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Given the following equations, determine the standard enthalpy of formation (ΔHf∘) for one mole of ICl3(g). I2(g) + 3 Cl2(g) ⟶ 2 ICl3(g) ΔH298∘ = −214 kJ I2(s) ⟶ I2(g) ΔH298∘ = 38 kJ Note that iodine (I2) is a solid at standard conditions. Your answer should have two significant figures. Provide your answer below: kJ

Given the following equations, determine the standard enthalpy of formation (ΔHf∘) for one mole of ICl3(g). I2(g) + 3 Cl2(g) ⟶ 2 ICl3(g) ΔH298∘ = −214 kJ I2(s) ⟶ I2(g) ΔH298∘ = 38 kJ Note that iodine (I2) is a solid at standard conditions. Your answer should have two significant figures. Provide your answer below: kJ

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Given the following equations, determine the standard enthalpy of formation ( Δ H f ∘ ) for one mole of I C l 3 ( g ) .
I 2 ( g ) + 3 C l 2 ( g ) ⟶ 2 I C l 3 ( g ) Δ H 298 ∘ = − 214 k J I 2 ( s ) ⟶ I 2 ( g ) Δ H 298 ∘ = 38 k J
Note that iodine ( I 2 ) is a solid at standard conditions.
  • Your answer should have two significant figures.
Provide your answer below: ◻ k J

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