Reactions of copper Experiment. Copper metal reacts with aqueous nitric acid to

Question

Reactions of copper Experiment. Copper metal reacts with aqueous nitric acid to produce copper (II) nitrate, nitrogen dioxide and water. a. Write a balanced chemical equation describing this reaction. Include the phase designation for each reactant and product (solid, liquid, gas, aqueous). b. Assuming that you start 0.1059 g of copper metal (63.546 g/mol), what with volume, in mL, of 9.0 M nitric acid would be required for all the copper to react? c. What two observations would be important for this reaction to verify that enough nitric acid was added and the reaction has gone to completion?

Explanation / Answer

For the reaction of copper with nitric acid

a. Balanced chemical equation

Cu(s) + 4HNO3(aq) ---> Cu(NO3)2(aq) + 2NO2(g) + 2H2O(l)

b. 1 mole of Cu reacts with 4 moles of HNO3

moles of Cu reacted = 0.1059 g/63.546 g/mol = 0.00167 mols

moles of HNO3 required = 4 x 0.00167 mol = 0.0067 mols

volume of HNO3 needed = 6.67 mmol/9 M = 0.74 ml

c. All of solid copper would dissolve, If the reaction has gone to completion. Secondly, no more evolution of reddish-brown NO2 gas would be seen, once the reaction goes to completion.

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