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7 April, 21:01

In a different experiment, the student uses a calorimeter which is perfectly insulated. She fills the calorimeter with 100.0 g of 25.00°C dilute HCl solution and adds 0.594 g Mg metal (24.3 g/mol). The final temperature of the apparatus comes to 41.83°C. Remember, the solution is made-up of the solute and the solvent. The specific heat for magnesium is negligible compared to the aqueous solution. What is the Molar Heat of Enthalpy for this reaction?

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  1. 7 April, 21:25
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    Mg + 2HCl = Mg Cl₂ + H₂

    .594 g =.594 / 24.3

    =.02444 mole

    Heat evolved = msΔ T, m is mass of water (solvant), s is specific heat of water, Δ T is rise in temperature

    = 100 x 4.2 x (41.83 - 25)

    = 7068.6 J

    .02444 mole of Mg evolves 7068.6 J of heat

    1 mole of Mg evolves 7068.6 /.02444 J

    = 289222.6 J

    = 289 kJ.

    Molar heat enthalpy = 289 kJ.
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