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
What is the pH of a 1.0 L buffer made with 0.300 mol of HF (Ka = 6.8 × 10⁻⁴) and 0.200 mol of NaF to which 0.160 mol of NaOH were added?
Can I please get help with this.
Determine if the following salt is neutral, acidic or basic. If acidic or basic, write the appropriate equilibrium equation for the acid or base that exists when the salt is dissolved in aqueous solution. If neutral, simply write only NR. Be sure to include the proper phases for all species within the reaction. N₂H₅ClO₄
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Calorimetry Concept, Examples and Thermochemistry | How to Pass Chemistry; Author: Melissa Maribel;https://www.youtube.com/watch?v=nSh29lUGj00;License: Standard YouTube License, CC-BY