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16 March, 14:21

In a coffee-cup calorimeter, 50.0ml of 0.100M AgNO3 and50.0ml of 0.100M HCl are mixed to yield the following reaction:

Ag + (aq) + Cl - (ag) >AgCl (s)

The two solutions were initially at 22.60oC, and the final temperature is 23.40oC. Calculate the heat that accompanies this reaction in KJ/mol of AgCl formed. Assume that the combined solution has a mass of 100.0 g and a specific heat capacity of 4.18 J/oC. g.

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  1. 16 March, 18:17
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    -66.88KJ/mol

    Explanation:

    It is possible to obtain the heat involved in a reaction using a calorimeter. Formula is:

    q = - C*m*ΔT

    Where q is heat of reaction, C is specific heat capacity (4.18J/°Cg), m is mass of solution (100.0g) and ΔT is temperature change (23.40°C-22.60°C = 0.80°C)

    Replacing:

    q = - 4.18J/°Cg*100.0g*0.80°C

    q = - 334.4J

    Now, in the reaction:

    Ag⁺ + Cl⁻→ AgCl

    AgNO₃ as source of Ag⁺ and HCl as source of Cl⁻

    Moles that react are:

    0.050L * (0.100mol / L) = 0.0050moles

    If 0.0050 moles produce - 334.4J. Heat of reaction is:

    -334.4J / 0.0050moles = - 66880J/mol = - 66.88KJ/mol
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