8. Using the activity serios, prodict whethe the following two reactions would occur. Na+KBrarrow K+NaBr Ca+AgClarrow Ag+CaCl

To determine whether the given reactions would occur, we need to consider the activity series of metals. The activity series is a list of metals arranged in order of their reactivity from highest to lowest. Metals higher in the activity series can displace metals lower in the series from their compounds.<br /><br />Let's analyze each reaction:<br /><br />1. $Na+KBr\rightarrow K+NaBr$<br /><br />In this reaction, sodium (Na) is trying to displace potassium (K) from potassium bromide (KBr). To determine if this reaction would occur, we need to compare the positions of sodium and potassium in the activity series.<br /><br />The activity series is as follows (from highest to lowest reactivity):<br />$Li > K > Na > Ca > Mg > Al > Zn > Fe > Pb > H > Cu > Hg > Ag > Pt > Au$<br /><br />From the activity series, we can see that sodium (Na) is higher in reactivity than potassium (K). Therefore, sodium can displace potassium from its compound. This means that the reaction $Na+KBr\rightarrow K+NaBr$ would occur.<br /><br />2. $Ca+AgCl\rightarrow Ag+CaCl$<br /><br />In this reaction, calcium (Ca) is trying to displace silver (Ag) from silver chloride (AgCl). Again, we need to compare the positions of calcium and silver in the activity series.<br /><br />From the activity series, we can see that calcium (Ca) is higher in reactivity than silver (Ag). Therefore, calcium can displace silver from its compound. This means that the reaction $Ca+AgCl\rightarrow Ag+CaCl$ would occur.<br /><br />In summary, both reactions $Na+KBr\rightarrow K+NaBr$ and $Ca+AgCl\rightarrow Ag+CaCl$ would occur based on the activity series of metals.