FCHAPJ REV[EW. Stoichiometry
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1 Date. FCHAPJ REV[EW. Stoichiometry :SE(TIQf$ I SHORT ANSWER Answer the following questions in the space provided. 1. b The coefficients in a chemical equation represent the (a masses in grams of all reactants and products. (h) relative number of moles of reactants and products. (c) number of atoms of each element in each compound in a reaction. (d) number of valence electrons involved in a reaction. 2. d Which of the following would not be studied within the topic of stoichiometry? (a) the mole ratio of Al to Cl in the compound aluminum chloride (b) the mass of carbon produced when a known mass of sucrose decomposes (c) the number of moles of hydrogen that will react with a known quantity of oxygen 2 (d> the amount of energy required to break the ionic bonds in CaF a A balanced chemical equation allows you to determine the (a) mole ratio of any two substances in the reaction. (b) energy released in the reaction. (c ele.tron configuration of all elements in the reaction. (d) reaction mechanism involved in the reaction. 4 C The relative number of moles of hydrogen to moles of oxygen that react to form water represents a(n) (a) reaction sequence. (b) bond energy. (C) mole ratio. (d) element proportion. 5. Given the reaction represented by the following unbalanced equation: N20(g) + 02(g) a. Balance the equation. 2N20(g) + 302(g) 2(g) 4N0 2(g) N0 4 mol N0 2:3 mol mol True False 5 What is the mole ratio of NO2 to 02? c. If 20.0 mol of NO consumed? d. Twice as many moles of NO True or False? e. Twice as many grams of NO True or False? 2 form, how many moles of 02 must have been 2 form as moles ofn20 are consumed. 2 form as grams ofn20 are consumed. p C, HJL I neh..r.,..5 -.h. e.erv. STOCHI0METRY 73
2 Name Date SECTION 1 continued PROBLEMS Wr[te the answer on the line to the left Show all your work in the space provided. 6. Given the Ibilowing eouation: N(g; ± 3H ç 2NH 3gl 28.0 g!mol N2 a. Determine to one decimal place the molar mass of each substance 2.0 g/mol H2 and express each mass in grams per mole g/rnol NH3 b. There are six different mole ratios in this system. Write out each one. 3 mol H2:1 mol N2; 2 mol NH 3:1 mol N2; 2 mol NH 3:3 mol H2; or their reciprocals 7. Given the following equation: 4NH(g) + 6N0(g) 1 5N2(g) ± 6H20(g) mol NO:1 mol H20 a. What is the mole ratio of NO toh20? 3 mol NO:2 mol NH3 b. What is the mole ratio of NO to NH3? 0,360 mol c. If mol of NH react according to the above equation. how many moles of NO will be consumed? 8. Propyne gas can be used as a fuel. The combustion reaction of propyne can be represented by the following equation: C3H4(g) + 4O2(g) 2(g) + 2H2O(g) > 3C0 a. Write all the possible mole ratios in this system. 4 mol 02:1 molc3h4; 3 mol C0 2:1 molc3h4; 2 mol H20:1 molc3h 3 mol C0 2:4 mol 02; 2 molh20:4 mol 0 2 moeh20:3 moe C0 or their reciprocals 2; b. Suppose that x moles of water form in the above reaction. The other three mole quantities (not in order) are 2x, equation above. I.5x. and 0.5x. Match these quantities to their respective components in the C3H4 is 0.Sx; 02 is 2x; and CO2 is 1.Sx 74STOICHIOMETRY C pyngh C) by FbH. Rrndart aid Wrnswn CC rtht reer.ed.
3 2NaOH(aq).. Date Class [.c..f1apter :R.EV1EW Stoichiometry [SECTION Z PROBLEMS Write the provided. 4,5 mol answer on the line to the left. Show all your work in the space The following equation represents a laboratory preparation for oxygen gas: 2KC10 3(s) 2KC1(s) ± 302(g) How many moles of 02 form if 3.0 mol of KCIO are totally consumed? g Given the following equation: H(g) Fg) * 2HF(g) How many grams of HF gas are produced as 5 mol of fluorine react? 0.53 g Water can he made to decompose into its elements by using electricity according to the following equation: 2H20(l) * 2H2(g) +02(g) How many grams of 02 are produced when mol of water decompose? ; / N C - v 34.8 g Sodium metal reacts with water to produce NaOH according to the following equation: 2Na(s) 2H20(l) + H2(g) How many grams of NaOH are produced if 20.0 g of sodium metal react with excess oxygen? Copyright by Holt, Rinehart and Wrnstvn. All rights reserved, STOICHIOMETRY 75
4 . Name Date Class SECTION 2 continued a. \ tt mash 01 ox aen Cas i pridui.ed it 100. of lithium c a C ti. I c o o g di I C1O c LCi(,; c. i h. The oxygen gas produced in part a has a density ot aiculate the olurne of thi as gil a. 6. A car air bag requires 70. L of nitrogen gas to inflate properly. The following equation represents the production of nitrogen gas: 81 g 3(s) 2NaN 2Na( ± 3N2(g) a. The density of nitrogen gas is typically 1.16 g/l at room temperature. Calculate the number of grams of N2 that are needed to inflate the air bag. 2.9 mol b. Calculate the number of moles of N7 that are needed. 1.3 x 1029 a. c. Calculate the number of grams of NaN 3 that must be used to generate the amount of N2 necessary to properly inflate the air bag., a STOICHIOMETRY (pvgh 0 by Heft. Rmebin and Winston. All ihts reserved.
