To determine whether the reactions will take place, we need to use the given activity series of metals. The activity series ranks metals by their ability to displace other metals from compounds; a metal can displace another metal that is lower in the series.
### Reaction 1: [tex]\( \text{Ag} + \text{NaNO}_3 \rightarrow \text{AgNO}_3 + \text{Na} \)[/tex]
1. Identify the metals involved: The metals in the reaction are silver (Ag) and sodium (Na).
2. Locate Ag and Na in the activity series:
- Silver (Ag) is towards the bottom of the series.
- Sodium (Na) is much higher in the series, above magnesium (Mg).
3. Compare their activities: Since sodium (Na) is higher in the activity series than silver (Ag), sodium is more active.
4. Apply the activity series rule: A less active metal (Ag) cannot replace a more active metal (Na) from its compound.
Conclusion: The reaction [tex]\( \text{Ag} + \text{NaNO}_3 \rightarrow \text{AgNO}_3 + \text{Na} \)[/tex] will not take place.
### Reaction 2: [tex]\( \text{Mn} + \text{CaO} \rightarrow \text{Ca} + \text{MnO} \)[/tex]
1. Identify the metals involved: The metals in the reaction are manganese (Mn) and calcium (Ca).
2. Locate Mn and Ca in the activity series:
- Manganese (Mn) is somewhere in the middle of the series.
- Calcium (Ca) is higher in the series, above sodium (Na).
3. Compare their activities: Since calcium (Ca) is higher in the activity series than manganese (Mn), calcium is more active.
4. Apply the activity series rule: A less active metal (Mn) cannot replace a more active metal (Ca) from its compound.
Conclusion: The reaction [tex]\( \text{Mn} + \text{CaO} \rightarrow \text{Ca} + \text{MnO} \)[/tex] will not take place.
### Final Answer:
Both reactions will not take place. This results in:
1. [tex]\( \text{Ag} + \text{NaNO}_3 \rightarrow \text{AgNO}_3 + \text{Na} \)[/tex] - False
2. [tex]\( \text{Mn} + \text{CaO} \rightarrow \text{Ca} + \text{MnO} \)[/tex] - False
Thus, neither reaction will occur under the given conditions.
