Moles Revisited Name Date Molar Mass How do you calculate the formula mass of a compound? Examples Potassium fluoride Strontium nitrate Aluminum nitride Magnesium phosphate Mole Conversions One-step How many moles are in 3.65 x 10 24 molecules of CaC 2? How many liters are in 0.43 moles of CO 2 at STP? How many moles are in 100 g of Au?
If there are 3.42 moles of RbS, how many particles would be present? How many moles of H 2 are equal 45 L? If a student calculated that a sample of K 2SO 4 contained 1.59 moles, how much would this sample weigh? Two -step If there are 3.87 x 10 25 molecules, how many grams of LiOH would be present? How many liters of H 2 are 5 g? How many particles are in 30 L of SO 2? Molar Ratio NH 3 + O 2 N 2 + H 2O How many moles of each?
Name: Period: Stoichiometry Practice Worksheet Directions Perform the following calculations. SHOW ALL WORK!!! 1. If you start with 56.0 grams of sodium, how many moles of water will react with it? Molar Mass of Na = Molar Mass of H 2 O = Molar Mass of NaOH = Molar Mass of H 2 = Na(s) + H 2 O(l) NaOH(aq) + H 2 (g) 2. If you start with 34.0 grams of silver (I) nitrate, how many grams of solid silver would be produced? Molar Mass of Cu = Molar Mass of AgNO 3 = Molar Mass of Ag = Molar Mass of Cu(NO 3 ) 2 = Cu(s) + AgNO 3 (aq) Ag(s) + Cu(NO 3 ) 2 (aq) 3. If you start with 72.0 grams of water, how many moles of sodium with react with it? Molar Mass of Na = Molar Mass of H 2 O = Molar Mass of NaOH = Molar Mass of H 2 = Na(s) + H 2 O(l) NaOH(aq) + H 2 (g)
4. If you start with 25.4 grams of copper, how many grams of solid silver would be produced? Molar Mass of Cu = Molar Mass of AgNO 3 = Molar Mass of Ag = Molar Mass of Cu(NO 3 ) 2 = Cu(s) + AgNO 3 (aq) Ag(s) + Cu(NO 3 ) 2 (aq) 5. If you start with 14.0 grams of diatomic nitrogen how many grams of diatomic hydrogen will react with it? Molar Mass of N 2 = Molar Mass of H 2 = Molar Mass of NH 3 = N 2 (g) + H 2 (g) NH 3 (g) 6. If you start with 83.9 grams of iron, how many grams of iron (III) oxide will be formed? Molar Mass of Fe = Molar Mass of Fe 2 O 3 = Molar Mass of O = Fe(s) + O 2 (g) Fe 2 O 3 (s)
Mixed Stoichiometry Practice Name Date Period Write and/or balance the following equations (remember the diatomic elements and to crisscross charges for ionic compounds!!!) Use the mole ratios from the balanced equations to solve the following stoichiometry problems. Use units and labels in all conversions, and round your answer to sig figs. 1. Potassium chlorate decomposes into potassium chloride and oxygen gas. 2. How many moles of oxygen are produced when 3.0 moles of potassium chlorate decompose completely? 3. Butane (C 4 H 10 ) undergoes combustion. C 4 H 10 (l) + O 2 (g) CO 2 (g) + H 2 O(l) 4. How many grams of CO 2 are produced when 88 g of O 2 are reacted with an excess of butane? 5. Water decomposes into hydrogen gas and oxygen gas by electrolysis. 6. How many grams of hydrogen will be produced when 6.0 moles of oxygen are produced? 7. How many grams of water are required to produce 9.00 grams of hydrogen?
8. Cobalt(II) chloride reacts with fluorine in a single replacement reaction to produce cobalt(ii) fluoride and chlorine gas. CoCl 2 + F 2 CoF 2 + Cl 2 9. How many grams of fluorine are required to produce 290.8 g of cobalt(ii) fluoride? 10. Balance the following equation. SrCl 2 (aq) + H 2 SO 4 (aq) HCl(aq) + SrSO 4 (s) 11. What is the mass of strontium chloride that reacts with 300.0 g of sulfuric acid? 12. Solid iron(iii) oxide reacts with hydrogen gas to form iron and water. 13. How many grams of iron are produced when 450 grams of iron(iii) oxide are reacted? 14. How many grams of water will be produced when 0.0155 moles of hydrogen gas react completely with iron(iii) oxide?