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Thermochemistry Problem

  1. Feb 22, 2009 #1
    1. The problem statement, all variables and given/known data

    When 0.612 g of Ca metal is added to 200.0 mL of 0.500 M HCl(aq), a temperature increase of 100C is observed.
    Assume the solution's final volume is 200.0 mL, the density is 1.00 g/mL, and the heat capacity is 4.184 J/gC.
    (Note: Pay attention to significant figures. Do not round until the final answer.)
    The molar heat of reaction, H rxn, for the reaction of

    Ca(s) + 2H+(aq) => Ca2+(aq) + H2 (g)

    2. Relevant equations

    Q=mc[tex]\Delta[/tex]T

    3. The attempt at a solution

    All I know is that mc[tex]\Delta[/tex]T is used... Our professor hasn't taught us how to do this yet so that's about all I know. Would I divide Q by the number of moles formed?
     
  2. jcsd
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