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 with 0.1059 g of copper metal (63.546 g/mol), what 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

a) balanced chemical equation

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

b)

moles of copper = 0.1059 / 63.546 = 1.67 x 10^-3

1 mole of Cu ---------------------> 4 moles HNO3

1.67 x 10^-3 mole Cu --------------> 1.67 x 10^-3 x 4 moles HNO3

-----------------> 6.67 x 10^-3 mole HNO3

moles of HNO3 =  6.67 x 10^-3

molarity = 9.0 M

molarity = moles / volume

9.0 = 6.67 x 10^-3 / volume

volume = 7.41 x 10^-4 L

volume = 0.741 mL

c)

(i) brown colored NO2 gas liberation stops when reaction stops

(ii) no metal can find in the solution when reaction gone completion

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