Formation of ICl(g) from it elements:
Natural element form of iodine → I2(s)
Natural element form of chlorine → Cl2(g)
In a formation equation, one mole of the product should be forming:
Formation equation of ICl(g): ½ I2(s) + ½ Cl2(g) → ICl(g)
Manipulate reaction such that when you add them you arrive to the formation equation of ICl(g):
Using the following data, calculate the standard heat of formation of ICl(g) in kJ/mol:
Cl2 (g) → 2Cl (g) ΔH° = 242.3 kJ
I2 (g) → 2I (g) ΔH° = 151.0 kJ
ICl (g) → I (g) + Cl (g) ΔH° = 211.3 kJ
I2 (s) → I2 (g) ΔH° = 62.8 kJ
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