🤓 Based on our data, we think this question is relevant for Professor Dixon's class at UCF.
Combine the reactions and take the sum of the ΔH applying Hess' Law
Hg(l) + Cl2(g) ⟶ HgCl2(s) ΔH = −224 kJ (reverse)
HgCl2(s) ⟶ Hg(l) + Cl2(g) ΔH = +224 kJ
Hg(l) + HgCl2(s) ⟶ Hg2Cl2(s) ΔH = −41.2 kJ (reverse)
Hg2Cl2(s) ⟶ Hg(l) + HgCl2(s) ΔH = +41.2 kJ
Combining the equations:
Calculate ΔH for the process Hg 2Cl2(s) ⟶ 2Hg(l) + Cl2(g) from the following information:
Hg(l) + Cl2(g) ⟶ HgCl2(s) ΔH = −224 kJ
Hg(l) + HgCl2(s) ⟶ Hg2Cl2(s) ΔH = −41.2 kJ
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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.
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Based on our data, we think this problem is relevant for Professor Dixon's class at UCF.
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Our data indicates that this problem or a close variation was asked in Chemistry - OpenStax 2015th Edition. You can also practice Chemistry - OpenStax 2015th Edition practice problems.