Question

Using the balanced chemical reaction below, how many grams of copper (cu) metal can be obtained from 1.00 kg of copper ore (cu3fes3)? 2cu3fes3 (s) + 7o2 (g) ; → 6cu (s) + 2feo (s) + 6so2 (g)

Answer 1

Answer : Mass of copper (Cu) metal obtained = 556.281 g

Solution : Given,

Mass of copper ore = 1 Kg = 1000 g

From the periodic table, the molar mass of copper and copper ore are

Molar mass of copper = 63.546 g/mole

Molar mass of copper ore, $Cu_{3}FeS_{3}$ = 342.678 g/mole

First we have to calculate the number of moles of copper ore, $Cu_{3}FeS_{3}$

Moles of  $Cu_{3}FeS_{3}$ = $\frac{\text{ Mass of copper ore}}{\text{ Molar mass of copper ore}}$ = $\frac{1000g}{342.678g/mole}$ = 2.918 moles

The balanced chemical reaction is :

$2Cu_{3} FeS_{3}(s)+7O_{2}(g)\rightarrow 6Cu(s)+2FeO(s)+6SO_{2}(g)$

From this chemical reaction, we conclude that

2 moles of $Cu_{3}FeS_{3}$ gives          →     6 moles of Cu

2.918 moles of $Cu_{3}FeS_{3}$ gives   →      $\frac{6moles}{2moles}\times 2.918moles$

                                                           = 8.754 moles

Thus, the Moles of copper (Cu) = 8.754 moles

Now, calculate the Mass of copper (Cu).

Mass of copper (Cu) = Moles of copper (Cu) × Molar mass of copper (Cu)

                                  = 8.757 moles × 63.546 g/moles

                                  = 556.281 g                                

Answer 2

The mass of copper that can be obtained from 1.00 kg of copper ore is 556 g.

Further Explanation

This problem can be solved using basic stoichiometry.

To start, the balanced chemical equation is:

2 Cu₃FeS₃(s) + 7 O₂(g) → 6 Cu(s) + 2 FeO(s) + 6 SO₂(g)

From the equation, the stoichiometric ratio of  the copper ore and the copper metal is known to be 2:6.

To use dimensional analysis, the following conversion factors are needed:

• 1 kg = 1000 g
• 2 mol Cu₃FeS₃ consumed = 6 mol Cu formed

• 1 mol Cu₃FeS₃ = 342.678 g
• 1 mol Cu = 63.546 g

Setting up the dimensional analysis, first convert the mass in kilograms to grams (since molar masses are in grams). Then, convert the mass of the copper ore to moles. Finally, use the stoichiometric ratio to determine how many moles of Cu will form.$moles \ of \ Cu = 1.00 \ kg \ Cu_3FeS_3 \times \frac{1000 \ g}{1 \ kg} \times \frac{1 \ mol \ Cu_3FeS_3}{342.678 \ g} \times \frac{6 \ mol \ Cu}{2 \ mol \ Cu_3FeS_3}\\\\\boxed {moles \ of \ Cu = 8.755 \ mol}$

To get the mass of copper metal, simply multiply the number of moles of copper formed by its molar mass as shown below:

$mass \ of \ Cu \ = 8.755 \ mol Cu \times \frac{63.546 \ g}{1 \ mol}\\\\\boxed {mass \ of \ Cu \ = 556.35 \ g}$

Since the given has three significant figures only, the final answer must have three significant figures as well. Therefore, the final answer is:

$\boxed {\boxed {mass \ of \ Cu \ = 556 \ g}}$

Learn More

• Learn more about Ore Extraction https://brainly.com/question/4529876
• Learn more about Mole Conversion brainly.com/question/6125309

Keywords: Stoichiometry, copper, ore extraction