1)Use standard thermodynamic data (in the Chemistry References) to calculate G at 298.15 K for the following reaction, assuming that all gases have a pressure of 19.31 mm Hg. 2N2(g) + O2(g)2N2O(g)
G = ? kJ/mol
2)Using standard thermodynamic data (linked), calculate the equilibrium constant at 298.15 K for the following reaction. C2H4(g) + H2O(g)CH3CH2OH(g)
K = ?
3) Calculate the temperature (in kelvins) at which the sign of G° changes from positive to negative for the reaction below. This corresponds to the temperature at which K < 1 changes to K > 1. Assume that ΔH° and ΔS° are constant and do not change with temperature. Fe3O4(s) + 4H2(g)3Fe(s) + 4H2O(g) ΔH° = 151 kJ/mol and ΔS° = 169 J/K ⋅ mol
T = ? K
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