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Maksim231197 [3]
3 years ago
9

For the following reaction, 5.05 grams of copper are mixed with excess silver nitrate. The reaction yields 11.0 grams of copper(

II) nitrate. silver nitrate (aq) copper (s) copper(II) nitrate (aq) silver (s) What is the ideal yield of copper(II) nitrate
Chemistry
1 answer:
andreyandreev [35.5K]3 years ago
8 0

Answer:

14.9 g is the ideal yield of Cu(NO₃)₂

Explanation:

Reactants for the reaction: Cu and AgNO₃

Products: Copper nitrate and Ag

The balanced reaction is: Cu(s) + 2AgNO₃(aq) →  2Ag (s) + Cu(NO₃)₂

As the silver nitrate is in excess, the Cu will be the limiting reagent.

We convert the mass to moles → 5.05 g . 1 mol/ 63.55 g = 0.0794 moles

Ratio is 1:1, so 0.0794 moles will produce 0.0794 moles of Cupper(II) nitrate. We convert the moles to mass, and that value will be the theoretical yield.

0.0794 mol . 187.55 g /1 mol =  of Cu(NO₃)₂

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Explanation:

Hello!

In this case, since the net ionic equations are ionic representations of the molecular equation in which the spectator ions (those at both reactants and products sides) are cancelled out, we first write the complete ionic equation for this reaction, considering that the solid silver chloride is not ionized due to its precipitation:

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