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29 June, 08:13

2.00 L of 0.500 M H2SO4 (density = 1.030 g/mL) at 25.000°C is mixed with 200. g of a NaOH solution, also at 25.000°C. After stirring, the temperature of the solution is 36.820°C. Calculate q for the reaction. (Assume the specific heat capacity of each solution is 4.184 J/g °C.) Is the reaction exothermic or endothermic?

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  1. 29 June, 12:06
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    Q = 111.8 kJ;

    The reaction is endothermic.

    Explanation:

    The heat of the mixture can be calculated by the equation:

    Q = m*c*ΔT

    Where Q is the heat, m is the mass of the solution, c is the specific heat, and ΔT is the variation in the temperature (fina - initial).

    The mass of H₂SO₄ is the volume multiplied by its density:

    mH₂SO₄ = 2000 mL * 1.030 g/mL = 2060 g

    Then the total mass is:

    m = 2060 + 200

    m = 2260 g

    Q = 2260*4.184 * (36.820 - 25.000)

    Q = 111,468.03 J

    Q = 111.8 kJ

    The reaction is endothermic because the solution is absorbing heat (Q > 0), which can be noticed by the increase in the temperature. When the reaction loses heat, it is exothermic and the temperature decreases.
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