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21 August, 18:18

A sample of 14.5 g of sodium bicarbonate (NaHCO3) was dissolved in 100 ml of water in a coffee-cup calorimeter with no lid by the following reaction

NaHCO3 (s) → Na + (aq) + HCO3 - (aq)

If the temperature of the water and the calorimeter (heat capacity of calorimeter = 150 J/oC) decreases from 25.00oC to 19.86oC, (1) what is the ΔH of the reaction?

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  1. 21 August, 18:46
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    The ΔH of the reaction is + 12.45 KJ/mol

    Explanation:

    Mass of water = 100ml = 100g. (You should always assume 1cm3 of water as 1g)

    heat capacity of water = 4.18 Jk-1 Mol-1

    Change in temperature = (19.86 - 25.00) = - 5.14 K (This is an endothermic reaction because of the fall in temperature)

    Molar mass of NaHCO3 = 84 g/mol

    Mole of NaHCO3 = 14.5 / 84 = 0.173 mol

    Step 1 : Calculate the heat energy (Q) lost by the water.

    Q = M x C x ΔT

    Q = - 100 x 4.18 x (-5.14)

    Q = 2148.5 joules

    Q = 2.1485 K J

    Step 2: Calculating the ΔH of the reaction?

    ΔH = Q / number of moles of NaHCO3

    ΔH = 2.1485 / 0.173

    ΔH = 12.42 KJ/mol
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