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3Fe(s) + 4H2O(g) Fe3O4(s) +

Iron will react with water to produce an iron oxide and hydrogen gas. Which equation below represents a correctly balanced
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Hydrogen is generated by passing hot steam over iron, which oxidizes to form Fe3O4 in the following equation.3Fe(s) + 4H2O(g) ->
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2. asked by Vachirawit
3. 2,619 views
For each reaction, calculate the moles of product (in parentheses) when 2.00 moles of each reactant is usedA: 2SO2 + O2 = 2SO3
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2. asked by Boo Boo
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How many grams of water and iron must react to produce 543 g of iron oxide, Fe3O4?3Fe + 4H2O---> Fe3O4 + 4H2
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2. asked by Christian
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For the reaction at equilibrium: 3Fe(s) + 4H2O(g) Fe3O4(s) + 4H2(g), removing some of the product, Fe3O4(s), would:Answer A.
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2. asked by ken
3. 3,596 views
3Fe(s) + 4H2O(g) <-> Fe3O4(s) + 4H2(g)What happens when Fe(s) is added? Would the reaction shift right?
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2. asked by scilover
3. 2,601 views
what type of reaction occurs Fe3O4 + 4H2 → 3Fe + 4H2O
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2. asked by Kyle
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3Fe + 4H₂O ⎯→ Fe₃O₄ + 4H₂ identify reducing and oxidising agent
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Use the reaction to calculate the mass of iron that must be used to obtain 0.500L of hydrogen at STP.3Fe(s)+4H2O(I)->Fe3O4(s)+4H
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2. asked by A
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Use the reaction shown to calculate the mass of iron that must be used to obtain 0.500 L of hydrogen at STP: 3Fe(s) + 4H2O(l)
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2. asked by jason
3. 3,858 views