Consider the reaction described by the following chemical equation. 2 HN3(1) + 2 NO(g) — H2O2(1) + 4 N, (g) What is the enthalpy

Question

Consider the reaction described by the following chemical equation.
2 HN3(1) + 2 NO(g) — H2O2(1) + 4 N, (g)
What is the enthalpy change associated with the production of 1 mol of H, O, if a reaction that produces
2.50 g of H, O, releases 65.9 kJ of heat?

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Diễm Kiều 3 years 2021-08-30T13:38:15+00:00 1 Answers 8 views 0

Answers ( )

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    2021-08-30T13:39:26+00:00

    Answer:

    Q = -897 kJ/mol

    Explanation:

    From the given information:

    The heat released Q = -65.9 kJ

    To start with the molar mass of H_2O_2 = 2 × (molar mass of H) + 2 × (molar mass of O)

    = (2 × 1.008) + (2 × 16.0 )

    = 34.016 g/mol

    However, given that:

    mass of H_2O_2  2.50 g

    The number of moles of H_2O_2  = \dfrac{mass}{molar \ mass}

    = \dfrac{2.5}{34.016}

    = 7.349 \times 10^{-2} \ mol

    Finally; Using the formula:

    \Delta H = \dfrac{Q}{number \ of \ moles}\\ \\ Q = \dfrac{-65.9 \ kJ}{7.349 \times 10^{-2} \ mol}

    Q = -897 kJ/mol

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Giải phương trình 1 ẩn: x + 2 - 2(x + 1) = -x . Hỏi x = ? ( )