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Bond Enthalpies

Descrição

A level Chemistry (3.2 Physical Chemistry) FlashCards sobre Bond Enthalpies, criado por Yinka F em 05-03-2018.
Yinka F
FlashCards por Yinka F, atualizado more than 1 year ago
Yinka F
Criado por Yinka F quase 7 anos atrás
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Resumo de Recurso

Questão Responda
What is bond dissociation enthalpy? The energy needed to break one mole of the bond to give separated atoms - everything being in the gaseous state
Compare the energy required to break bonds with the energy released when bonds are made during an exothermic reaction Less energy is needed to break bonds than is released when bonds are made Released > needed
Compare the energy required to break bonds with the energy released when bonds are made during an endothermic reaction More energy is needed to break bonds than is released when bonds are made Needed > released
Nitrogen reacts with hydrogen to form ammonia in the reaction: N₂ + 3H₂ --> 2NH₃ The energy needed to break all the bonds in N₂ and H = 2253kJmol⁻¹ The energy released when forming the bonds in NH₃ = 2346kJmol⁻¹ Is this reaction endothermic or exothermic? The amount of energy released is bigger than the amount needed, so the reaction is exothermic (ΔH is negative)
What is the name for the difference between the energy absorbed and released? Enthalpy change of reaction Enthalpy change of reaction = (total energy absorbed) - (total energy released)
Calculate the enthalpy change for the following reaction: N₂ + 3H₂ --> 2NH₃ Bonds broken = 945 +3(436) =2253kJmol⁻¹ Bonds formed = 6(391) = 2346kJmol⁻¹ Enthalpy change of reaction = 2243 - 2346 = -93kJmol⁻¹ (exothermic)

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