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7 June, 11:04

If 8.00 g ammonium nitrate is dissolved in 1.0 l water, the water decreases in temperature from 21.0 °c to 20.39 °c. determine the molar heat of solution (in kj/mol) of the ammonium nitrate. the density of water is 1.0 g/ml and assume that the resulting solution has the same specific heat as water (4.184 j/goc).

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  1. 7 June, 14:33
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    When Heat of solution ΔH solution = m. C.ΔT

    when m is the mass of solution = mass of water + mass of ammonium nitrate

    mass of water = Volume * density = 1L * 1000 g/L = 1000 g

    by substitution:

    m of solution = 1000 g + 8 g = 1008 g

    ΔT = 21°C - 20.39 °C = 0.61°C

    C = 4.184 J / g. C°

    by substitution in ΔH formula:

    ΔH = 1008 * 4.184 * 0.61 = 2572.7 J / 1000 = 2.57KJ

    ∴ molar heat of solution = heat of solution / no of mol of solute

    no of moles of solute (NH4NO3) = weight / molecular weight = 8g / 80 g/mol

    = 0.1 mol

    ∴molar heat of solution = 2.57KJ / 0.1 mol

    = 25.7 KJ/mol
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