What is ΔH if 5.5 grams H₂O(l) is formed from this reaction? ( molar mass of H₂O = 18) H₂(g) + ½ O₂(g) → H₂O(l) ∆H = -285.8 kJ

–87.3 KJ.

Explanation:

The equation for the reaction is given below:

H₂(g) + ½O₂(g) —> H₂O(l) ∆H = -285.8 kJ

Next, we shall determine the mass of H₂O produced from the balanced equation. This can be obtained as follow:

Molar mass of H₂O = 18 g/mol

Mass of H₂O from the balanced equation = 1 × 18 = 18 g

SUMMARY:

From the balanced equation above,

When 18 g of H₂O was produced, ∆H was –285.8 KJ.

Finally, we shall determine ∆H when 5.5 g of H₂O is produced. This can be obtained as illustrated below:

From the balanced equation above,

When 18 g of H₂O was produced, ∆H was –285.8 KJ.

Therefore, 5.5 g of H₂O will produce ∆H of = (5.5 × –285.8) / 18 = –87.3 KJ

Thus, the ∆H when 5.5 g of H₂O was produced is –87.3 KJ.

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