Question

Use the activity series of metals to write a balanced chemical equation for each single-replacement reaction.
a) Au(s) + KNO3(aq)----->
b) Zn(s) + AgNO3(aq)----->
c) Al(s) + H2SO4(aq)----->

Answer 1

you're using the activity series to predict whether or not, the metal in the compound will oxidize the other metal present.

For example, Au(s) + KNO3(aq)

will \(K^+\) oxidize \(Au\)?

In order to do that, Au needs to be more reactive than K, and will be placed higher in the series. If Au is below K, this will not proceed.

Answer 2

okay, Au isn't on my chart, but K is and i don't think Au is more reactive cause K is pretty high...

Answer 3

you're right, i think Au is the lowest (although it might be Pt, regardless), it will not be oxidized by \(K^+\). Just follow the same logic for the next two.

Answer 4

okay i figured out which ones are more reactive, but i still don't know what i am supposed to put after the arrow..

Answer 5

"..single-replacement reaction"

Answer 6

the metals will "switch" places, as one it oxidized and the other is reduced.

Answer 7

Thank you so much for helping! These are the answers i got, but idk if they are right...will you check/correct them?
a) K(s) + AuNO3(aq)
b) Ag(s) + ZnNO3(aq)
c) H2(g) + AlSO4(aq)

Answer 8

hm the second and third are right, the first in wrong (Au will not be oxidized by \(K^+\), remember?).

Answer 9

oh okay. then it would stay the same? Au(s) + KNO3(aq) ?

Answer 10

yes

Answer 11

thank you so much for helping me with this! I just learned it today so still confused but this helped me understand better :)

Answer 12

no problem ! i'm glad it was helpful