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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Ammonia is produced from the reaction of nitrogen and hydrogen according to the following balanced equation: N2(g) + 3H2(9) → 2NH3(g) 1. What is the maximum mass of ammonia that can be produced from a mixture of 191.3 g of N2 and 46.25 g of H2? 2. Which element would be completely consumed? (enter nitrogen or hydrogen) 3. What mass of the starting material would remain unreacted? Submit Answer Tries 0/10
For the reaction CH4 (g) + Cl2 (9) → CH3 Cl (g) + HCl (g) When 41.6 g of CHĄ and 84.0 g of Cl, reacts completely, what is the mass of HCl that could be produced? Molar mass: CH4 = 16.05 g mol-1; Cl2 = 70.90 g mol-1; HCI = 36.46 g mol-1 O 43.2 g O 94.5 g O 191. g O 18.3 g O 21.4 g
13. The theoretical yield of a reaction is the amount of product obtained if the limiting reactant is completely converted to product. Consider the reaction:H2(g) + C2H4(g) → C2H6(g) If 16.05 g H2 is mixed with 8.450 g C2H4, calculate the theoretical yield (g) of C2H6 produced by the reaction.
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.
Silver sulfadiazine burn-treating cream creates a barrier against bacterial invasion and releases antimicrobial agents directly into the wound. If 20.0 g Ag₂O is reacted with 40.0 g C10H10 N4 SO₂, what mass of silver sulfadiazine, AgC₁0 H, N4 SO₂, can be produced, assuming 100% yield? Mass= Ag2O(s) + 2C10 H10 N4 SO₂ (s) → 2 AgC₁0H₂N SO₂ (s) + H₂O(1) 10 g
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 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?

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