1)One Copper penny contains 3 g of Copper.
100 Copper Pennies contains 300 g of Copper
No of moles of Copper=300/63.546=4.721
No of moles of chalcopyrite=4.721
Mass of chalcopyrite to be mined is 4.721×183.53=866.443g(Answer)
2)2CuFeS₂+3O₂→2CuS+2FeO+2SO₂
x moles 9x/10 moles
All other reactions have 100% yield.
So no of moles of copper produced is 9x/10 moles.
One Copper penny contains 3 g of Copper.
100 Copper Pennies contains 300 g of Copper.
No of moles of Copper=300/63.546=4.721
9x/10=4.721
x=4.721×10/9
x=5.24moles of Chalcopyrite.
Mass of chalcopyrite to be mined is 5.24×183.53=962.72g(Answer)
3)2CuFeS₂+3O₂→2CuS+2FeO+2SO₂
x moles 9x/10 moles
2CuS→Cu₂S+S
9x/10 81x/200
Cu₂S+S+2O₂→2Cu+2SO
81x/200 729x/1000
One Copper penny contains 3 g of Copper.
100 Copper Pennies contains 300 g of Copper
No of moles of Copper=300/63.546=4.721
729x/1000=4.721
x=4.721×1000/729
x=6.48moles of Chalcopyrite.
Mass of chalcopyrite to be mined is 6.48×183.53=1188.54g(Answer)
Comments
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I have the same exact question except with an 83 percent yield. I got parts 1 and 2 right following along for your answer, but for part 3 where did the 81x/200 come from? I'm asking so I know what to substitute for mine.
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