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

Answer 1

You need 16 g of copper.

The reaction's equation 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"#

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Answer 2

Ellie Andrews

To determine the amount of copper needed to replace 0.5 moles of silver nitrate, use the stoichiometry of the reaction. The balanced chemical equation is:

2AgNO₃ + Cu → Cu(NO₃)₂ + 2Ag

From the equation, 2 moles of silver nitrate react with 1 mole of copper. Therefore, for 0.5 moles of silver nitrate, you would need 0.25 moles of copper.

To convert moles of copper to grams, use the molar mass of copper:

Cu: 63.55 g/mol

0.25 moles * 63.55 g/mol = 15.8875 grams of copper

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.