Consider the following reaction, known as the Haber process for the production of ammonia: N2(g) + 3 H2(g) <> 2 NH3(g) a)Calculate the ∆H°, ∆S°, and∆G° at 25.0 °C and determine if the reaction is spontaneous. b)Is the spontaneity of this reaction depend on temperature? •If yes, determine at what temperature (if any) the reaction becomes nonspontaneous.•If no, explain how you know the spontaneity is not temperature-dependent. c)Calculate the equilibrium constant at 25.0 °C.

Determine ∆S° for 2 O₃(g) → 3 O₂(g).   O₃ =239 S° (J/mol*k) O₂ = 205 S° (J/mol*k)

Calculate the Free Gibb’s Energy, kJ/mol, at 298 K for the following reaction.  2CaSO4(s)→2CaO(s) + 2SO2(g) + O2(g) Substance ∆H(kJ/mol) ∆S (J/K mol) CaSO4(s) -1432.69 106.69 CaO(s) -635.6 39.8 SO2(g) -296.4 248.5 O2(g0 0 205.0

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 the following reaction, ΔH° is 47.7 kJ/mol and ΔS° is 81.8 J/mol*K. At what temperature in K will the reaction become spontaneous? A2D(g) + C3(g) → 2AC(g) + DC(g)

6) The reaction below shows how coal (carbon) can be converted to methane (natural gas): C(s)       +              2                                            H2(g)          -------->       CH4(g) Using the data provided, compute ∆G° at 25°C and then find the equilibrium constant K for the reaction;          Is the reaction spontaneous or non-spontaneous? Compound ∆Hf ∆Sf CH4 –74.848 kJ/mole 186.2 J/mole K H2 0 130.6 J/K mol K C(s) 0 5.69 J/K mole K Find the temperature at which the reaction changes  Find ∆G and Keq at 1000 K.

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?

The element gallium (Ga) freezes at 29.8°C its ΔHfus = 5.59 kJ/ mol. Calculate the valueof ΔS when 1.0 mol gallium freezes at its normal melting point. Is ΔS positive ornegative? Calculate the value of ΔS when 30.0 g of Ga(l) solidifies at 29.8 °C

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

Consider the reaction, O2(g) ⇌ 2 O(g) where ∆H° = 498 kJ/mol at 25°C.  At what temperatures (high or low) the reaction would more likely to be spontaneous?  Predict the sign of ∆S°