Given the following thermochemical equation: Fe3O4(s) + 4H2(g) -> 3Fe(s) + 4H2O(l) q = -4020 kJ If a reaction has a heat change of -4940 kJ, what quantity of H2O in grams is produced?
Added by Carlos A.
Step 1
Determine the moles of Fe3O4 and H2 consumed in the reaction: - From the equation, we know that 1 mole of Fe3O4 reacts with 4 moles of H2 to produce 4 moles of H2O. - Therefore, the moles of Fe3O4 consumed in the reaction is: moles of Fe3O4 = moles of H2 / 4 Show more…
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The following thermochemical equation is for the reaction of Fe3O4(s) with hydrogen(g) to form iron(s) and water(g). Fe3O4(s) + 4H2(g) -> 3Fe(s) + 4H2O(g) ΔH = 151 kJ When 88.7 grams of Fe3O4(s) react with excess hydrogen(g), kJ of energy are absorbed. Hint: An amount of energy is expressed as a positive number. The sign of ΔH in the thermochemical equation indicates whether the energy is absorbed or evolved.
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The following thermochemical equation is for the reaction of Fe3O4(s) with hydrogen(g) to form iron(s) and water(g). Fe3O4(s) + 4H2(g) → 3Fe(s) + 4H2O(g) ΔH = 151 kJ When 76.6 grams of Fe3O4(s) react with excess hydrogen(g), how many kJ of energy are either evolved or absorbed? The following thermochemical equation is for the reaction of ammonium nitrate(s) to form dinitrogen monoxide(g) and water(g). NH4NO3(s) → N2O(g) + 2H2O(g) ΔH = -35.9 kJ How many grams of NH4NO3(s) would have to react to produce 7.18 kJ of energy?
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