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Fe2O3 + 2Al → Al2O3 + 2Fe
The above reaction is an example of a:- a)Decomposition reaction
- b)Combination reaction
- c)Displacement reaction
- d)Single displacement reaction
Correct answer is option 'C'. Can you explain this answer?
Fe2O3 + 2Al → Al2O3 + 2Fe
The above reaction is an example of a:
The above reaction is an example of a:
a)
Decomposition reaction
b)
Combination reaction
c)
Displacement reaction
d)
Single displacement reaction
|
Anushka Chopra answered |
The given equation is a displacement reaction in which Fe of Fe2O3 has been displaced by Al. Hence, (c) is the correct option.
Which of the following is an example of displacement reaction?- a)4 Na+ O2 → 2 Na2O
- b)2 Cu + O2 → 2 CuO
- c)Mg + 2 HCl → MgCl2 + H2
- d)N2 + 3 H2 → 2 NH3
Correct answer is option 'C'. Can you explain this answer?
Which of the following is an example of displacement reaction?
a)
4 Na+ O2 → 2 Na2O
b)
2 Cu + O2 → 2 CuO
c)
Mg + 2 HCl → MgCl2 + H2
d)
N2 + 3 H2 → 2 NH3
|
Pooja Shah answered |
It is a single replacement reaction.
Mg + 2HCl → MgCl2 + H2
Mg + 2HCl → MgCl2 + H2
Which of the following metals comes above zinc in reactivity series?
- a)Silver
- b)Copper
- c)Aluminium
- d)Iron
Correct answer is option 'C'. Can you explain this answer?
Which of the following metals comes above zinc in reactivity series?
a)
Silver
b)
Copper
c)
Aluminium
d)
Iron
|
Karthik murthy answered |
Reactivity Series:
The reactivity series is a list of metals arranged in order of their decreasing reactivity. The most reactive metal is placed at the top and the least reactive metal is placed at the bottom of the series.
The reactivity series of metals is as follows:
Potassium > Sodium > Calcium > Magnesium > Aluminium > Zinc > Iron > Lead > Copper > Silver > Gold
Explanation:
Aluminium is more reactive than zinc and is placed above zinc in the reactivity series. This is because aluminium has a stronger tendency than zinc to lose electrons and form positive ions.
When aluminium is exposed to air, it reacts with oxygen to form a layer of aluminium oxide. This layer of oxide is very thin and is also very stable. It prevents further reaction of aluminium with oxygen and protects the metal from corrosion.
Zinc, on the other hand, reacts with oxygen in the air to form zinc oxide. However, the layer of oxide formed on zinc is not as stable as the layer of oxide formed on aluminium. Therefore, zinc is more susceptible to corrosion than aluminium.
Conclusion:
In conclusion, aluminium is more reactive than zinc and is placed above zinc in the reactivity series. This means that aluminium can displace zinc from its compounds in a chemical reaction, but zinc cannot displace aluminium from its compounds.
The reactivity series is a list of metals arranged in order of their decreasing reactivity. The most reactive metal is placed at the top and the least reactive metal is placed at the bottom of the series.
The reactivity series of metals is as follows:
Potassium > Sodium > Calcium > Magnesium > Aluminium > Zinc > Iron > Lead > Copper > Silver > Gold
Explanation:
Aluminium is more reactive than zinc and is placed above zinc in the reactivity series. This is because aluminium has a stronger tendency than zinc to lose electrons and form positive ions.
When aluminium is exposed to air, it reacts with oxygen to form a layer of aluminium oxide. This layer of oxide is very thin and is also very stable. It prevents further reaction of aluminium with oxygen and protects the metal from corrosion.
Zinc, on the other hand, reacts with oxygen in the air to form zinc oxide. However, the layer of oxide formed on zinc is not as stable as the layer of oxide formed on aluminium. Therefore, zinc is more susceptible to corrosion than aluminium.
Conclusion:
In conclusion, aluminium is more reactive than zinc and is placed above zinc in the reactivity series. This means that aluminium can displace zinc from its compounds in a chemical reaction, but zinc cannot displace aluminium from its compounds.
The reaction, Zn + 2HCl → ZnCl2 + H2 is an example of:- a)Displacement reaction
- b)Combination reaction
- c)Double displacement reaction
- d)Decomposition reaction
Correct answer is option 'A'. Can you explain this answer?
The reaction, Zn + 2HCl → ZnCl2 + H2 is an example of:
a)
Displacement reaction
b)
Combination reaction
c)
Double displacement reaction
d)
Decomposition reaction
|
Neha Patel answered |
This is a metal/acid reaction if carried out in aqueous solution.
It is also a displacement reaction where 1 atom of Zinc displaces 2 H+ ions
and it is a redox reaction as the Zn atom loses electrons (it is OXIDISED) and the 2 H+ ions gain electrons (they are REDUCED)
The reaction between lead nitrate and potassium iodide is an example of _______ .- a)decomposition reaction
- b)double displacement reaction
- c)combustion reaction
- d)combination reaction
Correct answer is option 'B'. Can you explain this answer?
