Final answer:
The activity series ranks metals by their reactivity, helping predict single-replacement reactions. A more reactive metal can displace a less reactive one from its compound. Option A is correct.
Step-by-step explanation:
Understanding the Activity Series in Chemistry
The activity series is a list of metals arranged according to their reactivity from highest to lowest. It can be used to predict if a certain single-replacement reaction will occur. This prediction is based on the placement of the metals in the series. If a metal is above another in the series, it can displace the lower metal from its compounds.
To determine which of the reactions (F, G, H, I) is most likely to occur, we can look at the components involved against the activity series. Reaction F would require the metal in QTERV (assuming it represents a real metal) to be able to displace another metal from its compound.
We'd use the activity series to check if QTERV is higher than that other metal. Since we do not have the actual elements represented by these fictional codes, we cannot accurately predict which reaction is more likely to occur without the proper elemental symbols. Nonetheless, in real cases, we'd look for a reaction where a metal higher in the activity series attempts to displace a metal that is lower in the series.
In terms of actual chemical examples:
FeCl2 + Zn - Based on the activity series, zinc can displace iron from its compound because zinc is more reactive. Therefore, this reaction would occur.
HNO3 + Au - Gold is less reactive than hydrogen and will not react with nitric acid to produce hydrogen gas. No reaction (NR) will occur in this case.
Without the actual elements for reactions F, G, H, and I, we cannot determine which is most likely, but the concept applies universally across real chemical reactions.