Consider the reaction:  H2S(g)+SO2(g)---> 3S(g)+2H2O(l) for which delta H is -233 kJ and delta S is -424 J/K.  Assuming delta H and delta S do not depend on temperature, at what temperature is this reaction spontaneous?

For the reaction 2NO(g) + O2(g) → 2NO2(g), AH° = -113.1 kJ/mol and AS° = -145.3 J/K-mol. Under which temperature conditions would the reaction be spontaneous? Only at low temperatures Not possible to be spontaneous at all temperatures Only at high temperatures For all temperatures

For each of the following reactions indicate whether as written it will be spontaneous at all temperature only at high enough temperatures only at low temperatures not at any temperatures or if the given information is insufficient to draw a conclu

Given the data below, calculate the temperature at which the reaction becomes spontaneous:N2 (g) + 3 H2 (g) ⇌ 2 NH3 (g)(ΔH° = −92 kJ/mol and ΔS° = −199 J/mol K)

For a particular reaction, AH° = -93.8 kJ and AS° = –156.1 J/K. Assuming these values change very little with temperature, at what temperature does the reaction change from nonspontaneous to spontaneous? T = K Is the reaction in the forward direction spontaneous at temperatures greater than or less than the calculated temperature? less than greater than

What is the temperature at which the reaction below becomes spontaneous, if the standard entropies of reactants and products at 25oC are So (C(gr)) = 5.74 J/mol*K, So(H2(g)) = 130.68 J/mol*K, and So (C8H8(g)) = 345.2600J/mol*K and the heat of formation of C8H8(g)) is 147.8500 kJ/mol?C8H8(g) ↔ 8C(gr) + 4H2(g)a)661.88 Kb)707.958 Kc)the reaction is never spontaneousd)the reaction is always spontaneous

Consider the reaction below for the decomposition of carbon tetrachloride gas:  CCl4(g)    ------>     C(s)     +        2Cl2 (g)    ΔH = + 95.7 kJ;  ΔS = + 142.2 J/K  If the reaction above is not spontaneous at 25 oC, determine at what temperature (if any) the reaction becomes spontaneous.

The vaporization of compound A is described by the following chemical equation. A(1) A(g) AH vap (78.97 °C) = 37.87 kJ/mol Calculate the entropy of vaporization, A.Svap, for A(1) at 25.0 °C given that the boiling point of A is 78.97 °C, and the molar heat capacity of A(1) is 114.29 J/(mol K). Assume that the molar heat capacity of A(g) is 55.9% of that of A(1). ASvap = Calculate the standard enthalpy of vaporization, AHvap, for A(1) at 25.0 °C. AH vap = Calculate tl AG'vap = x10 TOOLS of vaporization, AGvap, at 25.0 °C. Determine the equilibrium constant K for the va 1970ea J. mol-1. K-1 kJ/mol kJ/mol

A reaction has AH°= 100 kJ/mol and AS°= 250 J/mol.K. Is the reaction spontaneous at room temperature? If not, under what temperature conditions will it become spontaneous?

Which are spontaneous at all temperatures? Choose one or more: 2H,0(g) + SO,(g) - 152.4 J/K 2H,S(g) +30,(g) AH°. rxn = - 1037 kJ, AS°. rxn → 2SO3(g) - 197.8 kJ, ASº. 2SO,(g) +O2(g) AH°. rxn - 187.8 J/K rxn O so,(8) + H,0(1) → H,SO4(1) AH°. rxn - 132.5 kJ, AS° - 169.9 J/K rxn S(g) +O2(8) –→ SO,(g) - 574.0 kJ, AS°, ΔΗ. rxn - 124.6 J/K rxn none of the above