Given that
3Fe2O3(s) +H2(g) ----- > 2 Fe3O4 (s) + H2O (g)
dH = -6.00 KJ
given that energy which is produce = 0.778 kj
Number of moles = 0.778 KJ * 3 mole Fe2O3 / 6.00 KJ
=0.389 mole Fe2O3
Amount in g = number of moles * molar mass
=0.389 mole Fe2O3*159.69 g/mol
= 62.1 g Fe2O3
The following thermochemical equation is for the reaction of iron(III) oxide(s) with hydrogen(g) to form Fe304(s)...
The following thermochemical equation is for the reaction of iron(III) oxide(s) with hydrogen(g) to form iron(s)and water(g). Fe2O3(s) + 3H2(g)—2Fe(s) + 3H2O(g) AHexn98.8 kJ How many grams of Fe2O3(s) would react if 36.2 kJ of energy were provided? grams Submit Answer
The following thermochemical equation is for the reaction of iron(III) oxide(s) with hydrogen(g) to form iron(s) and water(g). Fe2O3(s) + 3H2(g)— 2Fe(s) + 3H2O(g) AH = 98.8 kJ When 62.3 grams of iron(III) oxide(s) react with excess hydrogen(g), kJ of energy are Hint: An amount of energy is expressed as a positive number. The sign of AH in the thermochemical equation indicates whether the energy is absorbed or evolved. An automobile engine provides 523 Joules of work to push the...
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