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25 August, 10:15

When 10. g of CH3COOH is combusted in a sealed calorimeter, it releases enough energy to heat 2000. g of water from 23.5 °C to 34.3 °C. a. Calculate the energy released per 10 g of CH3COOH. b. Calculate the energy released per mole of CH3COOH.

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  1. 25 August, 10:20
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    a. 90.288 kJ.

    b. - 54.06 kJ/mol.

    Explanation:

    a. Calculate the energy released per 10 g of CH₃COOH.

    We can calculate the amount of heat (Q) released to water using the relation:

    Q = m. c.ΔT,

    where, Q is the amount of heat released to water (Q = ? J).

    m is the mass of water (m = 2000.0 g).

    c is the specific heat capacity of solution (c = 4.18 J/g.°C).

    ΔT is the difference in T (ΔT = final temperature - initial temperature = 34.3°C - 23.5°C = 10.8°C).

    ∴ Q = m. c.ΔT = (2000.0 g) (4.18 J/g.°C) (10.8°C) = 90288 J = 90.288 kJ.

    b. Calculate the energy released per mole of CH₃COOH.

    To find ΔH:

    ∵ ΔH = Q/n

    no. of moles of CH₃COOH (n) = mass/atomic mass = (10.0 g) / ((60.052 g/mol) = 0.167 mol.

    ∴ ΔH = - Q/n = - (90.288 kJ) / (0.167 mol) = - 54.06 kJ/mol.

    The negative sign is not from calculation, but it is an indication that the reaction is exothermic.
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