Question

Predict the products of the following reactions. If no reaction occurs, write “NR” for No Reaction. Do not worry about balancing the equation?

Answer 1

Here's what I got.

Explanation:

You can predict if single replacement reactions will take place by using the metal reactivity series.

In general, a metal that is higher in the reactivity series will displace a metal that is lower in the reactivity series.

In your case, aluminium, `"Al"`, is actually higher in the reactivity series than silver, `"Ag"`, which means that silver cannot displace aluminium from aliminium chloride, `"AlCl"_3`.

Therefore, you will have

`"AlCl"_ (3(aq)) + "Ag"_ ((s)) -> "N.R."`

The second reaction will take place because hydrobromic acid, `"HBr"`, a strong acid, will react with sodium hydroxide, `"NaOH"`, a strong base, to produce aqueous sodium bromide and water.

`"HBr"_ ((aq)) + "NaOH"_ ((aq)) -> "NaBr"_ ((aq)) + "H"_ 2"O"_ ((l))`

In this case, you're dealing with a neutralization reaction that basically looks like this

`overbrace("H"_ 3"O"_ ((aq))^(+))^(color(blue)("coming from HBr")) + overbrace("OH"_ ((aq))^(-))^(color(green)("coming from NaOH")) = 2"H"_ 2"O"_((l))`

The third reaction will take place because it results in the formation of silver chloride, `"AgCl"`, an insoluble solid that precipitates out of solution.

`"AgNO"_ (3(aq)) + "HCl"_ ((aq)) -> "AgCl"_ ((s)) darr + "HNO"_ (3(aq))`

This is a double replacement reaction for which the net ionic equation looks like this

`"Ag"_ ((aq))^(+) + "Cl"_ ((aq))^(-) -> "AgCl"_ ((s)) darr`

Silver chloride is a white insoluble solid that precipitates out of solution.