CHEM 1050 Lecture Notes - Lecture 4: Exothermic Reaction, Exothermic Process
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1 Feb 2016
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Do the same for h and o in 3. 26 g of h2o. Recall: when you have an increase in the number of moles of gas (+ve) from reactants to products => there is lots of work done: The heat q increases the u internal energy => so it does work w against the force of atmosphere. Work = - p v and we know that : u = q + w. Move q to the left side: q = u + p v enthalpy ( h) Tells us that heat added to bring change at q is the sum of u and pv work. Enthalpy (h): most chemical reactions take place at constant pressure. H is the same as qp p means constant pressure. Heat added to the system at constant pressure. The enthalpies h of the products will be different than the enthalpies of the reactants. Change in h of the system going from reactants to products.
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