Value of free energy for standard state Δ G ° for following reaction is to be calculated. The reaction is spontaneous at 25 ° C should be shown. Also, the reason and temperature at which reaction becomes nonspontaneous should be determined. 2 H 2 S ( g ) + SO 2 ( g ) → 2 S ( s ) + 2 H 2 O ( g ) Concept introduction: Standard free-energy of substance formation use to define free-energy change to form 1 mol of substance in standard state. The reactant must be in its maximum stable form of constituent elements. It is denoted by Δ G ° f . The general expression for Δ G ° f is as follows: Δ G ° = Δ G ° f ( product ) − Δ G ° f ( reactant ) For example, formation reaction of ammonia is as follows: N 2 ( g ) + 3 H 2 ( g ) → 2 NH 3 ( g ) Standard free-energy change of 2 mol of ammonia is − 33.0 kJ , thus free-energy change of formation of 1 mol NH 3 is equal to − 16.5 kJ .
Value of free energy for standard state Δ G ° for following reaction is to be calculated. The reaction is spontaneous at 25 ° C should be shown. Also, the reason and temperature at which reaction becomes nonspontaneous should be determined. 2 H 2 S ( g ) + SO 2 ( g ) → 2 S ( s ) + 2 H 2 O ( g ) Concept introduction: Standard free-energy of substance formation use to define free-energy change to form 1 mol of substance in standard state. The reactant must be in its maximum stable form of constituent elements. It is denoted by Δ G ° f . The general expression for Δ G ° f is as follows: Δ G ° = Δ G ° f ( product ) − Δ G ° f ( reactant ) For example, formation reaction of ammonia is as follows: N 2 ( g ) + 3 H 2 ( g ) → 2 NH 3 ( g ) Standard free-energy change of 2 mol of ammonia is − 33.0 kJ , thus free-energy change of formation of 1 mol NH 3 is equal to − 16.5 kJ .
Solution Summary: The author explains the value of free energy for standard state Delta G° and the reason and temperature at which reaction becomes nonspontaneous.
Value of free energy for standard state ΔG° for following reaction is to be calculated. The reaction is spontaneous at 25°C should be shown. Also, the reason and temperature at which reaction becomes nonspontaneous should be determined.
2H2S(g)+SO2(g)→2S(s)+2H2O(g)
Concept introduction:
Standard free-energy of substance formation use to define free-energy change to form 1mol of substance in standard state. The reactant must be in its maximum stable form of constituent elements. It is denoted by ΔG°f. The general expression for ΔG°f is as follows:
ΔG°=ΔG°f(product)−ΔG°f(reactant)
For example, formation reaction of ammonia is as follows:
N2(g)+3H2(g)→2NH3(g)
Standard free-energy change of 2 mol of ammonia is −33.0 kJ, thus free-energy change of formation of 1 mol
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