The Haber process for ammonia synthesis is exothermic: N2(g) + 3H2(g) ⇌ 2NH3(g); ΔH° = -92 kJ If the equilibrium constant Kc for this process at 500.°C is 6.0 × 10-2, what is its value at 300.°C?
The Haber process for ammonia synthesis is exothermic: N2(g) + 3H2(g) ⇌ 2NH3(g); ΔH° = -92 kJ If the equilibrium constant Kc for this process at 500.°C is 6.0 × 10-2, what is its value at 300.°C?
Chemistry by OpenStax (2015-05-04)
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Chapter13: Fundamental Equilibrium Concepts
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The Haber process for ammonia synthesis is exothermic:
N2(g) + 3H2(g) ⇌ 2NH3(g); ΔH° = -92 kJ
If the equilibrium constant Kc for this process at 500.°C is 6.0 × 10-2, what is its value at 300.°C?
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