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Why are entropies absolute2/28/2024 ![]() ![]() C ΔG<0 because although energy is absorbed as the bond between the H and Clatoms forms, entropy increases because the number of gaseous product particles is less than the number of gaseous reactant particles. ![]() B ΔG>0 because energy is absorbed as the bond between the H and Cl atoms forms, and entropy decreases because the number of gaseous product particles is less than the number of gaseous reactant particles. Which of the following best explains why the reaction is thermodynamically favored? A ΔG>0 because energy is released as the bond between the H and Cl atoms forms, and entropy increases because the number of gaseous product particles is less than the number of gaseous reactant particles. H(g)+Cl(g)→HCl(g) The formation of HCl(g) from its atoms is represented by the equation above. Because ΔH is large and negative, the reaction will be not be thermodynamically favorable at any temperature. D There are more particles (including particles in the gas state) in the reactants than in the product, thus ΔSrxn>0. Because ΔH is large and negative, the reaction will be thermodynamically favorable at all temperatures. ![]() Which of the following correctly explains whether or not the reaction is thermodynamically favorable? A There are more particles (including particles in the gas state) in the reactants than in the product, thus ΔSrxn0. 4Fe(s)+3O2(g)⇄2Fe2O3(s)ΔH=−1,650kJ/molrxn The oxidation of Fe(s) is represented by the chemical equation above. ![]()
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