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9 September, 03:34

During an experiment, a student adds 1.23 g of cao to 200.0 ml of 0.500 m hcl. the student observes a temperature increase of 5.10 °c. assuming the solution/'s final volume is 200.0 ml, the density if 1.00 g/ml, and the heat capacity is 4.184 j / (g·°c, calculate the heat of the reaction,? hrxn.

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  1. 9 September, 07:18
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    Given:

    Mass of CaO = 1.23 grams

    Volume of HCl = 200 mL

    Concentration of HCl = 0.500 M

    Termperature increase = 5.10 degrees celcius

    Final volume = 200 mL

    Density of sol'n = 1 g/mL

    Cp = 4.184 J/gC

    Balanced Equation:

    CaO + 2HCl - - - > CaCl2 + H2O

    Mass of HCl = 200 mL/1000 * 0.5 mol/L * 36.46 g/mol

    = 3.646 grams

    Mass solution = 200mL * 1 g/mL = 200 grams

    H = mCpdT

    = 200 grams * 4.184 J/gC * 5.10 C

    H = 4267.68 Joules
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