University:
Cornell University
Course:
CHEM 1729 | Solve It!
Academic year:

2023
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187

Pages:

2
Author:

co2olkbp

Name Hour Date Stoichiometry Practice Quiz Honors Chemistry Show ALL work and include units (ex: mol H₂O) with your final answer!! 1. How many liters of oxygen are required to react completely with 1.2 liters of hydrogen to form water at STP? 2H2(g) + O2(g) 2H2O (9) 1.21112 x Imolotta x I moto02 x 22.4L02 0.6L02 22.412 2mottta I moto O2 2. How many molecules of NO2 are produced when 2.0 moles of N₂O are decomposed according to the following equation? [2.4×1024 molecules N2O4 → 2NO2 23 2.0 mol N204x 2 moto NO2, 6.02x102 molecules NO 3. How many liters of CO at STP are produced when 68.0g of CaCO, is heated according to the following equation? CaCO3 → CaO + CO2 68.09 CatO3x Imole Cal03 x Imoto CO2 x 22.4LC0215.2 X X 100.09 glat 03 I mololacoz Imote coa LC02 For #'s 5-6, use the following equation: 3Cu + 8HNO3 → 3Cu(NO3)2 + 2NO + 4H2O 4. Calculate the number of moles of water produced when 3.3 mol of Cu(NO3)2 are formed in the reaction. 3.3molCoNO3)2 x 4 mol H20 3 moLfo(NO3)2 =4.4mol H2O. 5. How many grams of Cu would be needed to react with 2.0 mol HNO3? 2.0mol HNO3x 3mottu * 63.55g(U=/47.7g Cu Smot #NO3 I moteu 192+96.21+5396 6. If a 500 g sample of aluminum sulfate is reacted with 450 g of calcium hydroxide, calculate the mass of calcium sulfate produced and identify the limiting reactant. Al2(SO4)3 + 3Ca(OH)2 → 2Al(OH)3 + 3CaSO4 136.15 15 500gA(504)3x Imolo Al(SO4)3 x 3mol x 10808glasoy 597 342.17g Al2(SO4)3 Imole 450g Ca(OH)2 x Imole (a(OH)2 x Imok Casoy 3mol 1309 CaSO4. 74.1g (a(0H)2 3 mol X Imo 6 Ca 504 = 650g 827 LIMITING REACTANT: A12(504)3 7. If 4.0 g of H₂ are made to react with excess CO, how many grams of CH3OH can theoretically be produced according to the following equation? CO + 2H2 → CH3OH 4.0g Hax Imol Ha X Imol CH3OH x 32.05g(H30H-31.79 2.029 Ha 2moletta Imole (B3OH CH3OH If 28.0 g of CH3OH are produced in the lab, what is the percent yield? % yield=28.0 x100=88% 31.7 8. What is the pressure, in atmospheres of a 0.108-mol sample of helium gas at a temperature of 20.0 °C if it s volume is 0.505 L? PV=nRT P(0.505L)=(0.108) (0.0821) (293K) P=5.14 atm 9. Calculate the grams of ammonia gas (NH3) contained in a 2L vessel at 350 K with a pressure of 3.25 atm. PV=nRT (3.25 atm) (2L)=n(0.0821)(350K) n=0.226 mol NH3 x 17.049 149 $3.85g NH3 Imol

Chem Stoichiometry Practice Solutions 2

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