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19 September, 16:34

A 0.250-g chunk of sodium metal is cautiously dropped into a mixture of 50.0 g of water and 50.0 g of ice, both at 08C. The reaction is 2Na (s) 1 2H2O (l) 88n 2NaOH (aq) 1 H2 (g) DH 5 2368 kJ

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  1. 19 September, 19:22
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    The ice will not melt

    Explanation:

    Given:

    Mass of chunk = 0.25 g

    moles of sodium = mass / molar mass = 0.25 / 23 = 0.010 g

    ΔH = - 368 KJ

    Hence, 2 moles of Na produced 368 KJ

    So 1 mole will produce 368 / 2 KJ and 0.01 mole will produce

    = (368 / 2) * 0.01 = 2.0056 KJ

    Also, moles of ice = mass / molar mass of water = 50 / 18 = 2.8 g

    Energy required to melt the ice = enthalpy of fusion of ice * number of moles of ice

    = 6.01 * 2.8 = 16.722 KJ

    But we have 2.0056 KJ, so the ice will not melt.
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