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

Question

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

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RobertKer 4 years 2021-07-17T20:00:43+00:00 1 Answers 11 views 0

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  1. thienan
    0
    2021-07-17T20:02:24+00:00
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    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.

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