Ms. Parmar Chem 11 Extra Practice

Chemistry 11: Extra Practice Worksheet Stoichiometry Mass-mass problems Be sure to have the correct significant figures. 1. 4 FeCr2O 7 + 8 K 2CO 3 + O 2 ---> 2 Fe2O 3 + 8 K 2CrO 4 + 8 CO 2 (a) How many grams of FeCr 2O 7 are required to produce 44.0 g of CO 2? (b) How many grams of O 2 are required to produce 100.0 g of Fe 2O 3? (c) If 300.0 g of FeCr 2O 7 react, how many g of O 2 will be consumed? (d) How many g of Fe2O 3 will be produced from 300.0 g of FeCr 2O 7? (e) How many grams of K 2CrO 4 are formed per gram of K 2CO 3 used? 2. Given the reaction S + O 2 ---> SO 2 (a) How many grams of sulfur must be burned to give 100.0 g of SO 2 (b) how many grams of oxygen will be required for the reaction in part? 3. 6 NaOH + 2 Al ---> 2 Na3AlO3 + 3 H 2 (a) How much aluminum in required to produce 17.5 g of hydrogen? (b) How much Na3AlO3 can be formed from 165.0 g of sodium hydroxide? (c) How many moles of NaOH are required to produce 3 g of hydrogen?

Ms. Parmar Chem 11 Extra Practice

(d) How many mol of hydrogen can be prepared from 1 gram atom of aluminum? 4. BaO + H 2SO 4 ---> BaSO 4 + H 2O (a) How much BaSO 4 can be formed from 196.0 g of H 2SO 4? (b) If 81.00 g of water is formed during this reaction, how much BaO was used? 5. NaCl + AgNO 3 ---> AgCl + NaNO 3 (a) 78.00 g of NaCl should produce how many grams of AgCl? (b) How much AgCl can be produced from 107.0 g of AgNO 3? 6. B2O 3 + 3 Mg ---> 3 MgO + 2B (a) How much boron can be obtained from 10.00 tons of B 2O 3? (b) how much magnesium is required to produce 400.0 mg of boron? 7. SnO 2 is reduced by carbon according to the this reaction: SnO 2 + C ---> Sn + CO 2 (a) How many pounds of CO2 are formed when 1.00 kg of tin is produced? (b) How much SnO 2 is required to produce 6.00 Mg of tin? (c) How much tin is produced per ton of carbon used? 8. 2 KMnO 4 + H 2SO 4 ---> K 2SO 4 + Mn2O 7 + H 2O (a) How many moles of Mn 2O 7 can be formed from 196.0 g of KMnO 4? (b) How many grams of Mn 2O 7 can be formed from 390.0 g of KMnO 4?

Ms. Parmar Chem 11 Extra Practice

(c) How much H 2SO 4 is needed to produce 27.00 g of water? 9. Determine moles of barium bromate that can be prepared from 7.000 moles each of HBrO 3 and Ba(OH) 2 given this equation: HBrO 3 + Ba(OH)2 ---> Ba(BrO 3) 2 + H 2O 10. Determine moles of Na 2S that can be prepared by the reaction of 0.2240 moles of sodium with 0.1320 moles of sulfur. Which reactant is the limiting factor? 16 Na + S 8 ---> 8 Na2S Mole- Volume STP and Limiting Reagent 1. Sodium reacts with water to form sodium hydroxide and hydrogen gas according to the equation: 2 Na (s) + 2 H 20 (l) ---> 2 NaOH (aq) + H 2 (g) a. If 90.0 grams of sodium is dropped into 80.0 g of water, how many liters of hydrogen at STP would be produced? b. Which reactant is in excess and how much of it is left over? 2. Phosphorus burns in oxygen gas to produce phosphorus (V) oxide (P 4O 10) according to the equation: P 4 (s) + 5O 2 (g) ---> P 4O 10 (g) a. If 2.50 grams of phosphorus is ignited in a flask containing 750 mL of oxygen at STP, how many grams of P 4O 10 are formed? b. Which reactant is in excess and how much of it is left over?

Ms. Parmar Chem 11 Extra Practice

Magnesium burns in oxygen to produce magnesium oxide.

a. If 1.00 of magnesium is ignited in a flask containing 0.500 liter of oxygen at STP, how many grams of magnesium oxide are produced?

b. What is the name and amount of the reactant in excess? Miscellaneous questions 1. For the reaction: 6 Li(s) + N 2(g) → 2 Li3N(s) Determine: a) the mass of N 2 needed to react with 0.536 moles of Li. b) the number of moles of Li required to make 46.4 g of Li 3N. c) the mass in grams of Li 3N produced from 3.65 g Li. d) the number of moles of lithium needed to react with 7.00 grams of N 2. 2. For the reaction: SnO 2( s ) + 2 H 2( g ) → Sn(s ) + 2 H 2O(l ) Determine: a) the mass of tin produced from 0.211 moles of hydrogen gas.

Ms. Parmar Chem 11 Extra Practice

b) the number of moles of H 2O produced from 339 grams of SnO 2. c) the mass of SnO 2 required to produce 39.4 grams of tin. d) the number of atoms of tin produced in the reaction of 3.00 grams of H 2. e) the mass of SnO 2 required to produce 1.20 x 10 21 molecules of water. 3. Given the following equation: 2 KClO 3 ---> 2 KCl + 3 O 2. How many moles of O 2 can be produced by letting 12.00 moles of KClO 3 react? 4. Given the following equation: 2 NaClO 3 ---> 2 NaCl + 3 O 2. a. 12.00 moles of NaClO 3 will produce how many grams of O 2? b. How many grams of NaCl are produced when 80.0 grams of O 2 are produced? 9. The average human requires 120.0 grams of glucose (C 6H 12O 6) per day. How many grams of CO 2 (in the photosynthesis reaction) are required for this amount of glucose? The photosynthetic reaction is: 6 CO 2 + 6 H 2O ---> C6H 12O 6 + 6 O 2