A key step in the production of sulphuric acid is the oxidation of SO2(g) + O2(g) → 2SO3(g) At 98K, ΔGosys = - 500.51kJ; ΔHosys = - 494.61. kJ; and ΔSosys = -60.16 J/K a) Use the data to decide if this reaction is spontaneous at 25°, and predict how ΔGo will change with increasing T b) Assuming ΔHosys and ΔSosys are constant with increasing T, is the reaction spontaneous at 900oC?
A key step in the production of sulphuric acid is the oxidation of SO2(g) + O2(g) → 2SO3(g) At 98K, ΔGosys = - 500.51kJ; ΔHosys = - 494.61. kJ; and ΔSosys = -60.16 J/K a) Use the data to decide if this reaction is spontaneous at 25°, and predict how ΔGo will change with increasing T b) Assuming ΔHosys and ΔSosys are constant with increasing T, is the reaction spontaneous at 900oC?
Chemistry by OpenStax (2015-05-04)
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A key step in the production of sulphuric acid is the oxidation of SO2(g) + O2(g) → 2SO3(g) At 98K, ΔGosys = - 500.51kJ; ΔHosys = - 494.61. kJ; and ΔSosys = -60.16 J/K
a) Use the data to decide if this reaction is spontaneous at 25°, and predict
how ΔGo will change with increasing T
b) Assuming ΔHosys and ΔSosys are constant with increasing T, is the reaction spontaneous at 900oC?
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