Sample Problem (mole-mass)



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Name: KEY Class: Sample Problem (mole-mass) Potassium chlorate is sometimes decomposed in the laboratory to generate oxygen. What mass of KClO 3 do you need to produce 0.50 moles of O 2? 2 KClO 3 (s) 2 KCl(s) + 3 O 2 (g). What do you know? (What are the facts?) Amount of O 2 in moles: 0.5 mol O 2 Where do you want to go? (What is the unknown?) Mass of potassium chlorate: mass of KClO 3 How do you get there? (conversion factor set-up) What steps are needed to calculate the mass of KClO 3 needed to produce 0.50 moles O 2? 0.5 mol O 2 x 2 mol KClO 3 x 122 g KClO 3 = 40.7 g KClO 3 1 3 mol O 2 1 mol KClO 3 Does it make sense? Are the units correct? yes 1

Practice Problems (Mole-Mass or Mass-Mole) 1. Phosphorus burns in air to produce a phosphorus oxide in the following reaction: 4 P (s) + 5_O 2 P 4 O 10 (s). a. What mass of phosphorus will be needed to produce 3.25 moles of P 4 O 10? 3.25 mol P 4 O 10 x _4 mol P x _31 g P_ = 403 g P 1 1 mol P 4 O 10 1 mol P b. If 0.489 moles of phosphorus burn, what mass of oxygen is used? What mass of P 4 O 10 is produced? (1) 0.489 mol P X 5 mol O 2 x 32 g O2 = 19.56 g O 2 1 4 mol P 1 mol O 2 (2) 0.489 mol P x 1 mol P 4 O 10 x 284 g P 4 O 10 = 34.72 g P 4 O 10 1 4 mol P 1 mol P 4 O 10 2. Hydrogen peroxide breaks down, releasing oxygen, in the following reaction: 2 H 2 O 2 (aq) 2 H 2 O (l) + O 2 (g) a. What mass of oxygen is produced when 1.840 moles of H 2 O 2 decompose? 1.84 mol O 2 x _1 mol O 2 _ x _32 g O 2 = 29.44 g O 2 1 2 mol H 2 O 2 1 mol O 2 b. What mass of water is produced when 5.0 moles O 2 are produced by this reaction? 5 mol O 2 x 2 mol H 2 O x 18 g H 2 O = 180 g H 2 O 1 2 mol H 2 O 2 1 mol H 2 O 3. Sodium carbonate reacts with nitric acid according to the following equation: Na 2 CO 3 (s) + _2_HNO 3 (aq) _2_NaNO 3 (aq) + CO 2 (g) + H 2 O(l) a. How many moles of Na 2 CO 3 are required to produce 100.0 g of NaNO 3? 100 g NaNO 3 x 1 mol NaNO 3 x 1 mol Na 2 CO 3 = 0.588 mol Na 2 CO 3 1 85 g NaNO 3 2 mol NaNO 3 b. If 7.50 g of Na 2 CO 3 reacts, how many moles of CO 2 are produced? 7.5 g Na 2 CO 3 x 1 mol Na 2 CO 3 x 1 mol CO 2 = 0.071 mol CO 2 1 106 g Na 2 CO 3 1 mol Na 2 CO 3 2

Sample Problem (mass-mass) Methane burns in air by the following reaction: CH 4 (g) + _2_O 2 CO 2 (g) + _2_H 2 O (g) What do you know? (What are the facts?) The mass of methane in grams 500 g CH 4 (Molar mass = 16 g ) Where are you going? (What is the unknown?) The mass of water produced unknown (Molar Mass = 18 g ) How do you get there? (conversion factor set-up) What steps are needed to calculate the mass of H 2 O produced from the burning of 500g of CH 4? 500 g CH 4 x 1 mol CH 4 x 2 mol H 2 O x 18 g H 2 O = 1125 g H 2 O 1 16 g CH 4 1 mol CH 4 1 mol H 2 O Does it make sense? yes 3

Practice Problems (Mixed Stoichiometry) To tell which equation process to use, look to the units on your fact and unknown. If your fact is in grams (mass) and the unknown is to be moles, then it is a mass to mole problem. If your fact is in mole, and the unknown is to be mole, then it is a mole to mole problem. Again, your units will let you know which process to use. 1. Ammonium hydrogen phosphate, (NH 4 ) 2 HPO 4, a common fertilizer, is made from reacting phosphoric acid, H 3 PO 4, with ammonia, NH 3. H 3 PO 4 + 2 NH 3 (NH 4 ) 2 HPO 4 a. If 10.0 g of ammonia react, how many moles of fertilizer will be produced? (mass-mol) 10 g NH 3 x 1 mol NH 3 x 1 mol (NH 4 ) 2 HPO 4 = 0.29 mol (NH 4 ) 2 HPO 4 1 17 g NH 3 2 mol NH 3 b. What mass of ammonia will react with 2800 kg of H 3 PO 4? (hint: convert kg to g) (mass-mass) 2800 kg H 3 PO 4 x 1000 g x 1 mol H 3 PO 4 x 2 mol NH 3 x 17 g NH 3 = 9.71x10 5 g NH 3 1 1 kg 98 g H 3 PO 4 1 mol H 3 PO 4 1 mol NH 3 2. The following reaction shows the synthesis of zinc citrate, and ingredient in toothpaste, from zinc carbonate and citric acid. _3_ZnCO 3 + _2_C 6 H 8 O 7 (aq) Zn 3 (C 6 H 5 O 7 ) 2 (aq)+ _3_H 2 O(l)+ _3_CO 2 (g) a. How many moles of ZnCO 3 and C 6 H 8 O 7 are required to produce 30.0 mol of Zn 3 (C 6 H 5 O 7 ) 2? (mol-mol) (1) 30 mol Zn 3 (C 6 H 5 O 7 ) 2 x 3 mol ZnCO 3 = 90 mol ZnCO 3 1 1 mol Zn 3 (C 6 H 5 O 7 ) 2 (2) 30 mol Zn 3 (C 6 H 5 O 7 ) 2 x _2 mol C 6 H 8 O 7 = 60 mol C 6 H 8 O 7 1 1 mol Zn 3 (C 6 H 5 O 7 ) 2 (mol-mass)b. What quantities, in kilograms, of H 2 O and CO 2 are produced by the reaction of 500 mol of citric acid? (hint: answer calculates to grams, then convert to kg.) (1) 500 mol C 6 H 8 O 7 x 3 mol H 2 O x 18 g H 2 O x 1 kg = 13.5 kg H 2 O 1 2 mol C 6 H 8 O 7 1 mol H 2 O 1000 g (2) 500 mol C 6 H 8 O 7 x 3 mol CO 2 x 44 g CO 2 x 1 kg = 33 kg CO 2 1 2 mol C 6 H 8 O 7 1 mol CO 2 1000 g 4

Source: Team 3, ICLCS Project, UIUC, 2007-08; IL State Stds: 11.A.4d; 11.5d; 12.C.5a 5

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