The following chemical reaction occurs on the seafloor:12 FeO(s) + 2 H2O(1) + CO2(g) → 4 Fe3O4(s) + CH4(g)Starting with 70.2 kg of FeO, how many kilograms of Fe3O4 will be produced if the percent yield for this reaction is 43.1 %?Assume that H20 and CO2 are present in excess.Given molecular masses: Fe0: 71.844 g/mol; Fe3O4: 231.531 g/molEnter the numerical value below (without units), using 3 significant figures.

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Answered: The following chemical reaction occurs…

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?
SO2(g) + H2O(l) → H2SO3(g) Given an initial mass of 14.12 g SO2, an excess of H2O, and assuming that all of the reactant is converted to product(s), and none is lost, calculate the mass (g) of H2SO3 produced by the reaction.
Lithium hydroxide is frequently used to neutralize sulfuric acid according to the equation: 2LiOH + H2SO4 ⟶ 2H2O + Li2SO4. If 5.6 g of LiOH reacts with 10.2 grams of H2SO4, what is the theoretical yield of water in this reaction? (In other words, how much water do you expect to produce?)
A sample of 62.3 g of tetraphosphorous decoxide (P4O10) reacts with 73.8 g of water to produce phosphoric acid (H3PO4) according to the following balanced equation. P4O10+6H2O⟶4H3PO4What is the limiting reactant for the reaction?Calculate the mass of H3PO4 produced in the reaction. Calculate the percent yield of H3PO4 if 37.9 of H3PO4 is isolated after carrying out the reaction.
How much (in gram) of HCl is required to produce 21.45 g of AlCl3 if the percentage yield for the following reaction is 61.24% ? Enter your answer without units. Molar masses (in g/mol):Al = 26.98H2 = 2.016HCl = 36.46AlCl3 = 133.34 2Al(s) + 6 HCl (aq) ⟶⟶ 2 AlCl3(s) + 3H2(g)
1) 2 Cu + S> Cużs When copper is heated with sulfur, the reaction above takes place. If 100. g of Cu is heated with 50.0 g of sulfur, which is the limiting reactant? What is the theoretical yield of Cu>S?
Consider following reaction: 4 Al (s) + 5 O2(g) ? 2 Al2O5(s) What mass of Al2O5 (in grams) is produced from the reaction of 5.00 moles of Al and 96.0 g O2 if the reaction results in a 75.0% yield?
Sodium hydroxide reacts with phosphoric acid to yield sodium phosphate and water. If 45 g of NaOH reacts with 35 g of H3PO4, what is the limiting reagent of this reaction if it yields a certain amount of NA3PO4? (Atomic masses: Na = 22.99 u ; O = 16.00 u; H = 1.01 u ; P = 30.97 u) Phosphoric Acid Sodium Hydroxide Water Sodium Phosphate 00
Condisder the balanced chemical equation shown. A table of molecular weights is given below.2 SiF4 (g) + Na2CO3 (s) + H2O (l) → Na2SiF6 (s) + SiO2 (s) + CO2 (g) + 2 HF (g)• How many grams of Na2SiF6 can be produced by the reaction of 70.00 grams of SiF4 and an excess amount of all other reactants?Answer in grams of Na2SiF6Molecular WeightsSiF4 104.077 g/molNa2CO3 105.988 g/molH2O 18.015 g/molNa2SiF6 188.053 g/molSiO2 60.083 g/molCO2 44.009 g/molHF 20.006 g/mol
When heated, Fe(OH) decomposes into Fe2O3 and water, according to the followingequation:2 Fe(OH)3 (s) > Fe2O3 (s) + 3 H20 (g)If 25.96 g of Fe(OH)3 decomposes, and 11.06 g of Fe2O3g are obtained in the reaction,what is the percent yield of the reaction?
Alcoholic fermentation converts glucose (C6H12O6) into ethanol (C2H5OH) and carbon dioxide (CO2). What mass of carbon dioxide can be formed from the alcoholic fermentation of 25.4 g of glucose?
Ethanol (C₂H₆O) is combusted in air according to the following reaction: C₂H₆O(l) + O₂(g) → CO₂(g) + H₂O(l) How many grams of water would be produced by the complete combustion of 6.45 moles of ethanol in the presence of excess oxygen?

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