A constant volume calorimeter was calibrated by carrying out a reaction known to release 0 90 kJ of heat in 0 60 L of solution in the calorimeter (q 0 90 kJ), resulting in a temperature rise of 2 85C In a subsequent experiment, 30 0 mL of 0 20 m HClO 2 (aq) and 30 0 mL of 0 20 m NaOH(aq) were mixed in the same calorimeter and the temperature rose by 1 31C What is the change in the internal energy of the reaction mixture as a result of the neutralization reaction

Question: A constant-volume calorimeter was calibrated by carrying out a reaction known to release 0.90 kJ of heat in 0.60 L of solution in the calorimeter

A constant-volume calorimeter was calibrated by carrying out a reaction known to release 0.90 kJ of heat in 0.60 L of solution in the calorimeter (q = –0.90 kJ), resulting in a temperature rise of 2.85°C. In a subsequent experiment, 30.0 mL of 0.20 m HClO₂(aq) and 30.0 mL of 0.20 m NaOH(aq) were mixed in the same calorimeter and the temperature rose by 1.31°C. What is the change in the internal energy of the reaction mixture as a result of the neutralization reaction?

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