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29 November, 18:53

Two solutions, initially at 24.60°C, are mixed in a coffee cup calorimeter. When a 100.0 mL volume of 0.100 M AgNO3 solution is mixed with a 100.0 mL sample of 0.200 M NaCl solution, the temperature in the calorimeter rises to 25.30°C. Determine the △ H°rxn in units of kJ/mol AgCl. Assume that the density and heat capacity of the solutions is the same as that of water. The specific heat capacity of water = 4.18 J/g°C.

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  1. 29 November, 19:20
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    58520kJ / mol

    Explanation:

    It is possible to obtain the heat produced in a reaction in a coffe cup calorimeter using the formula:

    q = - C*m*ΔT

    Where q is heat, C is specific heat capacity (4.18 J/g°C), m is mass of the solution (200,0 mL = 200,0g), and ΔT is change in temperature (25.30°C - 24.60°C = 0.70°C)

    Replacing:

    q = - 4.18J/g°C*200.0g*0.70°C

    q = - 585.2J

    In the reaction:

    AgNO₃ (aq) + NaCl (aq) → AgCl (s) + NaNO₃ (aq)

    Moles that react are:

    0.1000L ₓ (0.100mol / L) = 0.0100 moles

    The ΔH°rxn is defined as the heat released or consumed per mole of reaction. That is:

    ΔH°rxn = - 585.2J / 0.01mol = 58520kJ / mol
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