# Problem: Using the following data, calculate the standard heat of formation of ICl(g) in kJ/mol:Cl2 (g) → 2Cl (g)          ΔH° = 242.3 kJI2 (g) → 2I (g)               ΔH° = 151.0 kJICl (g) → I (g) + Cl (g)    ΔH° = 211.3 kJI2 (s) → I2 (g)               ΔH° = 62.8 kJ

###### FREE Expert Solution

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):

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###### Problem Details

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

I(s) → I2 (g)               ΔH° = 62.8 kJ

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Hess's Law concept. You can view video lessons to learn Hess's Law. Or if you need more Hess's Law practice, you can also practice Hess's Law practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Davis' class at UCF.

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.