state -2
Since there is no change in the oxidation states of the elements, this is not a redox reaction.
B) [tex]\( \text{AgNO}_3 + \text{KCl} \rightarrow \text{AgCl} + \text{KNO}_3 \)[/tex]
- Ag in AgNO[tex]\(_3\)[/tex]: Oxidation state +1
- N in AgNO[tex]\(_3\)[/tex]: Oxidation state +5
- O in AgNO[tex]\(_3\)[/tex]: Oxidation state -2
- K in KCl: Oxidation state +1
- Cl in KCl: Oxidation state -1
In the products:
- Ag in AgCl: Oxidation state +1
- Cl in AgCl: Oxidation state -1
- K in KNO[tex]\(_3\)[/tex]: Oxidation state +1
- N in KNO[tex]\(_3\)[/tex]: Oxidation state +5
- O in KNO[tex]\(_3\)[/tex]: Oxidation state -2
Since there is no change in the oxidation states of the elements, this is not a redox reaction.
C) [tex]\( \text{Ca(OH)}_2 + \text{CO}_2 \rightarrow \text{CaCO}_3 + \text{H}_2\text{O} \)[/tex]
- Ca in Ca(OH)[tex]\(_2\)[/tex]: Oxidation state +2
- O in Ca(OH)[tex]\(_2\)[/tex]: Oxidation state -2
- H in Ca(OH)[tex]\(_2\)[/tex]: Oxidation state +1
- C in CO[tex]\(_2\)[/tex]: Oxidation state +4
- O in CO[tex]\(_2\)[/tex]: Oxidation state -2
In the products:
- Ca in CaCO[tex]\(_3\)[/tex]: Oxidation state +2
- C in CaCO[tex]\(_3\)[/tex]: Oxidation state +4
- O in CaCO[tex]\(_3\)[/tex]: Oxidation state -2
- H in H[tex]\(_2\text{O}\)[/tex]: Oxidation state +1
- O in H[tex]\(_2\text{O}\)[/tex]: Oxidation state -2
Since there is no change in the oxidation states of the elements, this is not a redox reaction.
D) [tex]\( 2 \text{H}_2 + \text{O}_2 \rightarrow 2 \text{H}_2\text{O} \)[/tex]
- H in H[tex]\(_2\)[/tex]: Oxidation state 0 (elemental form)
- O in O[tex]\(_2\)[/tex]: Oxidation state 0 (elemental form)
In the product:
- H in H[tex]\(_2\text{O}\)[/tex]: Oxidation state +1
- O in H[tex]\(_2\text{O}\)[/tex]: Oxidation state -2
Here, the oxidation state of hydrogen changes from 0 to +1 and the oxidation state of oxygen changes from 0 to -2. This indicates that electrons are transferred—hydrogen is oxidized and oxygen is reduced.
Therefore, reaction D is a redox reaction.
Conclusion:
The redox reaction among the given options is:
[tex]\[ 2 \text{H}_2 + \text{O}_2 \rightarrow 2 \text{H}_2\text{O} \][/tex]
The correct answer is D.
Let's go through each of the reactions step by step:
A) [tex]\( 2 \text{HCl} + \text{CaCO}_3 \rightarrow \text{CaCl}_2 + \text{CO}_2 + \text{H}_2\text{O} \)[/tex]
- H in HCl: Oxidation state +1
- Cl in HCl: Oxidation state -1
- Ca in CaCO[tex]\(_3\)[/tex]: Oxidation state +2
- C in CaCO[tex]\(_3\)[/tex]: Oxidation state +4
- O in CaCO[tex]\(_3\)[/tex]: Oxidation state -2
In the products:
- Ca in CaCl[tex]\(_2\)[/tex]: Oxidation state +2
- Cl in CaCl[tex]\(_2\)[/tex]: Oxidation state -1
- C in CO[tex]\(_2\)[/tex]: Oxidation state +4
- O in CO[tex]\(_2\)[/tex]: Oxidation state -2
- H in H[tex]\(_2\text{O}\)[/tex]: Oxidation state +1
- O in H[tex]\(_2\text{O}\)[/tex]: Oxidation state -2
Since there is no change in the oxidation states of the elements, this is not a redox reaction.
B) [tex]\( \text{AgNO}_3 + \text{KCl} \rightarrow \text{AgCl} + \text{KNO}_3 \)[/tex]
- Ag in AgNO[tex]\(_3\)[/tex]: Oxidation state +1
- N in AgNO[tex]\(_3\)[/tex]: Oxidation state +5
- O in AgNO[tex]\(_3\)[/tex]: Oxidation state -2
- K in KCl: Oxidation state +1
- Cl in KCl: Oxidation state -1
In the products:
- Ag in AgCl: Oxidation state +1
- Cl in AgCl: Oxidation state -1
- K in KNO[tex]\(_3\)[/tex]: Oxidation state +1
- N in KNO[tex]\(_3\)[/tex]: Oxidation state +5
- O in KNO[tex]\(_3\)[/tex]: Oxidation state -2
Since there is no change in the oxidation states of the elements, this is not a redox reaction.
C) [tex]\( \text{Ca(OH)}_2 + \text{CO}_2 \rightarrow \text{CaCO}_3 + \text{H}_2\text{O} \)[/tex]
- Ca in Ca(OH)[tex]\(_2\)[/tex]: Oxidation state +2
- O in Ca(OH)[tex]\(_2\)[/tex]: Oxidation state -2
- H in Ca(OH)[tex]\(_2\)[/tex]: Oxidation state +1
- C in CO[tex]\(_2\)[/tex]: Oxidation state +4
- O in CO[tex]\(_2\)[/tex]: Oxidation state -2
In the products:
- Ca in CaCO[tex]\(_3\)[/tex]: Oxidation state +2
- C in CaCO[tex]\(_3\)[/tex]: Oxidation state +4
- O in CaCO[tex]\(_3\)[/tex]: Oxidation state -2
- H in H[tex]\(_2\text{O}\)[/tex]: Oxidation state +1
- O in H[tex]\(_2\text{O}\)[/tex]: Oxidation state -2
Since there is no change in the oxidation states of the elements, this is not a redox reaction.
D) [tex]\( 2 \text{H}_2 + \text{O}_2 \rightarrow 2 \text{H}_2\text{O} \)[/tex]
- H in H[tex]\(_2\)[/tex]: Oxidation state 0 (elemental form)
- O in O[tex]\(_2\)[/tex]: Oxidation state 0 (elemental form)
In the product:
- H in H[tex]\(_2\text{O}\)[/tex]: Oxidation state +1
- O in H[tex]\(_2\text{O}\)[/tex]: Oxidation state -2
Here, the oxidation state of hydrogen changes from 0 to +1 and the oxidation state of oxygen changes from 0 to -2. This indicates that electrons are transferred—hydrogen is oxidized and oxygen is reduced.
Therefore, reaction D is a redox reaction.
Conclusion:
The redox reaction among the given options is:
[tex]\[ 2 \text{H}_2 + \text{O}_2 \rightarrow 2 \text{H}_2\text{O} \][/tex]
The correct answer is D.
Your participation means a lot to us. Keep sharing information and solutions. This community grows thanks to the amazing contributions from members like you. Your questions find answers at IDNLearn.com. Thanks for visiting, and come back for more accurate and reliable solutions.
