# For the following questions, assume that you start with 0.427 g of copper turnings? a) Calculate...

## Question:

For the following questions, assume that you start with 0.427 g of copper turnings?

a) Calculate the initial number of moles of {eq}Cu {/eq}.

b) Calculate the minimum volume of 16.0 M {eq}HNO_{3} {/eq} required to dissolve all of the copper.

c) If, in practice, 5.0 mL of 16.0 M nitric acid were added to effect the dissolution of the copper, what would be the minimum volume of 4.00 M {eq}NaOH {/eq} required to neutralize the remaining acid and convert all of the {eq}Cu^{2+}(aq) {/eq} to {eq}Cu(OH)_{2}(s) {/eq}?

d) Calculate the minimum volume of 1.00 M {eq}H_{2}SO_{4} {/eq} required to dissolve all of the {eq}CuO(s) {/eq}.

e) Calculate the minimum mass of zinc required to reduce all of the {eq}Cu^{2+}(aq) {/eq} to {eq}Cu(s) {/eq}.

## Balanced Chemical Equation:

Chemical equations are balanced to determine the stoichiometric quantities of reactants and products. These equations can be used to calculate the relative amounts of reactants required for the complete reaction and the theoretical percentage yield of the reaction.

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Given Data:

• Mass of copper turnings used is 0.427 g.

Part a

The atomic mass of copper is 63.55 g/mol.

The number of moles of copper can be...