Consider following reaction:4 Al (s) + 5 O2 (9) → 2 Al2O5 (s)What mass of Al205 (in grams) is produced from the reaction of 12.00 moles of Al and 512.0 g of O2 if the reaction results in a 65.0% yield?Given molar masses: Al: 26.982 g/mol; O2: 31.998 g/mol; Al205: 133.96 g/molEnter the numerical value below (no untis), using 3 significant figures.Type your answer...

Answered: Image /qna-images/answer/523adda4-a3bc-4eeb-a0a0-90499c9b7498.jpg

Answered: Consider following reaction: 4 Al (s) +…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Iron(III) oxide (molar mass: 159.70 g/mol) reacts with carbon monoxide to produce iron and carbon dioxide. Fe2O3(s) + 3CO (g) à 2Fe(s) + 3CO2 (g). What is the theoretical yield for iron, if the reaction of 65.0 g of iron(III) oxide produces 38.0 g Iron?
Cryolite, Na3AlF6(s), an ore used in the production of aluminum, can be synthesized using aluminum oxide. Balance the equation for the synthesis of cryolite. equation: Al2O3(s)+NaOH(l)+HF(g)⟶Na3AlF6+H2O(g) If 17.3 kg of Al2O3(s), 54.4 kg of NaOH(l), and 54.4 kg of HF(g) react completely, how many kilograms of cryolite will be produced? mass of cryolite produced: ________ kg Na3AlF6 Which reactants will be in excess? -Al2O3Al2O3 -NaOHNaOH -HFHF What is the total mass of the excess reactants left over after the reaction is complete? total mass of excess reactants: _________ kg
C6H12 + 4 Br2 ¦ C6H8Br4 + 4 HBr Molar mass = 84.1 159.8 399.7 80.9 g/mol Based on the above equation, calculate the theoretical yield and percent yield of C6H8Br4 for an experiment where 15.0 g of C6H12 are reacted with 95.0 g Br2 to give 55.5 g of C6H8Br4. (Molar masses are given below each compound.)
If 6.89 g of calcium phosphide are produced from 12.45 g of calcium cyanide, what is the percent yield in the following unbalanced reaction? (molar masses: Ca(CN)2 = 92.12 g/mol, Co3P2 = 238.73 g/mol, Co(CN)2 = 110.97 g/mol, Ca3P2 = 182.18 g/mol) Ca(CN)2 + Co3P2 --> Co(CN)2 + Ca3P2
How many moles of Na2O (s) can be produced by the reaction of 0.7500 moles of Na (s) and 0.3000 moles of KNO3 (s) according to the equation below?10 Na (s) + 2 KNO3 (s) → K2O (s) + 5 Na2O (s) + N2 (g)------ moles of Na2O (s)
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2Na+Cl2->2NaCl is the balanced reaction for the formation of table salt. Given 20 grams of Ana and ten grams of Cl2, which reactant is in excess?How much NaCl should be produced from these amounts of the two reactants?
Elemental silicon can be produced by the reduction of silicon dioxide, or sand, with carbon: SiO2 + 2 C → Si + 2 CO When 35.0 kg of SiO2 react with 25.3 kg of C, 14.4 kg of Si are recovered. What is the percent yield for the reaction?
The balanced equation for the combustion of ethanol (CH3CH2OH) is CH3CH2OH (l) + 3O2 (g)2CO2 (g) + 3H2O (g) How many grams of water will be produced from 25 g of CH3CH2OH?
The fuel you burn in your car's engine contains octane, C3H18. When octane is burned, the products are CO2 and H20. 2C8H18(1) + 2502(g) → 16CO2(g) + 18H20(g) Emissions testing is an important tool for protecting our environment and informs car owners if their car is emitting too much CO2 while driving. Using the balanced equation above, answer the following questions. If 10.22 g of octane (C3H18 ) and 17.35 g of oxygen are used in the reaction, what is the limiting reactant and how much CO2 is produced?
For the balanced equation: 4NH3 (g) + 5 O2 ---- 4NO (g)+ 6H2O (l) If 2.3g of NH3 reacts with 4.5 g O2, how much NO is produced?
2NH3(g) + 3CuO(s)-> N2(g) + 3Cu(s) + 3H2O(g) What is the theoretical yield of solid copper that should form when 18.1 g of NH3 is reacted with 90.4 g of CuO? If only 45.3 g of copper is actually collected, what is the percent yield?

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