Calcium carbonate can be converted to quick lime by the following reaction: CaCO3(s) --> CaO(s) + CO2(g) Given that: for CaCO3(s) at 25Â°C DHfÂ° = -1206.9 kJ/mol SÂ° = 92.9 J/mol K, for CaO(s) DHfÂ° = -635.5 kJ/mol SÂ° = 39.8 J/mol K for CO2(g)) DHfÂ° = -393.5 kJ/mol SÂ° = 213.6 J/mol K Use these data to calculate DGo for the reaction.

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Limestone (CaCO3) is converted to calcium oxide (CaO) in a continuous kiln. The conversion process is represented by the following reaction: CaCO3(s) CaO(s) + CO2 (g) The energy to decompose the limestone is supplied by the combustion of CH4 in direct contact with the limestone using 50% excess dry air. The CaCO3 and air enter the process at 25 Â°C, and CaO exits at 900 Â°C. The product gases exit at 200 Â°C. Using the heat of reaction approach and the heat of formation and sensible heat approach, calculate the maximum number of kg of CaCO3 that can be processed per 1000 m3 of CH4 measured at standard conditions (i.e., 0 Â°C and 1 atm for gases). Show that the two approaches will produce similar results.

ïH o f, CH4, gas = -74.84 kJ/mol

Cp (for all gases and vapors): 30 J/mol.K

ïH o f, CaCO3, solid = -1206.9 kJ/mol Cp,CaCO3(s) = 234.5 J/mol.K

ïH o f, CaO, solid = -635.6 kJ/mol

Cp,CaO(s) = 111.8 J/mol.K

ïH o f, CO2, gas = -393.51 kJ/mol

ïH o f, H2O, gas = -241.83 kJ/mol

The reaction shown below is involved in the refining of iron.
2Fe2O3(s) + 3C(s, graphite) ? 4Fe(s) + 3CO2(g)
Compound ?HfÂ° (kJ/mol) SÂ° (J/mol/K) ?GfÂ° (kJ/mol)
Fe2O3(s) â824.2 ? â742.2
C(s, graphite) 0 5.740 0
Fe(s) 0 27.3 0
CO2(g) â393.5 213.6 â394.4
(6 pts) (a). Use data from the table above as needed to find ?HÂ°for the reaction.
(6 pts) (b). ?SÂ° for the reaction above is 557.98 J/K. Find SÂ° forFe2O3(s).
c)Calculate ?GÂ° for the reaction at the standard temperature of 298K. (There are at least 2
possible ways that you could do this.)
(7 pts) (d). At what temperatures would this reaction bethermodynamically spontaneous?

answers should be 9. (a). 467.9 kJ, (b). 87.4 J/K/mol, (c). 301.5kJ, (d). T > 839 K

Consider the decomposition of calcium carbonate: CaCO3 (s) -> CaO(s) + CO2(g).

Calculate the pressure in atm of CO2 in an equilibrium process (a) at 25 C and (b) at 800 C. Assume that delta H = 177.8 kJ/mol and delta S = 160.5 J/K mol for the temperature range