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

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1 Answer
May 25, 2016

Answer:

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.

http://www.bbc.co.uk/education/guides/zqjsgk7/revision

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.

http://fphoto.photoshelter.com/image/I00004fXTXt7qohM