University:
Missouri State University
Course:
CHM 160 | General Chemistry I
Academic year:

2020
Views:

342

Pages:

2
Author:

Nehemiah Rojas

Name KEY Period: Gas Stoichiometry Worksheet Directions: Use the gas laws we have learned to solve each of the following problems. Each of the chemical equations must first be balanced. Show all your work for credit. 1. When calcium carbonate is heated strongly, carbon dioxide gas is released according to the following equation: 100. Igna 1 CaCO₂(s) 1 Cao(s) + 1 CO₂(9) What volume of CO2(g), measured at STP, is produced if 15.2 grams of CaCO₂(s) is heated? 15.2glo aulas mollae 22.42804 100.19 Imatkallas mal = 3.40LC 2. The synthesis of sodium chloride occurs according to the reaction: 2.Na(s) + Cl2(g) 2NaCl(s) What volume of chlorine at STP is necessary for the complete reaction of 4.81 grams of sodium metal? 4.8/9 Na 100 No Imo/6/22~2.342612 3. Potassium permanganate is produced commercially by the this reaction: 7 KMnO(aq) + [Cl₂(g) 2 KMnO4(5) + 2KCl(aq) What volume of chlorine gas at STP would be required to produce 10.0 grams of KMnO4? 10.0 Imul And Imol Clz 122.44 1158 may 2 mol Aray Timal 200 709Liters 4. Consider the following unbalanced chemical equation for the combustion of propane: CH(g) +50%(9) 3 CO₂(g) H₂O(g) What volume of oxygen at 25°C and 1.04 atm is needed for the complete combustion of 5.53 grams of propane? P=1.04am T = 25% = 298k R=0.082/tes 5.5396548 Imal 6,6 Simol O2 628102 PU-ARTV-CF = (628) 60821) (+48k) = (14,810) (6281)(0821) (2988) (1.04am) 5. If water is added to magnesium nitride, ammonia gas is produced when the mixture is heated. Mg3N2(3) 3H₂O) + → + 2NH3(g) 3 MgO(s) When excess water is added to 10.3 grams of magnesium nitride, what volume of ammonia gas would be collected at 752m 24°C and 752 mmHg? 7 = 24n + 273 = 297H P=752m㎎ -.989atm Mo 10.39 MBN2 Imol mol Mg 12 Zmall 100.99 My No Imolyz -=:204mal NH3 PV-ART-DV = ART = (20) (00821) (247K) - 5.03LNHs P (989atm) 4 6. Ammonia and gaseous hydrogen chloride combine to form ammonium chloride according to this equation: NH(g) + HCI(g) NHCl(s) If 4.21 L. of NH(g) at 27°C and 1.02 atm is combined with 5.35 L of HCI(g)at 26°C and 0.998 atm, what mass of NH,CI(s) will be produced? Which gas is the limiting reactant? Which gas is the excess reactant? V=5.351 NH3 v = 4.21LN*H_{3} 1:27-273-300k m_{0}*P = 1.02atm R=0.0831 PYEART-DN=PV(1020tr) (4.216)/Pv (2082) (320k) 7-17%) musike Ima Hc T^ prime prime =26^ prime prime C + 3/290 * K Hel3 P R-0081 n= PV R 5 = (.999al.n)(0.354) (0.09pi*i)(209 1/2) = 0.218d Oxess ~ 3