Iron reacts with oxygen to form iron(III) oxide according to the chemical equation below. What is...
Iron reacts with oxygen to form iron(III) oxide according to the chemical equation below. What is the theoretical yield of product when 5.00 grams of Fe react with excess O2? [Molar masses: Fe, 55.85 g/mol; O, 16.00g/mol] 5 pts
4Fe(s) + 3O2(g) → 2Fe2O3(s)
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Iron reacts with oxygen to form iron(III) oxide according to the
chemical equation below. What is...
Iron reacts with oxygen at high temperatures to form iron(III) oxide. 4Fe(s)+3O2(g)⟶2Fe2O3(s) Suppose 14.2 g of...
Iron reacts with oxygen at high temperatures to form iron(III) oxide. 4Fe(s)+3O2(g)⟶2Fe2O3(s) Suppose 14.2 g of iron (Fe) is reacted with 18.1 g of oxygen (O2). Select the limiting reagent. Fe2O3 O2O2 FeFe Calculate the theoretical yield of iron(III) oxide (Fe2O3Fe2O3). theoretical yield = The reaction produces 5.40 g of Fe2O3. What is the percent yield of the reaction? percent yield =
An iron nail rusts when exposed to oxygen. According to the following reaction, how many grams...
An iron nail rusts when exposed to oxygen. According to the following reaction, how many grams of iron(III) oxide will be formed upon the complete reaction of 21.1 grams of oxygen gas with excess iron? 4Fe (s) + 3O2 (g) 2Fe2O3 (s)
iron and oxygen gas react to form iron oxide according to the chemical equation below 4...
iron and oxygen gas react to form iron oxide according to the chemical equation below 4 Fe +3 O2 = 2 Fe2O3 how many atoms of iron are required to react with 0.85 mol O2
Dry chemical hand warmers utilize the oxidation of iron to form iron oxide according to the...
Dry chemical hand warmers utilize the oxidation of iron to form iron oxide according to the following reaction: Part A 4Fe(s) + 3O2(g) 2Fe2O3(s) Standard thermodynamic quantities for selected substances at 25°C Calculate how much heat (in kilojoules) a hand warmer containing 28.0 g of iron powder produces. Express the energy in kilojoules to three significant figures. Reactant or product AH; (kJ/mol) EVO AQ R o 2 ? 0.0 Fe(s) O2(g) Fe2O3(s) 0.0 —824.2 k. Submit Previous Answers Request Answer...
Calculate w (in kJ) when 445 g iron (III) oxide (MM = 159.7 g/mol) reacts with...
Calculate w (in kJ) when 445 g iron (III) oxide (MM = 159.7 g/mol) reacts with excess carbon to produce carbon dioxide gas at 458 K: 2Fe2O3(s) + 3C(s) + 4Fe(s) + 3CO2(g) Answer: 511.64 x
Assume 117 grams of iron(III) oxide, Fe o reacts with excess hydrogen, H. The problem requires...
Assume 117 grams of iron(III) oxide, Fe o reacts with excess hydrogen, H. The problem requires that you determine the mass of iron, Fe, formed from this reaction. Fe, O (s) + 3 H (9) 2 Fe(s) + 3 H2O(1) 1 mol Fe 0, reus 159.70 g Fe,0, 55.85 g Fe --=81.8 g Fe Imol Fe
1. What mass of sodium nitride is required to produce 15.3g of nitrogen? 2Na3N → N2 + 6Na 2. What mass of oxygen will re...
1. What mass of sodium nitride is required to produce 15.3g of nitrogen? 2Na3N → N2 + 6Na 2. What mass of oxygen will react with 14.4 g of ethane according to the following reaction? 2 C2H6 + 7 O2 → 4 CO2 + 6 H2O 3. What mass of carbon dioxide will be produced from the complete reaction of 17.1 g of iron(III) oxide according to the following reaction? 2Fe2O3 + 3C → 4Fe + 3CO2 4. What mass...
5. Iron(III) oxide reacts with carbon monoxide to produce iron and carbon dioxide according to the...
5. Iron(III) oxide reacts with carbon monoxide to produce iron and carbon dioxide according to the following reaction: Fe2O3 + 3 CO → 2 Fe + 3 CO2 a) What is the percent yield of iron if 15.0 grams of FE is actually produced by reacting 65.0 of iron(III) oxide? b) What is the percent yield of carbon dioxide if the reaction produces 85.0 grams of carbon dioxide from 75.0 grams of carbon monoxide?
The reduction of iron (III) oxide to iron during steel making can be summarized by this...
The reduction of iron (III) oxide to iron during steel making can be summarized by this sequence of reaction: K1 2C(s) + O2(g) <--> 2CO(g) K2 Fe2O3(s) + 3CO(g) <--> 2Fe(l) + 3CO2(g) The net reaction is: K = 2Fe2O3(s) + 6C(s) + 3O2(g) <--> 4Fe(l) + 6CO2(g) Write an equation that gives the overall equilibrium constant K in terms of the equilibrium constants K1 and K2 .
Select the balanced chemical equation for the synthesis of iron(III) oxide from its elements Fe(s) +O(g)...
Select the balanced chemical equation for the synthesis of iron(III) oxide from its elements Fe(s) +O(g) + Feo Fe(s) + O2(g) + FO2 2 Fe(s) + 3 O2(g) - 2F03 4Fe(s) + 302() -2 70203 Fe(s) + 3 (a) --F03
Dry chemical hand warmers utilize the oxidation of iron to form iron oxide according to the following reaction: Part A 4Fe(s) + 3O2(g) 2Fe2O3(s) Standard thermodynamic quantities for selected substances at 25°C Calculate how much heat (in kilojoules) a hand warmer containing 28.0 g of iron powder produces. Express the energy in kilojoules to three significant figures. Reactant or product AH; (kJ/mol) EVO AQ R o 2 ? 0.0 Fe(s) O2(g) Fe2O3(s) 0.0 —824.2 k. Submit Previous Answers Request Answer...
Calculate w (in kJ) when 445 g iron (III) oxide (MM = 159.7 g/mol) reacts with excess carbon to produce carbon dioxide gas at 458 K: 2Fe2O3(s) + 3C(s) + 4Fe(s) + 3CO2(g) Answer: 511.64 x
Assume 117 grams of iron(III) oxide, Fe o reacts with excess hydrogen, H. The problem requires that you determine the mass of iron, Fe, formed from this reaction. Fe, O (s) + 3 H (9) 2 Fe(s) + 3 H2O(1) 1 mol Fe 0, reus 159.70 g Fe,0, 55.85 g Fe --=81.8 g Fe Imol Fe
5. Iron(III) oxide reacts with carbon monoxide to produce iron and carbon dioxide according to the following reaction: Fe2O3 + 3 CO → 2 Fe + 3 CO2 a) What is the percent yield of iron if 15.0 grams of FE is actually produced by reacting 65.0 of iron(III) oxide? b) What is the percent yield of carbon dioxide if the reaction produces 85.0 grams of carbon dioxide from 75.0 grams of carbon monoxide?
Select the balanced chemical equation for the synthesis of iron(III) oxide from its elements Fe(s) +O(g) + Feo Fe(s) + O2(g) + FO2 2 Fe(s) + 3 O2(g) - 2F03 4Fe(s) + 302() -2 70203 Fe(s) + 3 (a) --F03
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