CHM130 Lesson 8 AYL
Quiz yourself by thinking what should be in
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| When iron is produced from hematite, the following reaction occurs. How many grams of Fe are obtained from 50.0 g of hematite in this process? Fe2O3 + 3CO ® 2Fe + 3CO2 | You have to calculate the percentage of iron in the iron oxide:
(mmFe) 55.84 /(mmFe2O3) 159.68 *2 (because you produce 2 mols of Iron) *100 = 69.94%
50g*69.94/100 = 34.94g obtained of Iron
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| If 132.0 g CuO is reacted with 5.000 g H2, what mass of Cu would be prepared by the following reaction? CuO + H2 ® Cu + H2O | moles CuO = 132.0 g / 79.5454 g/mol = 1.66
moles H2 = 5.000 g/ 2.106 g/mol = 2.48 ( in excess)
moles Cu = 1.66
mass Cu = 1.66 mol x 63.546 g/mol =105.5 g
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| Sugar cane produces sucrose (C12H22O11) from water and carbon dioxide through photosynthesis: 12CO2 + 11H2O ® C12H22O11 + 12O2 If the reaction consumes 30.0 g of carbon dioxide and produces 6.84 g of sucrose, what is the percent yield? | Molar mass CO2 = 12.011+15.99*2 = 44.009g/mol
Molar mass C12H22O11 = 12.001*12+1.008*22+15.999*11= 342.297g/mol
30g CO2 = 30/44.009 = 0.682mol
0.682mol CO2 will produce : 0.682/12 = 0.0568mol sucrose
0.0568mol sucrose = 0.0568*342.297 = 19.445g su
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| Balance the following chemical equations: CaCl2 + Na2SO4 ® CaSO4 + NaCl | CaCl2 + Na2SO4 = CaSO4 + 2 NaCl
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| Al + O2 ® Al2O3 | 4 Al + 3 O2 = 2 Al2O3
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| KI + Cl2 ® KCl + I2 | 2 KI + Cl2 = 2 KCl + I2
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| The heads of matches are made with P4S3. This material is made by heating a mixture of red phosphorus and sulfur: 8P4 + 3S8 ® 8P4S3 If a match company uses 5435 grams of phosphorus (P4) with an excess of sulfur, how many grams of P4S3 can be made? | P4 MW = 123.88 g/mol
S8 MW = 256.48 g/mol
P4S3 MW = 220.06 g/mol
(5435 g P4 / 123.88 g/mol) = 43.87 moles P4
43.87 moles P4 x 220.06 g/mol P4S3 = 9654.03 g P4S3
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| Flashlights use magnesium because of the bright light that is formed when it burns. How many grams of magnesium oxide will be produced if 0.432 g Mg is reacted with 0.130 g O2? 2Mg + O2 ® 2MgO | 0.00876 mol MgO x (40.31 g MgO / 1 mol MgO) = 0.353 g Mg [Cancel moles of Mg]
The reaction yields approximately 353 milligrams of magnesium oxide.
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To hide a column, click on the column name.
To hide the entire table, click on the "Hide All" button.
You may also shuffle the rows of the table by clicking on the "Shuffle" button.
Or sort by any of the columns using the down arrow next to any column heading.
If you know all the data on any row, you can temporarily remove it by tapping the trash can to the right of the row.
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