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 =
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 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)
Iron reacts with oxygen at high temperatures to form iron(III) oxide
4Fe (s) + 3O2 (g) → 2Fe2O3 (s) Determine the number of electrons transferred for 1 g of fe (s) reacted
When 84.8 g of iron (III)oxide reacts with excess CO in the laboratory, 54.3 g of iron is isolated. Fe2O3 + 3 CO = 2 Fe + 3 CO2 What is the actual yield, the theoretical yield, and the percent yield?
help!! Name 1. Iron reacts with oxygen to form solid iron(IlI) oxide. a) Write a balanced chemical equation for the reaction. b) If 4.0g iron completely reacted, how many grams of iron(IlI) oxide would form? Work Check c) If 3.0g oxygen completely reacted, how many grams of iron(ll) oxide would form? d) If 4.0g iron reacted with 3.0g oxygen, which one would be the limiting reagent? e) How much iron(ll ) oxide would theoretically form? A student mixed 3.0g 02...
or HD Webcam HD Video Conferencing nment Score: 2283/4300 Resources Give Up? O tint Check Answer ion 33 of 43 > Iron reacts with oxygen at high temperatures to form iron(III)oxide. 4 Fe(s) + 30,(g) 2 Fe,0,() Suppose 22.7 g of iron (Fe) is reacted with 22.2 g of oxygen (0,). Select the limiting reagent. O Fe 002 OF, Calculate the theoretical yield of iron(III) oxide (Fe, 0). theoretical yield = The reaction produces 6.88 g of Fe, O. What...
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 .
Iron (III) oxide reacts with carbon monoxide to produce iron and carbon dioxide. Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g) Part A What is the percent yield of iron if the reaction of 67.0 g of iron(III) oxide produces 14.3 g of iron?
It is desired to produce 5.34 grams of iron(III)oxide by the following reaction. If the percent yield of iron(III)oxide is 85.4%, how many grams of iron would need to be reacted? grams iron iron(s) + oxygen(g) - iron(III) oxide(s) Submit Answer Retry Entire Group 2 more group attempts remaining The equation for this reaction is: 4 Fe(s) + 3 02(9) - Fe2O3(s)
4. What is the limiting reactant, theoretical yield, and % yield of iron metal (in kg) if 76.0 kg of Fe2O3 reacts with 22.1 kg of carbon to produce 42.3 kg Fe according to the following reaction: 2Fe2O3(s) + 3C(s) 4Fe(s) + 3CO2(g) Limiting Reactant - Fezoz Mass of Fe₂O₂ = 760kg Mole of Fe₂O₃ =475 grud Mass of carbon 22.1kg Mole of carbon = 1841.7 mol Theor. Yield =53.12 kg % Yield = 79.7%