Calculate ΔHHydrogenation of ethyne in Kcal/molC2H2 + 2H2 → C2H6If ΔHcomb(C2H2) = – 100 KcalΔHcomb(H2) = – 900 KcalΔHcomb(C2H6) = – 250 Kcal–500 Kcal–1250 Kcal–1650 Kcal–750 Kcal
Question
Calculate ΔHHydrogenation of ethyne in Kcal/molC2H2 + 2H2 → C2H6If ΔHcomb(C2H2) = – 100 KcalΔHcomb(H2) = – 900 KcalΔHcomb(C2H6) = – 250 Kcal–500 Kcal–1250 Kcal–1650 Kcal–750 Kcal
Solution
To calculate ΔHHydrogenation of ethyne, we need to use the given values of ΔHcomb(C2H2), ΔHcomb(H2), and ΔHcomb(C2H6).
The balanced chemical equation for the hydrogenation of ethyne is: C2H2 + 2H2 → C2H6
From the equation, we can see that 1 mole of C2H2 reacts with 2 moles of H2 to form 1 mole of C2H6.
Now, let's calculate the ΔHHydrogenation using the given values:
ΔHHydrogenation = ΔHcomb(C2H6) - (ΔHcomb(C2H2) + 2 * ΔHcomb(H2))
Substituting the given values: ΔHHydrogenation = -250 Kcal - (-100 Kcal + 2 * -900 Kcal)
Simplifying the equation: ΔHHydrogenation = -250 Kcal - (-100 Kcal - 1800 Kcal) ΔHHydrogenation = -250 Kcal + 100 Kcal + 1800 Kcal ΔHHydrogenation = 1650 Kcal
Therefore, the ΔHHydrogenation of ethyne is 1650 Kcal.
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