3. Carbon disulfide is an important organic solvent. It can be produced from sulfur dioxide, a byproduct of buring coal.
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1 L3 Chemistry: Stoichiometry: Unit 8: Name Page 1 Mol mol problems: (use only step 2 on the back)! (Chapter 9, p )! 4 P + 5 O 2 > 2 P 2 O 5! How many mol of P 2 O 5 are made from 12 mol P? 12 mol P 2 mol P 2 O 5 = 6 mol P 2 O 5! (where the 2 and 4 are coefficients! 4 mol P! from the balanced equation above) 1. Balance the reaction: Ca(NO 3 ) 2 + K 3 PO > KNO 3 + Ca 3 (PO 4 ) 2 a. How many mol of KNO 3 form when 2 mol of Ca 3 (PO 4 ) 2 form?! (12 mol) b. How many mol of K 3 PO 4 are needed to react with 9 mol Ca(NO 3 ) 2?! (6 mol) c. How many mol of Ca 3 (PO 4 ) 2 are formed from 12 mol Ca(NO 3 ) 2?! (4 mol) 2. Write the balanced equation for this word equation:! Iron metal + oxygen gas ----> Iron(III) oxide a. How many mol of iron are needed to form 2.3 mol of Iron (III) oxide?! (4.6 mol) b. How many mol of oxygen gas are required to react with 0.84 mol of Iron?! (0.63 mol) c. How many mol of Iron(III) oxide are formed when 17.4 mol of oxygen gas reacts? (11.6 mol) Volume-Volume (L L) Problems: Same as above, 1 (middle) step. The Coefficients in the equation can also represent Liters of a Gas at STP.! (p. 249) 3. Carbon disulfide is an important organic solvent. It can be produced from sulfur dioxide, a byproduct of buring coal. (Already balanced) 5 C + 2 SO 2 (g) ----> CS 2 (g) + 4 CO (g) a. How many Liters of CO gas form when 6.30 Liters of SO 2 gas reacts?(both gases at STP) (12.6 L) b. How many L of CS 2 gas are made at the same time as 7.24 L CO gas? (Gases are at STP) (1.81 L) c. How many ml of SO 2 gas react to make 182 ml of CS 2 gas? (Gases are at STP) (364 ml)
2 Mass-Mass (or g g) problems : Need three steps! ( p )! Page 2 **The general equation is: (a and b are the coefficients from the balanced equation)**! Step 1! Step 2! Step 3! g Known! 1 mol known! a mol unknown! formula wt of unknown (g)! = g Unknown formula wt! b mol known! 1 mol of unknown! of known (g)! Change known! Mol known to Mol unknown! Change unknown! grams to mol! (Mol ratio from balanced Equ.)! mol to grams 4. Sugars are made by plants during photosynthesis (already balanced): 6 CO H 2 O ----> C 6 H 12 O O 2 example: How many grams of CO 2 will react to form 630 grams of C 6 H 12 O 6?! 630 g C 6 H 12 O 6 1 mol C 6 H 12 O 6 6 mol CO 2 44 g CO 2 = 924 g CO g C 6 H 12 O 6! 1 mol C 6 H 12 O 6! 1 mol CO 2 a. How many grams of C 6 H 12 O 6 can a plant make from 110 grams CO 2?! (75.0 g) b. How many g of O 2 gas does a plant release as it makes 360 g of C 6 H 12 O 6?! (384 g) 5. Write the Balanced formula equation from this word equation: silver nitrate + copper metal > silver metal + copper (II) nitrate a. How many grams of copper are needed to react with 102 g of silver nitrate?! (19.05 g) b. How many g of copper(ii) nitrate are produced at the same time as 54.0 g of silver?! (46.9 g) Grams Mol (a: use steps 1 and 2 only) and Mol Grams (b, use steps 2 and 3 only) 6. Balance the following Double replacement reaction.! (p )! BaCl 2 + Na 3 PO > Ba 3 (PO 4 ) 2 + NaCl! a. How many mol of BaCl 2 react to form 88.0 g NaCl?! (0.750 mol)! b. How many grams of Na 3 PO 4 are needed to react with 1.20 mol BaCl 2?! (131.2 g)
3 L3 Chemistry: Stoichiometry (continued) Name Page 3 Volume (Liters) to/from mol or grams: Use 22.4 L gas at STP to convert to/from Liters (p )! 1 mol 1. Balance this equation for the combustion of Propane gas:! C 3 H 8 (g) + O 2 (g) > H 2 O (l) + CO 2 (g) example for a: How many Liters of CO 2 gas (at STP) will be produced from 66 g C 3 H 8 gas?! 66 g C 3 H 8 1 mol C 3 H 8! 3 mol CO 2! 22.4 L CO 2 = L CO 2 44 g C 3 H 8! 1 mol C 3 H 8! 1 mol CO 2 a. How many Liters of O 2 gas at STP are needed to burn 88.0 grams of C 3 H 8?(3 steps) (224 L) b. How many grams of H 2 O are made along with 121 ml of CO 2 gas at STP?(3 steps,+metric) (0.130 g) c. How many mol of C 3 H 8 will produce 67.2 L of CO 2 gas at STP? (2 steps)! (1.00 mol) % Yield problems : % yield = Experimental yield (or "Actual") x 100! (p ) Theoretical yield ("what you should get") 2. Balance this reaction.! Al + CuSO 4 > Al 2 (SO 4 ) 3 + Cu a. How many mol of Cu would Theoretically be made from the reaction of mol of Al with excess CuSO 4? (This is the "Theoretical Yield")! (0.825 mol) b. In an Experiment, mol of Cu are actually produced by the reaction in part a. What is the % yield of the Cu?! (90.9%) c. How many grams of Cu would Theoretically be produced from the reaction of 1.87 g of Al with excess CuSO 4?! (6.60 g) d. What is the % yield of Cu if 3.74 g of Cu is experimentally produced (starting with the 1.87 g of Al as in part c)?! (56.7 %) 3. Use this balanced equation: SiO C > SiC + 2 CO! 50.0 g of SiO 2 is heated with an excess of C g of SiC is actually produced in the experiment. a. Calculate the theoretical yield of g of SiC. b. What is the % yield of the SiC in this reaction? (33.3 g, 96.9 %)
