Question

Copper metal (Cu) can be dissolved in nitric acid. The chemical equation for the reaction which occurs is: Cu + 4HNO3 → Cu(NO3)2 + 2NO2 + 2H2O a) In order to produce 5.0 moles of NO2, ___ mole(s) of Cu must react with _ mole(s) of HNO3 to produce _ mole(s) of Cu(NO3)2 and _ mole(s) of H2O. b) If 938 g of Cu(NO3)2 are formed, then _ g of copper and _ g of HNO3 are consumed. _ g of NO2 and _ g of H2O are also formed. 2) In an actual experiment, 100.0 g each of copper and nitric acid are used and 70.0 g of copper (II) nitrate is obtained. In this experiment, the limiting reactant is _ and the percentage yield of copper (II) nitrate is ___%. Please fill in the blanks, show step-by-step calculations.

          Copper metal (Cu) can be dissolved in nitric acid. The chemical equation for the reaction which occurs is: Cu + 4HNO3 → Cu(NO3)2 + 2NO2 + 2H2O

a) In order to produce 5.0 moles of NO2, _____ mole(s) of Cu must react with _____ mole(s) of HNO3 to produce _____ mole(s) of Cu(NO3)2 and _____ mole(s) of H2O.

b) If 938 g of Cu(NO3)2 are formed, then _____ g of copper and _____ g of HNO3 are consumed. _____ g of NO2 and _____ g of H2O are also formed.

2) In an actual experiment, 100.0 g each of copper and nitric acid are used and 70.0 g of copper (II) nitrate is obtained. In this experiment, the limiting reactant is _____ and the percentage yield of copper (II) nitrate is _____%. Please fill in the blanks, show step-by-step calculations.

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Added by Kelly M.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

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Solved by Expert Susan Hallstrom

10/12/2023

Step 1

0 moles of NO2. From the balanced chemical equation, we can see that 1 mole of Cu produces 2 moles of NO2. Therefore, we need 2.5 moles of Cu to produce 5.0 moles of NO2. To produce 2.5 moles of Cu(NO3)2, we need half as many moles of Cu, so 1.25 moles of Cu. Show more…

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Copper metal (Cu) can be dissolved in nitric acid. The chemical equation for the reaction which occurs is: Cu + 4HNO3 → Cu(NO3)2 + 2NO2 + 2H2O a) In order to produce 5.0 moles of NO2, _____ mole(s) of Cu must react with _____ mole(s) of HNO3 to produce _____ mole(s) of Cu(NO3)2 and _____ mole(s) of H2O. b) If 938 g of Cu(NO3)2 are formed, then _____ g of copper and _____ g of HNO3 are consumed. _____ g of NO2 and _____ g of H2O are also formed. 2) In an actual experiment, 100.0 g each of copper and nitric acid are used and 70.0 g of copper (II) nitrate is obtained. In this experiment, the limiting reactant is _____ and the percentage yield of copper (II) nitrate is _____%. Please fill in the blanks, show step-by-step calculations.

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