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.)
Substance A has a molar mass of 100–120 gmol–1. When 3.14 g of A is burned, the only products are 4.68 g of CO2 and 1.44 g of H2O, formed at a 100% yield. When 4.17 g of A reacts with 0.25 g of H2, 1.77 g of C2H6O2 is produced, along with some CH3OH. What is the percent yield of this reaction?
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
If 7.3 grams of sodium carbonate are used in the reaction and the result a 74.0% yield, what is the actual yield(grams )of sodium phosphate will be formed? (Molar masses: Na2CO3 = 105.99 g/mol and Na3PO4 = 163.94 g/mol Sn3(PO4)4 + 6 Na2CO3 → 3 Sn(CO3)2 + 4 Na3PO4note please explain well, I asked this already and it lacks info for me.
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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Aqueous hydrobromic acid (HBr) reacts with solid sodium hydroxide (NaOH) to produce aqueous sodium bromide (NaBr) and liquid water (H2O). If 1.24 g of water is produced from the reaction of 22.7 g of hydrobromic acid and 4.82 g of sodium hydroxide, calculate the percent yield of water.
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?

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