The thermite reaction, Fe2O31s2 + 2 Al1s2 ¡2 Fe1s2 + Al2O31s2,...

Question

The thermite reaction, Fe2O31s2 + 2 Al1s2 ¡2 Fe1s2 + Al2O31s2, H = -851.5 kJ>mol, is one of the most exothermic reactions known. Because the heat released is sufficient to melt the iron product, the reaction is used to weld metal under the ocean. How much heat is released per mole of Al2O3 produced? How does this amount of thermal energy compare with the energy released when 2 mol of protons and 2 mol of neutrons combine to form 1 mol of alpha particles?

Accepted Answer

Identify the given enthalpy change (ΔH) for the reaction, which is -851.5 kJ. This value represents the heat released when the reaction proceeds as written.. Note that the stoichiometry of the reaction shows that 1 mole of Al2O3 is produced per reaction cycle. Therefore, the heat released per mole of Al2O3 produced is directly given by the ΔH of the reaction.. Understand that the comparison with nuclear reactions, such as the combination of protons and neutrons to form alpha particles, involves different scales of energy. Nuclear reactions typically release much greater amounts of energy per mole than chemical reactions.. To compare the energies, you would need the specific ΔH value for the nuclear reaction mentioned. This typically involves looking up or calculating the energy released based on mass defects and conversion into energy using Einstein's equation E=$$mc^2.. $$Finally, compare the magnitude of the energy released in the thermite reaction to that of the nuclear reaction to understand the scale and applications of each type of reaction.

비슷한 문제에 대한 검증된 영상 답변:

주요 개념

Thermodynamics and Enthalpy

Stoichiometry

Nuclear Reactions and Energy Release