acU3(S) decomposes lhto (S) and CO21g) at 1 atm the air around the reaction decreases in temperature. Rxn: CaCO3(s) → CaO(s) + CO2(g) Which statement is true about the decomposition of CaCO3(s) into CaO(s) and CO2(g) at 1.00 atm? The reaction is spontaneous at low temperatures. The reaction is spontaneous at all temperatures. The reverse reaction is spontaneous at all temperatures.

The reaction, Fe203(s) + 3C(s) → 2Fe(s) + 3CO(g) AH° = +490.7 kJ, AS° = +541 J-K-1 %3D This reaction is spontaneous only below a certain temperature always spontaneous never spontaneous spontaneous only above a certain temperature

Determine whether the following reactions are spontaneous or non-spontaneous. a) N2 (g) + 3 H2 (g) ⟶ 2 NH3 (g), ΔG = -32,960 J b) 2 NH3 (g) ⟶ N2 (g) + 3 H2 (g), ΔG = 32,960 J HINT: The change in free energy (ΔG) for reaction is equal to the difference in free energy between the products (Gproducts) and the reactants (Greactants): ΔG = (Gproducts) - (Greactants) In spontaneous reactions, the free energy of the products (Gproducts) of a reaction is less than the free energy of the reactants (Greactants). When this is the case, will the change in free energy (ΔG) will have a negative value or a positive value?

For a given reaction, dH = 32 kJ/mol and dS = 117 J/mol. At approximately what temperature would this reaction become spontaneous?

The following reaction is endothermic. 2NH3(g) → N2(g) + 3H2(g) This means the reaction   A. will be spontaneous at high temperatures. B. will be spontaneous at low temperatures. C. is not spontaneous at any temperature. D. is spontaneous at all temperatures.

49.For the decomposition of hydrogen peroxide to water and oxygen,         H2O2(g) ⟶⟶ H2O(g) + O2(g) ΔΔH° = -106 kJ, and ΔΔS° = +0.0580 kJ/K. In what temperature range is the reaction spontaneous (ΔΔG° < 0)? A. The temperature must be greater than 1.83××103 K B. The temperature must be less than 1.83 ××103 K. C. The temperature must be between 225 K and 1.83 ××103 K. D. ΔΔG° is always less than zero. E. ΔΔG° is never less than zero.

For each reaction, calculate ΔH°rxn, ΔS°rxn, and ΔG°rxn at 25 °C and state whether or not the reaction is spontaneous. If the reaction is not spontaneous, would a change in temperature make it spontaneous? If so, should the temperature be raised or lowered from 25 °C?a. 2 CH4( g)------->C2H6( g) + H2( g)b. 2 NH3( g)------> N2H4( g) + H2( g)c. N2( g) + O2( g)-------->2 NO( g)d. 2 KClO3(s)-------->2 KCl(s) + 3 O2( g)

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?

A reaction has a ΔH of -87.36 kJ and a ΔS of -175.3 J/K. At what temperature (in K) does the reaction become spontaneous?     626.4 K     This reaction is always spontaneous     498.3 K     434.6 K     This reaction is never spontaneous

From the values of ΔH and ΔS predict which of the following reactions would be spontaneous at 25°C. Calculate the minimum temperature at which each reaction will become spontaneous. Enter "None" if the reaction is not spontaneous at any temperature. ΔH = -75.8 kJ/mol,  ΔS = 126  J/K · mol