Identify whether the entropy change is positive, negative, or equal to zero, for each process. Part 1 of 4 XeF (g) AS is (Choose one) Part 2 of 4 20(g) Part 3 of 4 AS is (Choose one) 2HgO(s) Xe(g) + 2 F₂ (g) 0₂ (8) Part 4 of 4 AS is (Choose one) X 2Hg(1) + O₂(g) X AS is (Choose one) × 3H₂(g) + N₂(g) 2NH₂ (g) x

Consider the combustion of propane gas:  C3H8(g)    +     5O2(g)           ------>           3CO2(g)        +            4H2O(g)            ΔHrxn  =  - 2044 kJ  Determine the sign of the entropy change for the system.

For each of the following reactions determine if the change in entropy was positive or negative:A) Water at 40°C → Water at 25°CB) 2NO2(g) → N2O4(g)C) CH3OH (l) → CH3OH (g)D) PbCl2(s) → PbCl2(aq)

Does the entropy increase or decrease in these reactions? Why? a) 4 Al + 3 O2 → 2 Al2O3 b) C + 2 Cl2 → CCl4 c) H2O (l) → H2O (g) d) CCl4 → C + 2 Cl2

What is the change in entropy, AS, for the following reaction? Use Table G in your book for values of standard entropies. Your answer should be in J/K mol. CaCO3(s) + 2 H'(aq) → → Ca² (aq) + H₂O(l) + CO2(g) O 264.9 J/K mol O 118.6 J/K mol 394.3 J/K mol 137.7 J/K mol 2

For each reaction, calculate ΔHrxn°, ΔSrxn°, and ΔGrxn° at 25 °C and state whether or not the reaction is spontaneous. If the reacton is not spontaneous, would a change in temperature make it spontaneous? If so, should the temperature be raised or lowered from 25 °C? 2 CH4(g) → C2H6(g) + H2(g) 2 NH3(g) → N2H4(g) + H2(g)

One mole of an ideal gas undergoes the cycle, A⟶B⟶C⟶A, as shown in the graph. For this gas, CV = 1.5R.  Step C⟶A is isothermal and reversible. 1) calculate ΔT, q, w, ΔU, ΔH, and ΔS for each step in the process.

Use the data to calculate the standard entropy change for the following reaction: 5. S°[Mt(s)] 43.2 J/K mol Mt(s) + ½ O2(g) → MtO(s) S°[O2(g)] = 305.1 J/K-mol S°[MtO(s)] 62.6 J/K mol a) -133.2 J/K b) -285.7 J/K c) 285.7 J/K d) 133.2 J/K

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