27-09-10 - Reaction releases energy o Enthalpy = delta h...

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Monday, September-27-10 - For page 19 – question o 1) w=0, delta u = q = -3 x 186.4 kJ o H = u + PV o Delta h = Delta u + delta (PV) o Delta PV = p(delta v) + (v delta p) o =0 =0 o Unusual case because delta H is equal to delta U - Enthalpy change of chemical reactions o + enthalpy values = endothermic reaction Means enthalpy of the products is higher than the enthalpy of the reactants And for the reaction to go through it requires energy to go into equivalence Reason why we can’t split water to extract hydrogen out of water o The enthalpy value between them Is a huge value and you need to much heat or energy to split it which you cannot do in industry realistically o – enthalpy = exothermic reaction
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Unformatted text preview: Reaction releases energy o Enthalpy = delta h Enthalpy is a state function If enthalpy goes towards a reaction then goes back it should be 0 because it went through a cycle. o Hesss Law The change in enthalpy is independent to the reaction path No matter how a reaction proceeds in how many steps the enthalpy change should be the same o Enthalpy of solution o Standard reaction enthalpy Standard conditions : t = 298 K p = 1 atm Standard State: H 2 (g) H 2 o(l) MgO(s) etc. Delta H for a reaction in which a compound is formed from its elements in their standard states-...
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27-09-10 - Reaction releases energy o Enthalpy = delta h...

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