Can aluminum (Al) react with K2SO4 by single replacement to yield products? Using the activity series chart, I know that K is more reactive than Al so does that mean that a reaction will occur or not?
AL can come back to life
In the activity series, a METAL above will replace an ION below it but not the other way around. Since Al is below K, no reaction will occur.
To determine whether a reaction will occur between aluminum (Al) and potassium sulfate (K2SO4) by single replacement, you can use the activity series chart.
The activity series chart lists metals in order of their reactivity. According to the activity series, potassium (K) is more reactive than aluminum (Al). When a more reactive metal displaces a less reactive metal in a compound, a single replacement reaction can occur.
In this case, potassium (K) is more reactive than aluminum (Al). Therefore, a reaction will occur between aluminum and potassium sulfate.
The balanced chemical equation for the reaction can be written as follows:
2Al + 3K2SO4 → Al2(SO4)3 + 6K
In this reaction, aluminum (Al) will replace potassium (K) in the potassium sulfate (K2SO4) compound, resulting in the formation of aluminum sulfate (Al2(SO4)3) and potassium (K) as products.
It is important to note that the activity series is a general guide, and other factors like temperature and concentration can also influence the reaction. However, in this case, based on the activity series chart, a reaction should occur between aluminum and potassium sulfate.