200.0 mL of 0.200 M HNO3 is added to 200.0 mL of 0.200 M KOH in a coffee cup calorimeter. The neutralization reaction that occurs can be described by the chemical equation- HNO3(aq) + KOH(aq) → KNO3(aq) + H₂O(l) Before the solutions are mixed they are both at 23.00 °C. After the mixing of the solutions the temperature increases until it remains constant at 24.39 °C. Assuming no heat lost to the surroundings, how much heat was lost in this reaction?

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200.0 mL of 0.200 M HNO3 is added to 200.0 mL of 0.200 M KOH in a coffee cup calorimeter. The neutralization reaction that occurs can be described by the chemical equation- HNO3(aq) + KOH(aq) → KNO3(aq) + H₂O(l) Before the solutions are mixed they are both at 23.00 °C. After the mixing of the solutions the temperature increases until it remains constant at 24.39 °C. Assuming no heat lost to the surroundings, how much heat was lost in this reaction? (Assume the specific heats and densities of the solutions is the same as water.)
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