Assuming that the specific heat of the solution is 4.18 j/(g⋅∘c), that its density is 1.00 g/ml, and that the calorimeter itself absorbs a negligible amount of heat, calculate δh in kilojoules for the reaction. h2so4(aq)+2naoh→2h2o(l)+na2so4(aq)

Q= mcâ†T Q = energy (heat) generated or absorbed m = mass of the substance undergoing the change in temperature c = specific heat of the substance undergoing the change in temperature â†T = T(final) - T(initial) We are given: m = (25.0 mL + 50.0 mL)*(1.00 g/mL) = 75.0 g c = 4.18 J g^-1 °C^-1 â†T = 33.9 °C - 25.0 °C = 8.9 °C Now we just plug those numbers in: Q= mcâ†T Q = (75.0 g)*(4.18 J g^-1 °C^-1)*(8.9 °C) Q = 2790.15 J = 2.79 kJ (to three sig figs)

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The answer for this is a