Explain how thermodynamic stability differes from kinetic stability. Can a substance or system be stable from one perspective but not the other?

8  a) -511.3 kJ   B) +511.3 kJ  NS) -697.5kJ    D) +697.5kJ  TO) -47.3 kJ

How could the calculated enthalpy be used to determine the minimum entropy required for a spontaneous process? Why is this known to be the minimum required entropy?

What happens to the entropy of an isolated system during an irreversible process?

Entropy is the randomness of a system. At the molecular level, entropy can be described in terms of the possible number of different arrangements of particle positions and energies, called microstates. The more microstates the system has, the greater its entropy. Another way of looking at entropy is that the universe is moving toward a broader distribution entropy has since been constantly increasing by distributing this energy. Heat distribution from high temperature to low temperature is a another example of this phenomenon. energy. The universe has a constant amount of energy as stated in the first law of thermodynamics. The universe started with low entropy (concentrated in the moment before the "big bang") and the Part A Rank these systems in order of decreasing entropy. Rank from highest to lowest entropy. To rank items as equivalent, overlap them. > View Available Hint(s) Reset Help Greatest entropy Least entropy 1 mol of helium gas at 273 K and 20L 1 mol of 1 mol of helium gas…

15. In which of the following systems is(are) work done by the surroundings on the system? AsSsume pressure and tempera- ture are constant. a. 2S0,(g) + 0,lg) → b. CO,(s) c. 4NH,(g) + 70,(g) → 4NO,(g) + 6H,O(g) d. N,O,(g) e. CACO;(s) –→ CaCO(s) + CO,(g) → 2S03(g) CO,(g) > → 2NO,(g) >

ΔHrxn∘=− 85 kJ, ΔSrxn= 154 J/K, T= 392 K Find ΔSuniv

Calculate for the Delta H (enthalpy) of the reaction below given the following data: 2NH3(g) + 3N₂O(g) →→→ 4N₂(g) + 3H₂O(l) N₂O(g) + 3H₂(g) →N₂H4(l) + H₂O(l) N₂H4(l) + O₂(g) H₂(g) + O₂(g) -141 kJ -163 kJ -450 kJ +356 kJ +150 kJ -131 kJ 2NH3(g) + O₂(g) →→→→N₂H4(1) + H₂O(l) -231 kJ - N₂(g) + 2H₂O(l) H₂O(l) AH-1010. kJ AH = -317 kJ AH = -623 kJ AH = -286 kJ

Calculate the ∆H°rxn for the reaction C(graphite) + 2H2(g) → CH4(g)from the following enthalpy changes: - Cgraphite + O2(g) → CO2(g)                        ∆H = -393.5 kJ - 2H2(g) + O2(g) → 2H2O(l)                          ∆H = -571.6 kJ - CH4(g) + 2O2(g) → CO2(g) + 2H2O(l)      ∆H = -890.4 kJ

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