Under what conditions is ∆Ssys < 0 for a spontaneous process?

Consider the following reaction between oxides of nitrogen: NO21g2 + N2O1g2 ¡ 3 NO1g2 Calculate ∆G at 800 K, assuming that ∆H° and ∆S° do not change with temperature. Under standard conditions is the reaction spontaneous at 800 K?

For a chemical reaction to be spontaneous at all temperatures, which of the following conditions must be met? O Itis not possible for a reaction to be spontaneous at all temperatures. O AS° > 0, AH > 0 O AS° > 0, AH 0

6. For each reaction below, determine the sign of AH and AS. Also state under what conditions the reaction is spontaneous (in the forward direction): (a) never spontaneous, (b) always spontaneous, (c) spontaneous at low temperatures, or (d) spontaneous at high temperatures. 1) C2 (g) → 2 Cl (g) (ii) 2 C2H6 (g) + 7 O2 (g) → 4 CO2 (g) + 6 H2O (g)

Under what conditions is N2 O3(g) ⟶ NO(g) + NO2(g) spontaneous?

For the reaction delta H° = 98.8 kJ/mol and delta S° =141.5 J/(mol*K). 3H2 (g) +Fe2O2(s) →2Fe(s) +3H2O(g) (19) Over what temperature range (if any) is the reaction spontaneous?

What is the sign of delta H and delta S for the reaction X(g) + Y(g) = XY(g) and state under what conditions would be spontaneous (in forward direction)?

At constant pressure, the reaction 2A(g) → B(g) is exothermic. Which of the following statements is true for this reaction? Select one: The reaction is never spontaneous at any temperature. The reaction is spontaneous at high temperatures. It is not possible to determine the spontaneity without more information. The reaction is spontaneous at all temperatures. The reaction is spontaneous at low temperatures.