Standard enthalpy of formation?
Given the following reactions and their standard enthalpy changes:
- H2 (g) + F2 (g) → 2HF (g) ΔH°rxn = -546.6 kJ
- 2H2 (g) + O2 (g) → 2H2O (l) ΔH°rxn = -571.6 kJ
Calculate the standard enthalpy change (ΔH°rxn) for the following reaction:
2F2 (g) + 2H2O (l) → 4HF (g) + O2 (g)
What is the value of ΔH°rxn?
1 Answers
Hi firefighter,
I am french (Boulogne sur mer 62200 – FRANCE)
. 2 x (. . F2 (g) + H2 (g) —> 2HF (g) . . . . . . . . . . . . . . . .ΔH°rxn = – 546.6 kJ
. . . . . . . . . . . .2H2O (l) —> 2H2 (g) + O2 (g) . . . . . . . . .ΔH°rxn = + 571.6 kJ
– – – – – – – – – – – – – – – – – – – – – – – – – – – – – – – – – – – – – – – – – – – – – – – – – – – – – – –
. . . .2F2 (g) + 2H2O (l) —> 4HF (g) + O2 (g) . . . . . . . . ΔH°rxn = ??
ΔH°rxn = 2 x ΔH°rxn(reaction 1) + ΔH°rxn(reaction 2)
ΔH°rxn = 2 x (- 546,6) + 571,6
ΔH°rxn = – 521,6 kJ
I hope to have answered your question.
.
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