Answer:
–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.
