Th given reaction is:
Fe + O2 -> Fe2O3
Balance Fe:
2 Fe + O2 -> Fe2O3
Balance O:
2 Fe + 3/2 O2 -> Fe2O3
Multiply all by 2 to remove fraction:
4 Fe + 3 O2 -> 2 Fe2O3
The equation now balanced.
The coefficient of Fe is 4
Answer: d
what is rhe coeffecient for iron after the following reaction is balamced Fe+O2-->Fe2O3 What is the...
Based on the balanced reaction 4 Fe + 3 O2 → 2 Fe2O3, a student starts this reaction with these amounts of chemicals: 12 mol Fe, 15 mol O2, and 0 mol Fe2O3. What chemical is the limiting reactant?
Based on the balanced reaction 4 Fe + 3 O2 → 2 Fe2O3, a student starts this reaction with these amounts of chemicals: 12 mol Fe, 15 mol O2, and 0 mol Fe2O3. What chemical is the excess reactant? SHOW WORK
Metallic iron can be made by the electrolysis of molten Fe2O3. (a) What mass of Fe is formed by passing a current of 9.15 A through molten Fe2O3 for 4.70 days? The unbalanced chemical reaction representing this electrolysis is shown below. Fe2O3 --> Fe + O2 ____ g of Fe is formed by this electrolysis. (b) How many minutes are needed to plate out 10.00 g of Fe from molten Fe2O3 using 7.29 A current? ____ minutes are needed.
Iron reacts with oxygen to produce iron(III) oxide. 4 Fe(s) + 3 O2(g) → 2 Fe2O3(s) If 4.03 moles of Fe react with excess O2, how many moles of Fe2O3 can be formed?
Consider the reaction: FeO (s) + Fe (s) + O2(g) → Fe2O3 (s) Given the following table of thermodynamic data at 298 K: Substance ΔHf° (kJ/mol) S° (J/K⋅mol) FeO (s) -271.9 60.75 Fe (s) 0 27.15 O2 (g) 0 205.0 Fe2O3 (s) -822.16 89.96 The value K for the reaction at 25 °C is ________. A.370 B.7.1 x 1085 C.3.8 x 10-14 D.5.9 x 104 E.8.1 x 1019
In the thermite reaction, iron (III) oxide is reduced by aluminum to give molten iron, Fe2O3 (s) + 2 Al (s) --> 2 Fe (l) + Al2O3 (s) If you begin with 10.0 g of Fe2O3 and 20.0 g Al, Which reactant is limiting? What mass of Fe can be produced? What mass of the excess reactant remains after the limiting reactant is consumed? Set up an amounts table for this problem.
Iron ore is converted to iron metal in a reaction with carbon. 2 Fe2O3 (s) + 3 C (s) ----------> 4 Fe (s) + 3 CO2 (g) If 2.24 moles of Fe2O3 are used, what amount of C is needed and what amounts of Fe and CO2, in moles are produced? _____ mol C _____ mol Fe _____ mol CO2
Select the balanced chemical equation for the synthesis of iron(III) oxide from its elements 4 Fe(s) + 3 O2(g) → 2 Fe2O3 2 Fe(s) + 3 O2(9) -2FeO3 Fe(s) + O2(g) – FeO2 Fe(s) + (g) - Feo Fe(s) + 3 O(g) - FeO3
The reaction of iron ore with carbon follows the equation: 2 Fe2O3+ 3 C 4 Fe+3 CO2 3. How many grams of Fe can be produced from a mixture of 200 g of Fe2O3 and 300. g of C?
3. Iron can be produced by the thermite reaction according to the following equation: Fe2O3 (s) +2Al (s) produces 2 Fe (s) + Al2O3 (s) a) If 100.0 g of Fe2O3 reacts with 30.0 g of Al, which one will be used up first? b) How much iron (in g) could be produced? c) If the only result in 45.0 g what is the percent yield?