What are the oxidation states of iron in Fe2O3 and Fe3O4?
in fe2o3 in general oxygen shows the -2 so 3 oxygens shows the 3*-2 = -6
then for 2 Fe shows the +6
then for 1 Fe it shows the 6 / 2 = +3
in fe3o4 the 4 oxygens so 4*-2 = -8
the 3 Fe shows the +8 for the 1 Fe 8/3 = +2.67
answers = in fe2o3 fe = +3
= in fe3o4 fe = +2.67
Magnetite is a magnetic iron ore. Its formula is Fe3O4. (a) Construct a pair of conversion factors that relate moles of Fe to moles of Fe304 (b) Construct a pair of conversion factors that relate moles of Fe to moles of O in Fe3O4 (c) How many moles of Fe are in 2.75 mol of Fe304? (d) If this compound could be prepared from Fe2O3 and Oz, how many moles of Fe2O3 would be needed to prepare 4.50 mol Fe3O4?
. Use the following half reactions to answer questions about the corrosion of iron: Fe3O4 (s)→Fe2O3 s H aq+O2 g→H2O (l) A. (5 pts) Balance the two half reactions and combine to form a balanced overall equation. B. (5 pts) Using your overall balanced equation, determine the Gibbs free energy of the reaction at 25°C. C. (5 pts) Determine the Cell potential of this reaction. (Hint: You can use Gibbs) D. (5 pts) Determine the Equilibrium constant for this reaction...
Compare the quantities of heat released per mole of iron formed when oxides of Fe3O4 and Fe2O3 react with aluminium. 3Fe3O4 + 8Al -> 4Al2O3 +9Fe Delta Heat = -3347.6KJ Fezo3 +2Al -> Al2O3 +2Fe Delta Heat = -851.4KJ
1. Use the information provided to determine AH*rxn for the following reaction: 3 Fe2O3(s) + CO(g) → 2 Fe3O4(s) + CO2(g) AH*rxn = ? kl AH*t (kJ/mol Fe2O3(s) -824 Fe3O4(s) -1118 colg) -111 CO2(9) -394
2. Find out which sample of iron ore contains the highest iron content by calculating the mass percentage of iron in hematite (Fe2O3), magnetite (Fe3O4), and siderite (FeCO3)
06 Question (3 points) 0.600g of Fe3O4 reacts with excess O2 to give Fe2O3 in14.2% yield according to the following balanced equation. 4Fe,O(s)+02(8) 6Fe,0,(s) 2nd attempt Part 1 (1.5 points) Calculate the theoreical yield of Fe2Og Part 2 (1.5 points) Calculate the actual yield of Fe2O3 <06/09 8 OF 9 QUESTIONS COMPLETED
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.
The thermite reaction, used for welding iron, is the reaction of Fe3O4 with Al. 8 Al (s) + 3 Fe3O4 (s) \longrightarrow ⟶ 4 Al2O3 (s) + 9 Fe (s) Δ H° = -3350. kJ/mol rxn Because this large amount of heat cannot be rapidly dissipated to the surroundings, the reacting mass may reach temperatures near 3000. °C. How much heat (in kJ) is released by the reaction of 19.3 g of Al with 63.2 g of Fe3O4? Enter a...
How would I approach this problem?
0450g of Fe3O4 reacts with excess O2 to give Fe2O3 in25.0% yield according to the following balanced equation. 4Fe,04(s)+Og6Fe20,(s) 1st attempt Part 1 (1 pt) See Periodic Table Calculate the theoretical yield of Fe203 Part 2 (1 pt) ? See Hint Calculate the actual yield of Fe203. 9
what is rhe coeffecient for iron after the following reaction is
balamced Fe+O2-->Fe2O3
What is the coefficient for iron after the following reaction is balanced? Fe + 0, - Fe,0 Select one: а. 6 оооо