Question

Iron reacts with oxygen at high temperatures to form iron(III) oxide. 4Fe(s)+3O2(g)⟶2Fe2O3(s)4Fe(s)+3O2(g)⟶2Fe2O3(s) Suppose 12.3 g12.3 g...

Iron reacts with oxygen at high temperatures to form iron(III) oxide.

4Fe(s)+3O2(g)⟶2Fe2O3(s)4Fe(s)+3O2(g)⟶2Fe2O3(s)

Suppose 12.3 g12.3 g of iron (Fe)(Fe) is reacted with 21.0 g21.0 g of oxygen (O2).(O2).

Select the limiting reagent.

FeFe

Fe2O3Fe2O3

O2O2

Calculate the theoretical yield of iron(III) oxide (Fe2O3Fe2O3).

theoretical yield =

g

The reaction produces 5.63 g5.63 g of Fe2O3.Fe2O3. What is the percent yield of the reaction?

percent yield =

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
1. In the following reaction, 451.4 g of lead reacts with excess oxygen forming 365.8 g...
1. In the following reaction, 451.4 g of lead reacts with excess oxygen forming 365.8 g of lead(II) oxide. Calculate the percent yield of the reaction. 2Pb(s)+O2(g) = 2PbO(s) 2. Assuming an efficiency of 32.60%, calculate the actual yield of magnesium nitrate formed from 119.8 g of magnesium and excess copper(II) nitrate. Mg + Cu(NO3)2 = Mg(NO3)2 + Cu 3. Combining 0.282 mol of Fe2O3 with excess carbon produced 18.8 g of Fe. Fe2O3 + 3C = 2Fe + 3CO...
How many moles of oxygen, O, are there in 479.07 g of iron (III) oxide, Fe2O3?...
How many moles of oxygen, O, are there in 479.07 g of iron (III) oxide, Fe2O3? Molar mass of Fe2O3 is 159.69 g/mol. 9.00 MOL 3.00 MOL 1.00 MOL 0.333 MOL From the Balanced Chemical Equation: 4 Al + 3O2 --> 2 Al2O3 Apply Stoichiometry to determine the yield (grams) of Al2O3 produced if you start with 108 grams of Al in excess O2 as reactants. Aluminum is the limiting reactant, and oxygen is present in excess. The formula weight...
Iron(III) oxide reacts with carbon to give iron and carbon monoxide. Fe2O3(s)+3C(s)→2Fe(s)+3CO(g) Part A: How many...
Iron(III) oxide reacts with carbon to give iron and carbon monoxide. Fe2O3(s)+3C(s)→2Fe(s)+3CO(g) Part A: How many grams of C are required to react with 19.9 g of Fe2O3? Part B: How many grams of CO are produced when 37.0 g of C reacts? Part C: How many grams of Fe can be produced when 5.60 g of Fe2O3 reacts? 2. How many moles of S are in each of the following quantities? Part A: 21 g of S (Express your...
Iron(III) oxide reacts with carbon monoxide according to the equation: Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g) A reaction mixture initially contains...
Iron(III) oxide reacts with carbon monoxide according to the equation: Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g) A reaction mixture initially contains 22.95 g Fe2O3 and 14.26 g CO. Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant is left?
Oxygen gas reacts with powdered iron according to the reaction: 4 Fe (s) + 3 O2...
Oxygen gas reacts with powdered iron according to the reaction: 4 Fe (s) + 3 O2 (g) → 2 Fe2O3 (s). What mass of Fe is required to completely react with 200.0 L of oxygen gas measured at 1055 mmHg and 71.2 °C?
The reaction between aluminum and iron(III) oxide can generate temperatures approaching 3000 degrees C and is...
The reaction between aluminum and iron(III) oxide can generate temperatures approaching 3000 degrees C and is used in welding metals: 2 Al + Fe2O3 = Al2O3 + 2Fe In one process, 126 g of Al are reacted with 601 g of Fe2O3 Calculate the mass, in grams, of Al2O3 formed
If 55.5 g of molten iron(III) oxide reacts with 30.1 g of aluminum, what is the...
If 55.5 g of molten iron(III) oxide reacts with 30.1 g of aluminum, what is the mass of iron produced? Fe2O3(l)+Al(l)⟶ΔFe(l)+Al2O3(s) Express your answer with the appropriate units.
In a crucible, a mixture of 15.325 g of iron (III) oxide and 25.734 g of...
In a crucible, a mixture of 15.325 g of iron (III) oxide and 25.734 g of aluminum metal is heated and the following reduction of the oxide takes place: Fe2O3 (s) + 2 Al (s) --> 2 Fe (l) + Al2O3 (l) a) What is the limiting reactant? b) Determine the maximum amount of aluminum oxide in grams that can be produced. c) Calculate the mass of excess reactant remaining in the crucible.
The chemical reaction that causes iron to corrode in air is given by 4Fe(s)+3O2(g)→2Fe2O3(s) and ΔrH∘...
The chemical reaction that causes iron to corrode in air is given by 4Fe(s)+3O2(g)→2Fe2O3(s) and ΔrH∘ = −1684 kJ mol−1 ΔrS∘ = −543.7 J K−1 mol−1 a) What is the standard Gibbs energy change for this reaction? Assume the commonly used standard reference temperature of 298 K. b) What is the Gibbs energy for this reaction at 3652 K ? Assume that ΔrH∘ and ΔrS∘ do not change with temperature. c) The standard Gibbs energy change, ΔrG∘, applies only when...
Iron(III) oxide reacts with carbon monoxide according to the equation: Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g) A reaction mixture initially contains...
Iron(III) oxide reacts with carbon monoxide according to the equation: Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g) A reaction mixture initially contains 23.00 g Fe2O3and 15.66 g CO. Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant is left?
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT