How many grams of copper are required to replace .5 moles of silver nitrate (which is dissolved in water), assuming a copper (II) product?

1 Answer
Mar 4, 2016

Answer:

You need 16 g of copper.

Explanation:

The equation for the reaction is

#"2Ag"^+("aq") + "Cu(s)" → "2Ag(s)" + "Cu"^(2+)("aq")#

Step 1. Calculate the moles of #"Cu"# required.

#0.5 color(red)(cancel(color(black)("mol Ag"^+))) × "1 mol Cu"/(2 color(red)(cancel(color(black)("mol Ag"^+)))) = "0.25 mol Cu"#

Step 2. Calculate the mass of #"Cu"#.

#0.25 color(red)(cancel(color(black)("mol Cu"))) × "63.55 g Cu"/(1 color(red)(cancel(color(black)("mol Cu")))) = "16 g Cu"#