From this reaction 2NO(g) + 2H2(g) à N2(g) + 2H2O(1), NO H2 N2 Sᵒ (J/mol K) 75.10 191.5 192.3 AH'f -283.74 0 0 (kJ/mol) What is the entropy change (in J/K) of the system? H2O 189.0 -373.57

For each equation answer the following questions: i) What does each variable stand for? ii) What are the units of each variable? iii) Each is a way to calculate a change in entropy, but for what type of situation is each equation used? a) ΔS = qrev/T b) ΔS = nR ln(V2/V1) c) ΔS = C ln (T2/T1) d) S = k ln W e) ΔS = ΔHvap/Tb f) ΔS = ΔHfus/Tf

1:44 1 LTE 4 1 Search Question 20.b of 23 Show Answer Consider the reaction Cl2(g) + Br2(g) → 2 BrCI(g) at 25 °C. Which of the following best explains why the change in entropy is so small? A) All of the components in the chemical equation are gases. B) There are the same moles of gas on both sides of the reaction. C) The temperature of the reaction does not change. Tap here or pull up for additional resources

2 NH3 (g) + 2 O2 (g) → N20 (g) + 3 H2O (g) Is this reaction spontaneous only at low temperatures, only at high temperatures, at all temperatures? AH°r, kJ/mol s°, J/mol·K NH3(g) -46.1 192.5 0:(g) 205.0 N 20 (g) 82.1 219.9 H2O(g) |-241.8 188.7 AH°i, kJ/mol s°, J/mol·K What is the lowest temperature at which the following reaction is spontaneous? H2O (g) + C (s) → H2 (g) + CO (g) Co(g) H2(g) C (s) -110.5 | 197.7 130.6 5.7 H2O(g) |-241.8 188.7

Ip acellus_engine.html?ClassID=D1653724337# Calculate the entropy of the phase change of uranium hexafluoride from gas to solid. UF6(g) → UF6(s) Substance S° (J/mol-K) UF (s) UF (g) ASiep = [ ? ] J/mol - K 228 380 Enter either a + or - sign AND the magnitude in your answer. Enter

1)spontaneous or non spontaneous 2) the change in Gibbs free energy is negative or the change in Gibbs free energy is positive 3)positive or negative

For the reactionNH4NO3(aq)  N2O(g) + 2 H2O(l)G° = -175.3 kJ and H° = -149.6 kJ at 257 K and 1 atm.This reaction is (reactant, product)  favored under standard conditions at 257 K.The entropy change for the reaction of 1.74 moles of NH4NO3(aq) at this temperature would be  J/K.

llus_engine.html?ClassID=1653724337# Calculate the change in entropy for the reaction. H2(g) + l2(g) = 2HI(g) Substance S° (J/mol·K) H,(g) 1,(8) HI(g) 130.58 116.73 206.30 AS° = [ ? ] J/mol - K Enter either a + or - sign AND the magnitude in your answer. Enter

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