One of the common oxidizing agents in explosives, fireworks, and match heads, undergoes a solid-state redox reaction when heated. In this reaction, note that the oxidation number of Cl in the reactant is higher in one of the products and lower in the other (disproportionation): 4KClO3(s) = 3KClO4(s) + KCl(s) Use △H o and So values to calculate △G o at 25 oC. Hint: Determine the thermodynamic entities from literature; place them into Gibbs free energy equation and solve.
1. Problem: Potassium chlorate
One of the common oxidizing agents in explosives,
fireworks, and match heads, undergoes a solid-state redox
reaction when heated. In this reaction, note that the
oxidation number of Cl in the reactant is higher in one of the
products and lower in the other (disproportionation):
4KClO3(s) = 3KClO4(s) + KCl(s)
Use △H o and So values to calculate △G o at 25 oC.
Hint: Determine the
place them into Gibbs free energy equation and solve.
2. Problem:
At 298 K, the formation of ammonia has a negative △S0
sys
H2(g) + 3H2(g) = 2NH3(g) △S 0
sys= -197 J/K
Calculate △S o and state whether the reaction
occurs spontaneously at this temperature.
Hint: △S o of the reaction must be p
3. How to use state functions to estimate the
thermodynamic status of a system?
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