specific solving strategy for stoichiometery problem, chemistry homework help

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Name Date Period 16. For the reaction represented by the equation 3Fe + 4H20 Fe3O4 + 4H2, how many moles of iron (III) oxide are produced from 500 g of iron in an excess of H2O? cannot be used for the reaction represented by the equation 3 g Mg(OH), 17. Explain why the conversion factor 6gH, Mg3N2() + 6H2O1) ► 2Mg(OH)2(aq) + 2NH3(Q). Completion Complete each statement. 18. The expression below converts the quantity, mass HCI, to the quantity, 1 mol HC1 1 mol C1, mass HC1 x molar mass HC1 2 mol HC1 х 19. The unit of the following expression is mol H,O 100 g H,Ox 18.02 g H, 20. The expression below converts the quantity, mass HCL, to the quantity, 1 mol HC1 1 mol Cl, molar mass Cly mass HC1 x molar mass HC1 2 mol HCI 1 mol C1 х Answer the following questions. Make sure to show ALL work on your on paper (missing = NO CREDIT) and don't forget your units. Due Monday, May 2nd. If it is not turned in on Monday, May 2nd you will receive NO CREDIT. 1. Why must a chemical equation be balanced to solve stoichiometry problems? 2. List the four types of reaction stoichiometry problems and briefly describe how to solve each one. 3. Describe the steps necessary to solve a mass-mass stoichiometry problem. 4. Correctly balance the formula: NH4NO2 → _N₂ + H2O. - 5. When the formula equation Fe is number is what? Fe3O4 + _Al → Al2O3 + Fe is correctly balanced the coefficient of 6. Given the equation 3A + 2B → 2C, the starting mass of A, and its molar mass, and you are asked to determine the moles of C produced, after you have written your given what is the next step? Write what you would put next when setting up the problem. 7. In the reaction represented by the equation 2Al2O3 → 4A1 + 302, what is the mole ratio of aluminum to oxygen? 8. In the reaction represented by the equation N2 + 3H2 → 2NH3, what is the mole ratio of hydrogen to ammonia? 9. In the equation 2KC103 → 2KCl + 302, how many moles of oxygen are produced when 3.0 mol of KClO3 decompose completely? 10. For the reaction represented by the equation N2 + 3H2 → 2NH3, how many moles of nitrogen are required to produce 18 mol of ammonia? 11. For the reaction represented by the equation 2Na + 2H2O → 2NaOH + H2, how many grams of sodium hydroxide are produced from 3.0 mol of sodium with an excess of water? 12. For the reaction represented by the equation 2Fe + O2 → 2FeO, how many grams of iron(II) oxide are produced from 8.00 mol of iron in an excess of oxygen? 13. For the reaction represented by the equation 2HNO3 + Mg(OH)2 + Mg(NO3)2 + 2H20, how many grams of magnesium nitrate are produced from 8.00 mol of nitric acid, HNO3, and an excess of Mg(OH)2? 14. For the reaction represented by the equation CH4 + 202 → CO2 + 2H20, how many moles of carbon dioxide are produced from the combustion of 100 g of methane? 15. For the reaction represented by the equation Pb(NO3)2 + 2KI → PbI2 + 2KNO3, how many moles of lead(II) iodide are produced from 300. g of potassium iodide and an excess of Pb(NO3)2?
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Final answers are

1. Why must a chemical equation be balanced to solve stoichiometry problems?
A stoichiometry problem requires that you convert from a known quantity of one
compound to an unknown amount of another. The only way to convert between two
compounds is through a molar ratio. The molar ratio is determined by the balanced
chemical equation.
2. List the four types of reaction stoichiometry problems and briefly describe how to
solve each one.
Mole-mole problems - use the molar ratio to change from moles of known to moles
unknown
Mass-mass problems - change to moles of known, the moles of unknown to mass of
unknown, then use the molar volume to solve for the volume
Volume-volume problems - change volume to moles of known, then to moles of unknown
and then to the volume of unknown
Mass-volume problems - change to moles of known, to moles of unknown
For more information see:
http://www.csun.edu/~psk17793/G%20Chemistry/solving_stoichiometry_problems.htm
3. Describe the steps necessary to solve a mass - mass stoichiometry...


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