4 Limiting Reactant Problems (p ) Page 4 4. Balance this equation: K +! O 2 > K 2 O a. How many mol of K 2 O could be made from 2.80 mol of K? b. How many mol of K 2 O could be made from mol of O 2? c. So, if 2.80 mol of K reacts with mol of O 2, what is the Limiting Reactant?! What is the Excess reactant? How many mol of K 2 O can actually be made? d. How many mol of the excess reactant were used up in the reaction? e. How many mol of excess reactant are left over when the reaction is complete?! 5. Complete and Balance this equation:! Al + S > a mol of Al react with 7.20 mol of S. Calculate how many mol of product could be made starting with the 5.40 mol Al. Then starting with the 7.20 mol S. b. What is the limiting reactant? What is the excess reactant? c. How many Grams of product are actually made? d. How many mol of the Excess reactant were used up in the reaction? e. How many mol of excess reactant are left over when the reaction is complete?! 6. Balance this reaction: Ca + H 2 O > Ca(OH) 2 + H 2 a mol of Ca reacts with 2.50 mol of H 2 O. What is the Limiting reactant? b. How many mol of Ca(OH) 2 are actually made in the reaction? ans: 4a mol; b mol; c. LR=O 2, ER= K, 1.20 mol K 2 O; d mol K used; e mol K leftover; 5. 2Al +3S > Al 2 S 3, a mol, 2.40 mol, ; b. LR = S, ER= Al; c mol or 360 g Al 2 S 3 ; d mol Al used; e mol Al leftover; 6. LR = Ca, b mol Ca(OH) 2 made
5 L3: Review problems: Stoichiometry Name Page 5 1. Complete and Balance this double replacement reaction. (ans below)! Na 3 PO 4 (aq) + MgBr 2 (aq) > a. Assume 14.6 g of Na 3 PO 4 reacts with 19.5 g of MgBr 2. How many moles of NaBr could be made starting with the Na 3 PO 4? b. How many moles of NaBr could be made from the MgBr 2? c. Identify the Limiting reactant And the Excess reactant d. How many grams of NaBr are actually produced?! e. How many grams of the Excess reactant were used up in the reaction? f. How many grams of the Excess reactant are left over?! g of Aluminum Chloride reacts with excess Silver nitrate solution. An Insoluble solid is produced and is filtered from the solution. The mass of the Insoluble solid plus the filter paper is g. The mass of the filter paper was 0.46 g. a. Calculate the mass of the Insoluble product made in the experiment. b. Write the Complete, Balanced formula equation for the reaction.! Identify the formula for the Insoluble Product Mass(g) #Sig fig Filter paper + product Filter paper Insoluble Product % yield c. Calculate the Theoretical Yield of grams of Insoluble product that should have been made from the 3.50 g of Aluminum Chloride. d. Calculate the % yield of the Insoluble product. (1. 2 Na 3 PO MgBr 2 >Mg 3 (PO 4 ) NaBr; a mol; b mol, c. LR = MgBr 2 ; d g NaBr; e g Na 3 PO 4 used ; f g Na 3 PO 4 left; 2a g Silver chloride; b. AlCl 3 +3AgNO 3 > 3 AgCl(s) +Al(NO 3 ) 3 ; c g ; d. 91.2%)
6 3. The space shuttle uses monomethylhydrazine as a liquid fuel and dinitrogen! Page 6 tetroxide as a liquid oxidant. One possible balanced equation for the combustion is: N 2 H 3 CH 3 (l) + 2 N 2 O 4 (l) ----> CO 2 (g) + 3 H 2 O(l) + 3 N 2 O(g) a. How many mol of N 2 O 4 does the shuttle need to carry to oxidize 125 mol of N 2 H 3 CH 3?(250 mol) b. How many kg of H 2 O are expelled from the rocket engine along with 3000 g of CO 2?! (3.682 kg) c. How many grams of N 2 O 4 react to produce 75.0 mol of N 2 O?! (4600 g) d. How many Liters of N 2 O gas are produced along with 250 Liters CO 2? (both gases at STP) (750 L)! f. How many L of N 2 O gas (at STP) are produced from kg N 2 H 3 CH 3?! (168 L) 4. Balance this equation for the complete combustion of butane: (also use for #5) Ans below c! C 4 H 10 (g) + O 2 (g) ----> CO 2 (g) + H 2 O(g) a g of C 4 H 10 react with 65.0 L of O 2 gas at STP. Determine the Limiting reactant b. How many grams of CO 2 are actually made? c. How much of the excess reactant is used up? How much of the excess reactant is left over?! (2, 13 > 8, 10; a. O 2; b g CO 2, c. 3.2 g C 4H 10) 5. (same equation as 4) grams of C 4 H 10 are burned in excess O ml of CO 2 gas is experimentally produced at STP. a. What is the Theoretical Yield of ml of CO 2 gas? b. What is the % yield of CO 2 gas?! c. If you assume the same % yield as part b, how many grams of H 2 O would be produced by this experiment?! a. 247 ml; b % ; c g
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