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Chemistry
Calculating Energy Released by Sodium Reacting with Water
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[QUOTE="xpell, post: 6522962, member: 397416"] Hi! After watching a couple videos about the explosive reaction of sodium in freshwater and seawater, I felt curious and wanted to calculate how much energy is released. However, my Chemistry is super rusty and I think that my result is way too high (equivalent to [URL='https://en.wikipedia.org/wiki/TNT_equivalent']almost 2 g of TNT[/URL] per gram of sodium!) Would you please confirm or tell me where did I mess it up:? The balanced equation for the reaction is: 2Na + 2H2O → 2NaOH + H2 Change in enthalpy for the reaction at 20ºC (ΔH20C) is: -368.6 kJ. So, the energy released in the reaction = 368.6 kJ Mass of 2Na (2 moles of sodium) = 23 x 2 = 46 grams Energy released for 46 grams of sodium = 368.6 kJ Hence, energy released for 1 g of sodium = 368.6/46 = 8,013 J ≈ 8 kJ (!) PS. If someone is so kind to tell me how to calculate this under different conditions of water pressure / temperature, I'd appreciate it a lot too. [/QUOTE]
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Calculating Energy Released by Sodium Reacting with Water
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