The reaction between lead nitrate and potassium iodide is an example of _______ .
a)
decomposition reaction
b)
double displacement reaction
c)
combustion reaction
d)
combination reaction
|
Subset Academy answered |
Lead nitrate reacts with Potassium iodide to form Lead iodide and Potassium nitrate.
Pb(NO3)2 + 2KI → PbI2 + 2KNO3
The given reaction indicates that:
Cu + 2AgNO3 → Cu(NO3)2 + 2Ag- a)Copper is more reactive than silver.
- b)Silver is more reactive than copper.
- c)Both are equally reactive.
- d)None of these
Correct answer is option 'A'. Can you explain this answer?
The given reaction indicates that:
Cu + 2AgNO3 → Cu(NO3)2 + 2Ag
Cu + 2AgNO3 → Cu(NO3)2 + 2Ag
a)
Copper is more reactive than silver.
b)
Silver is more reactive than copper.
c)
Both are equally reactive.
d)
None of these
|
Malini sharma answered |
Explanation:
The given reaction is: Cu + 2AgNO3 → Cu(NO3)2 + 2Ag
This reaction involves the displacement of silver from its compound (AgNO3) by copper. This type of reaction is known as a single displacement reaction or a substitution reaction.
To determine which metal is more reactive, we need to look at the activity series of metals. This series arranges metals in order of their reactivity, with the most reactive metals at the top and the least reactive at the bottom.
Copper is placed below silver in the activity series, which means that silver is more reactive than copper. Therefore, when copper is added to silver nitrate solution, it displaces the silver from its compound and forms copper nitrate. The displaced silver ions combine with copper atoms to form solid silver, which is observed as a brownish precipitate.
Hence, the correct option is A - Copper is more reactive than silver.
The given reaction is: Cu + 2AgNO3 → Cu(NO3)2 + 2Ag
This reaction involves the displacement of silver from its compound (AgNO3) by copper. This type of reaction is known as a single displacement reaction or a substitution reaction.
To determine which metal is more reactive, we need to look at the activity series of metals. This series arranges metals in order of their reactivity, with the most reactive metals at the top and the least reactive at the bottom.
Copper is placed below silver in the activity series, which means that silver is more reactive than copper. Therefore, when copper is added to silver nitrate solution, it displaces the silver from its compound and forms copper nitrate. The displaced silver ions combine with copper atoms to form solid silver, which is observed as a brownish precipitate.
Hence, the correct option is A - Copper is more reactive than silver.
Which form of energy is responsible for the decomposition reactions ?- a)Heat
- b)All of these
- c)Electricity
- d)light
Correct answer is option 'B'. Can you explain this answer?
Which form of energy is responsible for the decomposition reactions ?
a)
Heat
b)
All of these
c)
Electricity
d)
light
|
Sahana Menon answered |
Decomposition reactions and energy:
There are various forms of energy that can drive decomposition reactions, breaking down compounds into simpler substances.
All of these:
- Heat: Many decomposition reactions are initiated by heating the compound, which provides the necessary energy to break bonds and start the decomposition process. This is a common method used in industries and laboratories.
- Electricity: In some cases, passing an electric current through a compound can trigger decomposition reactions. This is known as electrolysis and is commonly used in processes like electroplating and water electrolysis.
- Light: Certain compounds can undergo decomposition reactions when exposed to light, especially ultraviolet light. This phenomenon is known as photolysis and is utilized in various chemical reactions.
Therefore, all of these forms of energy - heat, electricity, and light - can be responsible for driving decomposition reactions. Each form of energy provides the necessary activation energy to break the existing bonds in a compound, leading to its decomposition into simpler substances.
There are various forms of energy that can drive decomposition reactions, breaking down compounds into simpler substances.
All of these:
- Heat: Many decomposition reactions are initiated by heating the compound, which provides the necessary energy to break bonds and start the decomposition process. This is a common method used in industries and laboratories.
- Electricity: In some cases, passing an electric current through a compound can trigger decomposition reactions. This is known as electrolysis and is commonly used in processes like electroplating and water electrolysis.
- Light: Certain compounds can undergo decomposition reactions when exposed to light, especially ultraviolet light. This phenomenon is known as photolysis and is utilized in various chemical reactions.
Therefore, all of these forms of energy - heat, electricity, and light - can be responsible for driving decomposition reactions. Each form of energy provides the necessary activation energy to break the existing bonds in a compound, leading to its decomposition into simpler substances.
Assertion (A): The iron nail becomes brownish in color and the blue color of copper sulfate solution fades.Reason (R): In the reaction Fe(s) + CuSO4(aq) → FeSO4(aq) + Cu(s), iron displaces copper in the copper sulfate solution.- a)If both Assertion and Reason are true and Reason is the correct explanation of Assertion
- b)If both Assertion and Reason are true but Reason is not the correct explanation of Assertion
- c)If Assertion is true but Reason is false
- d)If both Assertion and Reason are false
Correct answer is option 'A'. Can you explain this answer?
