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To determine which reaction will form products more stable than the reactants, we need to consider the reactivities of the elements involved, focusing primarily on trends in activity series tables or reactivity series.
The reactivity series (or activity series) ranks elements in order of their tendency to form positive ions. For metals, a higher position in the series indicates a greater tendency to lose electrons (higher reactivity), while for nonmetals, a lower position indicates a greater tendency to gain electrons (higher reactivity).
Here's a typical reactivity series for some metals:
- Lithium (Li), Potassium (K), Barium (Ba), Calcium (Ca), Sodium (Na), Magnesium (Mg), Aluminum (Al), Zinc (Zn), Iron (Fe), Lead (Pb), Copper (Cu), Silver (Ag), Gold (Au).
Let's analyze each reaction:
A. [tex]\(2 \text{AlBr}_3 + 3 \text{Zn} \rightarrow 3 \text{ZnBr}_2 + 2 \text{Al}\)[/tex]
- Aluminum (Al) is above Zinc (Zn) in the activity series, indicating that Al is more reactive than Zn. This reaction suggests that a less reactive metal (Zn) is trying to replace a more reactive metal (Al), which is not favorable.
B. [tex]\(\text{CaBr}_2 + 2 \text{Na} \rightarrow 2 \text{NaBr} + \text{Ca}\)[/tex]
- Sodium (Na) is higher than Calcium (Ca) in the activity series, indicating that Na is more reactive than Ca. The reaction suggests that a more reactive metal (Na) is replacing a less reactive metal (Ca), making this reaction favorable.
C. [tex]\(\text{MgBr}_2 + H_2 \rightarrow 2 \text{HBr} + \text{Mg}\)[/tex]
- Magnesium (Mg) is much higher in the reactivity series compared to hydrogen (H). More reactive magnesium replacing less reactive hydrogen does not typically happen in this type of reaction.
D. [tex]\(\text{BaBr}_2 + \text{Ca} \rightarrow \text{CaBr}_2 + \text{Ba}\)[/tex]
- Barium (Ba) is higher than Calcium (Ca) in the reactivity series. This reaction would suggest a less reactive metal (Ca) is trying to replace a more reactive metal (Ba), which is not favorable.
E. [tex]\(2 \text{LiBr} + \text{Ba} \rightarrow \text{BaBr}_2 + 2 \text{Li}\)[/tex]
- Lithium (Li) is above Barium (Ba) in the reactivity series, indicating that Li is more reactive than Ba. This reaction would suggest that a less reactive metal (Ba) is trying to replace a more reactive metal (Li), which is not favorable.
Correct answer:
B. [tex]\(\text{CaBr}_2 + 2 \text{Na} \rightarrow 2 \text{NaBr} + \text{Ca}\)[/tex]
In conclusion, the only reaction where the products are more stable (more favorable) than the reactants based on the activity series is B. This is because sodium (Na) is more reactive than calcium (Ca), leading to a reaction where sodium displaces calcium, resulting in more stable products.
The reactivity series (or activity series) ranks elements in order of their tendency to form positive ions. For metals, a higher position in the series indicates a greater tendency to lose electrons (higher reactivity), while for nonmetals, a lower position indicates a greater tendency to gain electrons (higher reactivity).
Here's a typical reactivity series for some metals:
- Lithium (Li), Potassium (K), Barium (Ba), Calcium (Ca), Sodium (Na), Magnesium (Mg), Aluminum (Al), Zinc (Zn), Iron (Fe), Lead (Pb), Copper (Cu), Silver (Ag), Gold (Au).
Let's analyze each reaction:
A. [tex]\(2 \text{AlBr}_3 + 3 \text{Zn} \rightarrow 3 \text{ZnBr}_2 + 2 \text{Al}\)[/tex]
- Aluminum (Al) is above Zinc (Zn) in the activity series, indicating that Al is more reactive than Zn. This reaction suggests that a less reactive metal (Zn) is trying to replace a more reactive metal (Al), which is not favorable.
B. [tex]\(\text{CaBr}_2 + 2 \text{Na} \rightarrow 2 \text{NaBr} + \text{Ca}\)[/tex]
- Sodium (Na) is higher than Calcium (Ca) in the activity series, indicating that Na is more reactive than Ca. The reaction suggests that a more reactive metal (Na) is replacing a less reactive metal (Ca), making this reaction favorable.
C. [tex]\(\text{MgBr}_2 + H_2 \rightarrow 2 \text{HBr} + \text{Mg}\)[/tex]
- Magnesium (Mg) is much higher in the reactivity series compared to hydrogen (H). More reactive magnesium replacing less reactive hydrogen does not typically happen in this type of reaction.
D. [tex]\(\text{BaBr}_2 + \text{Ca} \rightarrow \text{CaBr}_2 + \text{Ba}\)[/tex]
- Barium (Ba) is higher than Calcium (Ca) in the reactivity series. This reaction would suggest a less reactive metal (Ca) is trying to replace a more reactive metal (Ba), which is not favorable.
E. [tex]\(2 \text{LiBr} + \text{Ba} \rightarrow \text{BaBr}_2 + 2 \text{Li}\)[/tex]
- Lithium (Li) is above Barium (Ba) in the reactivity series, indicating that Li is more reactive than Ba. This reaction would suggest that a less reactive metal (Ba) is trying to replace a more reactive metal (Li), which is not favorable.
Correct answer:
B. [tex]\(\text{CaBr}_2 + 2 \text{Na} \rightarrow 2 \text{NaBr} + \text{Ca}\)[/tex]
In conclusion, the only reaction where the products are more stable (more favorable) than the reactants based on the activity series is B. This is because sodium (Na) is more reactive than calcium (Ca), leading to a reaction where sodium displaces calcium, resulting in more stable products.
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