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8 June, 10:41

The addition of 3.72 g of Ba (OH) 2 · 8 H2O to a solution of 1.26 g of NH4SCN in 133 g of water in a calorimeter caused the temperature to fall by 4.3°C. Assuming the specific heat of the solution and products is 4.20 J/g·°C, calculate the approximate amount of heat (in J) absorbed by the reaction, which can be represented by the following equation. Ba (OH) 2 · 8 H2O (s) + 2 NH4SCN (aq) → Ba (SCN) 2 (aq) + 2 NH3 (aq) + 10 H2O (l)

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  1. 8 June, 11:09
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    The amount of heat absorbed by the reaction is 2491.92 J

    Explanation:

    Step 1: The balanced equation

    Ba (OH) 2 · 8 H2O (s) + 2 NH4SCN (aq) → Ba (SCN) 2 (aq) + 2 NH3 (aq) + 10 H2O (l)

    Step 2: Data given

    mass of Ba (OH) 2 · 8 H2O (s) = 3.72g

    Molar mass of Ba (OH) 2 · 8 H2O (s) = 315.46 g/mol

    mass of NH4SCN = 1.26 g

    Molar mass of NH4SCN = 76.122 g/mol

    mass of water = 133g

    Molar mass of water = 18.02 g/mol

    Temperature decreases with 4.3 °C this is an endothermic reaction

    specific heat of the solution and products is 4.20 J/g·°C

    Step 3: Calculate heat transfer

    Q = m*c*ΔT

    with m = the mass = mass of Ba (OH) 2 · 8 H2O + mass of NH4SCN + mass of water = 3.72 + 1.26 + 133 = 137.98

    with c = the specific heat capacity of the solution = 4.20 J/g°C

    with ΔT = The change in temperature = 4.3 °C

    Q = 137.98 * 4.20 * 4.3 = 2491.92 J

    The amount of heat absorbed by the reaction is 2491.92 J
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