5 Date (lass Stoichiometry PROBLEMS Write the answer on the line to the left, Show all your work in the space provided. 1 88% The actual yield of a reaction is 22 g and the theoretical yield is 25 g. Calculate the percentage yield mol of N2 are mixed with 12.0 mol of H2 according to the following equation: N2(g) + 3H2(g) 2NH 3(g) N2; 2.0 mol a. Which chemical is in excess? What is the excess in moles? 8.0 mol b. Theoretically, how many moles of NH 3 will be produced? 6,4 mol c. If the percentage yield of NH 3 is 80%, how many moles of NH 3 are actually produced? mol of Ca(OH) 2 are combined with mol of HCI according to the following equation: Ca(OH) 2(aq) + 2HC1(aq) * CaCI 2(aq) + 2H20(l) 0.10 mol a. How many moles of HC1 are required to neutralize all 0,050 mol of Ca(OH) 2? Cp n,tn J) y Hofl, Rinehart nd W nton. Ji righ reserei. STO!CHOMETRY 77
6 Dare Cias SECTION 3 continued b, What is He irniting reactan m this niutraiiiat in eactier c. How many grams of water will form in this reaction? 4. Acid rain can form in a two-step process, producing HNOi(aq) x 10 N2(g) + 202(g) 3N0(g) + HO(g) 2g) 2NO 3(aq) > 2HN0 ± NO(g) a. A car burns 420. g of N2 according to the above equations. How many grams will be produced? of HNO b. For the above reactions to occur. 02 must be in excess in the first step. What is the minimum amount 02 needed in grams? of 69 x c. What volume does the amount is 1.4 g/l? of 02 in part b occupy if its density 78 STOTCHIOMETRY Conht 0. I-loft. Rinehart nd Wirwon..!I rights re-et-sed.
7 Date [ PtE:R REVtEW Stoichiometry MIXED REVIEW SHORT ANSWER Answer the following questions in the space provided. 1. Given the following equation: C3H4(g) + x0(g) 2(g) + 2H20(g) 3C0 a. What is the value of the coefficient x in this equation? g/mol h. What is the molar mass of C3H4? 2 mol 02:1 mol H20 c. What is the mole ratio of 02 to H20 in the above equation? 0.20 mol d. How many moles are in an 8.0 g sample ofc3h4? 3z e. If z mol of C3H4 react, how many moles of CO2 are produced, in terms of z? 2. a. What is meant by ideal conditions relative to stoichiometric calculations? The limiting reactant is completely converted to product with no losses, as dictated by the ratio of coefficients. b. What function do ideal stoichiometric calculations serve? They determine the theoretical yield of the products of the reaction. c. Are actual yields typically larger or smaller than theoretical yields? smaller PROBLEMS Write the answer on the line to the left. Show all your work in the space provided. 3. Assume the reaction represented by the following equation goes all the way to completion: 3 N2 + 3H2 * 2NH 4 mol a. If 6 mo) of H2 are consumed, how many moles of NH3 are produced? b. How many grams are in a sample of NIT molecules 3 that contains 3.0 X 1023 Ccpyright 5 by Heft, Rinehart and Wieston. Ab rights reserved, STOICHIOMETRY 79
8 2Hg(I) Name MIXED REVIEW continued c. If 0.1 mol of N camhine sith H,. what rnut he true about the quantity of H for N- to he the limitiog reactant? 0.3 mol of H2 m ust be rovided. 4. 5% If a reaction s theoretical yield is 8.0 g and the actual yield is 6.0 g. what is the percentage yield? 5. Joseph Priestley generated oxygen gas by strongly heating rnercury(1i) oxide according to the following equation: mo! 2HgO(s) + 02(g) a. If 15.0 g HgO decompose. how many moles of HgO does this represent? mo! b. Ho many moles of 02 are theoretically produced? c. How many grams of 02 is this? d. If the density of 02 gas is 1.41 g/l, how many liters of 02 are produced? 1.05 e. If the percentage yield is 95.0%, how many grams of 02 are actually collected? 80 STOICHIOMETRY (1 pyrtght ) 1w ill It. Ritwh.trt and Vinoon. All nght reaerved.
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