Given the following equation, calculate the mass of iron(III)
oxide necessary to
release 150 kJ of energy in the form of heat.
3Fe2O3(s) + CO(g) -> 2Fe3O4(s) + CO2(g) ^H = -39 kJ
Given the following equation, calculate the mass of iron(III) oxide necessary to release 150 kJ of...
What mass of iron(II) oxide must be used in the reaction given by the equation below to release 16.5 kJ? 6FeO(s) + O2(g) => 2Fe3O4(s) ΔH° = -635 kJ The answer is 11.2 g but I don't know how
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...
Calculate the standard free-energy change at 25°C for the reduction of iron (III) oxide with carbon monoxide: Fe,0,(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g) AG®(Fe,0,) = -742.2 kJ/mol AG (CO) = -137.2 kJ/mol AG® (CO2) = -394.4 kJ/mol
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 Fe304(s) and water(g) 00'9-HV (o'H+()oz(a)H+() How many grams of Fe,Os(s) would have to react to produce 0.778 kJ of energy?
The following thermochemical equation is for the reaction of iron(III) oxide(s) with aluminum(s) to form aluminum oxide(s) and iron(s). Al03(s)+ 2Fe(s) FezO3(s) + 2Al(s) AH = -852 kJ kJ of energy are When 48.5 grams of iron(III) oxide(s) react with excess aluminum(s).
The reduction of iron(III) oxide (Fe203) to pure iron during the first step of steelmaking 2 Fe2O3(s) 4 Fe(s) + 3 O2(g) is driven by the high-temperature combustion of coke, a purified form of coal: Cs)+O2(8) CO2(g) alo AG of CO2 and Fe,03 are Suppose at the temperature of a blast furnace the Gibbs free energies of formation Ar 447. kJ/mol and 801. kJ/mol, respectively. Calculate the minimum mass of coke needed to produce 3000. kg of pure iron. Round...
47. Iron (III) oxide reacts with carbon monoxide according to the equation: Fe2O3(s) + 3 CO(g) 2 Fe(s) +3 CO2(8) A reaction mixture initially contains 22.55 g Fe203 and 14.78 g CO. Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant remains?
The thermite reaction involves aluminum and iron(III) oxide forming aluminum oxide and liquid iron. Calculate the heat released in kJ per gram of aluminum reacted. The standard enthalpy of formation for liquid iron is 12.40 kJ/mol.
Blast furnaces extract pure iron from the iron(III) oxide in iron ore in a two step sequence. In the first step, carbon and oxygen react to form carbon monoxide: 2C (s) + O2 (g) → 2CO (g) In the second step, iron(III) oxide and carbon monoxide react to form iron and carbon dioxide: Fe2O3 (s) + 3CO (g) → 2Fe (s) + 3CO2 (g) Write the net chemical equation for the production of iron from carbon, oxygen and iron(III) oxide....