Assertion (A): The iron nail becomes brownish in color and the blue color of copper sulfate solution fades.
Reason (R): In the reaction Fe(s) + CuSO4(aq) → FeSO4(aq) + Cu(s), iron displaces copper in the copper sulfate solution.
a)
If both Assertion and Reason are true and Reason is the correct explanation of Assertion
b)
If both Assertion and Reason are true but Reason is not the correct explanation of Assertion
c)
If Assertion is true but Reason is false
d)
If both Assertion and Reason are false
|
Lakesway Classes answered |
- The Assertion is true as the iron nail indeed becomes brownish and the blue color of the copper sulfate solution fades due to the displacement reaction described.
- The Reason is also true as iron displaces copper from the copper sulfate solution.
- The Reason is the correct explanation of the Assertion because the observed color changes are a direct result of the displacement reaction where iron replaces copper in the solution.
Why does an iron nail become brownish in color and the blue color of copper sulfate solution fades?- a)Due to a chemical reaction with air
- b)Because of a change in temperature
- c)As a result of a displacement reaction
- d)Through a physical reaction with water
Correct answer is option 'C'. Can you explain this answer?
Why does an iron nail become brownish in color and the blue color of copper sulfate solution fades?
a)
Due to a chemical reaction with air
b)
Because of a change in temperature
c)
As a result of a displacement reaction
d)
Through a physical reaction with water
|
Divey Sethi answered |
- When an iron nail is immersed in a copper sulfate solution, a displacement reaction occurs.
- In this reaction, iron displaces copper from copper sulfate solution, leading to the formation of iron sulfate and metallic copper.
- This explains why the iron nail turns brownish and the blue color of the copper sulfate solution fades, showcasing a classic example of a displacement reaction.
Identify the reaction: AgNO3(aq) + KCl(aq) → AgCl↓ + KNO3(aq)- a)Combination reaction
- b)Decomposition reaction
- c)Precipitation reaction
- d)None of these
Correct answer is option 'C'. Can you explain this answer?
Identify the reaction:
AgNO3(aq) + KCl(aq) → AgCl↓ + KNO3(aq)
a)
Combination reaction
b)
Decomposition reaction
c)
Precipitation reaction
d)
None of these
|
|
Tushar Kumar answered |
Understanding the Reaction
The reaction in question is:
AgNO3(aq) + KCl(aq) → AgCl↓ + KNO3(aq)
This equation represents the interaction of silver nitrate and potassium chloride in aqueous solution.
What is a Precipitation Reaction?
- A precipitation reaction occurs when two soluble salts react in solution to form an insoluble product, known as a precipitate.
- In this case, AgCl is the precipitate, which is insoluble in water, and it forms as a solid that can be seen separating from the solution.
Identifying the Components
- Reactants:
- AgNO3 (silver nitrate) and KCl (potassium chloride) are both soluble in water and dissociate into their respective ions.
- Products:
- AgCl (silver chloride) is the insoluble precipitate that forms and KNO3 (potassium nitrate) remains soluble.
Why is it a Precipitation Reaction?
- The formation of AgCl (a solid) from the reaction indicates that a new substance is created that cannot stay dissolved in the solution.
- The downward arrow (↓) next to AgCl signifies that it is a precipitate.
Conclusion
In summary, the reaction between AgNO3 and KCl is classified as a precipitation reaction (option C) because it results in the formation of an insoluble solid (AgCl) from the interaction of two aqueous solutions. This is a key concept in understanding chemical reactions and their classifications in chemistry.
The reaction in question is:
AgNO3(aq) + KCl(aq) → AgCl↓ + KNO3(aq)
This equation represents the interaction of silver nitrate and potassium chloride in aqueous solution.
What is a Precipitation Reaction?
- A precipitation reaction occurs when two soluble salts react in solution to form an insoluble product, known as a precipitate.
- In this case, AgCl is the precipitate, which is insoluble in water, and it forms as a solid that can be seen separating from the solution.
Identifying the Components
- Reactants:
- AgNO3 (silver nitrate) and KCl (potassium chloride) are both soluble in water and dissociate into their respective ions.
- Products:
- AgCl (silver chloride) is the insoluble precipitate that forms and KNO3 (potassium nitrate) remains soluble.
Why is it a Precipitation Reaction?
- The formation of AgCl (a solid) from the reaction indicates that a new substance is created that cannot stay dissolved in the solution.
- The downward arrow (↓) next to AgCl signifies that it is a precipitate.
Conclusion
In summary, the reaction between AgNO3 and KCl is classified as a precipitation reaction (option C) because it results in the formation of an insoluble solid (AgCl) from the interaction of two aqueous solutions. This is a key concept in understanding chemical reactions and their classifications in chemistry.
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