Use the data shown below, to calculate AH°rxn, AS°rxn, and AG°rxn at 25°C for the following reaction: 3 H2(g) + Fe2O3(s) → 2 Fe(s) + 3 H20(g) What is the value of AG°rxn at 25°C? FeOds Substance: AHr (kJ-mol) SJ-Kmol ) 130.7 Hag) Fels) HOle) -824.2 -241.8 87.40 27.28 188.8

At 25 oC liquid water is in equilibrium with water vapor with a Q = 0.0313. Please calculate ∆Gfor this equilibrium.

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

As shown here, one type of computer keyboard cleaner contains liquefied 1,1-difluoroethane 1C2H4F22, which is a gas at atmospheric pressure. When the nozzle is squeezed, the 1,1-difluoroethane vaporizes out of the nozzle at high pressure, blowing dust out of objects.Predict whether ∆S is positive or negative for this 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?

Two different gases occupy the two bulbs shown here. Consider the process that occurs when the stopcock is opened, assuming the gases behave ideally. Predict the signs of ∆H and ∆S for the process.

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.

Nitric oxides, NONO and NO2NO2, contribute to air pollution, acid rain, and the depletion of the ozone layer. After NONO forms in the combustion chamber of an automobile engine, it reacts further with oxygen to form NO2NO2. The reaction is given by: 2NO(g)+O2(g)→2NO2(g). Calculate ΔS∘rxn for the reaction?   Entropy values given by following table SubstanceSubstance S∘ (J/mol⋅K)S∘ (J/mol⋅K) NO2NO2 240.0 O2O2 205.2 NONO 210.8

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

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°