D)ΔG<0 because although entropy decreases because the number of gaseous product particles is less than the number of gaseous reactant particles, energy is released as the bond between the H and Cl atoms forms. Internationally agreed, internally consistent, values for the thermodynamic properties (standard enthalpy of formation, entropy and H(298)-H(0)) of key chemical substances. D) Entropy increases with the number of microstates of the. C) The total entropy of the universe increases in any spontaneous process. B) Any irreversible process results in an overall increase in entropy. C) ΔG<0⁢ because although energy is absorbed as the bond between the H and Cl atoms forms, entropy increases because the number of gaseous product particles is less than the number of gaseous reactant particles. A) The change in entropy in a system depends on the initial and final states of the system and the path taken from one state to the other. B) ΔG>0because 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. Standard Entropy is defined as the absolute entropy of a substance at 25 C.

Any sample less ordered than a perfect crystal will have a positive entropy. (Remember, there is no way to determine absolute enthalpy.) The entropy of any substance at a finite temperature will be greater then zero. 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. crystal at absolute zero has zero entropy. 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. The more microstates the system has, the greater its entropy. Because ΔH is large and negative, the reaction will be thermodynamically favorable at all temperatures. At the molecular level, entropy can be described in terms of the possible number of different arrangements of particle positions and energies, called microstates. 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.

What is the absolute entropy of o2