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Titanium exists in nature as the mineral rutile, TiO2. One method of obtaining Ti is by heating the mineral in the presence of carbon. ΔS° has a value of + 366 J K−1 mol–1 for this reaction.
TiO2(s) + 2 C(s) Ti(s) + 2 CO(g)
Given that the standard enthalpy of formation of TiO2 (s) and CO (g) are –944 and –111 kJ mol−1 respectively, calculate ΔH ° and thus using the value given for ΔS °, estimate ΔG ° for the reaction at 2200 K assuming that that ΔS is independent of temperature.
*Comment on the feasibility of the reaction at this temperature and indicate why an endothermic reaction could be spontaneous.
in details plz
TiO2(s) + 2 C(s) Ti(s) + 2 CO(g)
Given that the standard enthalpy of formation of TiO2 (s) and CO (g) are –944 and –111 kJ mol−1 respectively, calculate ΔH ° and thus using the value given for ΔS °, estimate ΔG ° for the reaction at 2200 K assuming that that ΔS is independent of temperature.
*Comment on the feasibility of the reaction at this temperature and indicate why an endothermic reaction could be spontaneous.
in details plz