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Free Energy of Formation

N2_2 (g) + 3 H2_2 (g) \leftrightharpoons 2 NH3_3 (g)

For the reaction above, calculate the free energy of formation, \triangleGf_f^\circ for each of the products and reactions.

Posted by Katie Adams 8 months ago

Related Problems

N2_2 (g) + 3 H2_2 (g) \leftrightharpoons 2 NH3_3 (g)

For the reaction above, what is the sign and value of entropy for the reaction, given:

H2_2 (g), S^\circ(at 25^\circC) = 130.7 J/(mol*K)

N2_2 (g), S^\circ(at 25^\circC) = 191.56 J/(mol*K)

NH3_3 (g), S^\circ(at 25^\circC) = 192.77 J/(mol*K)

N2_2 (g) + 3 H2_2 (g) \leftrightharpoons 2 NH3_3 (g)

For the reaction above, calculate the change in free energy for the reaction, if it were to go to completion.

Calculate the standard free energy change, \triangleG^\circ, for the following reaction. Is the reaction spontaneous?

CH4_4 (g) + 2 O2_2 (g) \longrightarrow CO2_2 (g) + 2 H2_2O (l)

Values of standard molar entropy, Sf_{f}^\circ are as follows: CH4_4 (g), 186 J/(K*mol); O2_2 (g), 205 J/(K*mol); CO2_2 (g), 213.6 J/(K*mol); 2 H2_2O (l), 69.9 J/(K*mol)

\triangleH^\circ for this reaction is -890.3 kJ

What is the standard free energy change, \triangleG^\circ, for the following reaction at 298 K? Is the reaction spontaneous?

2 PCl3_3 (g) + O2_2 (g) \longrightarrow 2 POCl3_3, \triangleH = - 620.6 kJ/mol

Values of standard molar entropy, Sf_{f}^\circ are as follows: 2 PCl3_3 (g), 311.8 J/K; O2_2 (g), 205.1 J/K; POCl3_3, 222.4 J/K