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A

Anonymous

Feb 07, 2025

Hess’ Law Question, Calculating Enthalpy Change?

I have a question regarding Hess's Law and calculating enthalpy change.

I need to calculate the standard enthalpy change for the following reaction:

2 HCl (g) + F2 (g) → 2 HF (l) + Cl2 (g)

Given the following reactions:

1) 4 HCl (g) + O2 (g) → 2 H2O (l) + 2 Cl2 (g), ΔH = -202.4 kJ/mol 2) (1/2) H2 (g) + (1/2) F2 (g) → HF (l), ΔH = -600 kJ/mol 3) H2 (g) + (1/2) O2 (g) → H2O (l), ΔH = -285.8 kJ/mol

To approach this, I multiplied the first reaction by 1/2 and the second reaction by 2. This gives me the following equations:

2 HCl (g) + (1/2) O2 (g) → H2O (l) + Cl2 (g), ΔH = -101.2 kJ/mol H2 (g) + F2 (g) → 2 HF (l), ΔH = -1200 kJ/mol H2 (g) + (1/2) O2 (g) → H2O (l), ΔH = -285.8 kJ/mol

After calculating, I arrived at an answer of -1587 kJ/mol for the reaction, but it seems to be incorrect.

Could someone help me identify my mistake and guide me on how to correct it? Thank you!

3 Answers

M
Marco Littel

Feb 21, 2025

you end up subtracting the last line of reactions because if you add that, your result ends up having H2, O2, and H2O

so your answer should be -1015.4 kJ/mol

A
Anonymous

Nov 09, 2024

I thing in equation 3 you need to divide the answer to 1/2?

A
Anonymous

Feb 12, 2025

I don't see your F2(g) canceling out, maybe thats why? Idk I only got a 75% on this unit last week so I could be wrong

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