Hi!
The first step for this problem is to convert our 55.0 kg of Fe3O4 to moles using the molar mass (231.55 grams per mole). Note: we need to convert 55.0 kg to grams first!
Next, we look at the balanced reaction equation given in the problem and see that for every 1 mole of Fe3O4 that is decomposed, +1118 kJ of energy is required. We use this to determine how much energy is required to decompose 237.53 moles:
So, we need 265,558.0 kJ of energy to decompose 55 kg of Fe3O4. That's a lot of energy!
I hope this helps! Please rate if it does : )
According to the following reaction, how much energy is required to decompose 55.0 kg of Fe3O4? The molar mass of Fe3O4...
According to the following reaction, how much energy is required to decompose 55.0 kg of Fe3O4? The molar mass of Fe3O4 is 231.55 g/mol. Fe3O4(s) ? 3 Fe(s) + 2 O2(g) ?H°rxn = +1118 kJ
Please help with these two questions :( 1. How much energy (in kJ) is evolved during the reaction of 76.9 g of Al, according to the reaction below? Fe2O3(s) + 2 Al(s) → Al2O3(s) + 2 Fe(s) ΔH°rxn = -852 kJ Assume that there is excess Fe2O3. 2. A 12.43 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter with a heat capacity, C = 5.65 kJ/°C. C2H5OH(l) + 3 O2(g) → 2 CO2(g) + 3 H2O(g) ΔH°rxn...
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...
he 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) \Delta 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 16 g of Al with 76.3 g of Fe3O4? Enter...
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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
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How much energy is evolved during the reaction of 53.4 g of Al, according to the reaction below? Assume that there is excess Fe2O3. Fe,Og(s) + 2 Al(s) + AlzO3(s) + 2 Fe(s) AHnx = -852 kJ 53.4 kJ O 843 kJ 430 kJ 1686 kJ 215 kJ Using the following equation for the combustion of octane, calculate the heat of reaction for 400.0 g of octane. The molar mass of octane is 114.33 g/mole 2 CH + 25 02...
How much energy is evolved during the reaction of 273 g of Fe 2O 3, according to the reaction below? Assume that there is excess Al. Fe 2O 3(s) + 2 Al(s) → Al 2O 3(s) + 2 Fe(s) ΔH°rxn = -852 kJ
Question 7 1 pts The thermite reaction, used for welding iron, is the reaction of Fe3O4 with Al. 8 Al(s) + 3 Fe3O4 (s) —+ 4 A1203 (s) + 9 Fe (s) AH° = -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 17.2 g of Al with 70.5 g of Fe3O4? Enter...