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A 97.2 mL sample of 1.00 M NaOH is mixed with 48.6 mL of 1.00 M...

A 97.2 mL sample of 1.00 M NaOH is mixed with 48.6 mL of 1.00 M H2SO4 in a large Styrofoam coffee cup; the cup is fitted with a lid through which passes a calibrated thermometer. The temperature of each solution before mixing is 23.05 °C. After adding the NaOH solution to the coffee cup and stirring the mixed solutions with the thermometer, the maximum temperature measured is 32.50 °C. Assume that the density of the mixed solutions is 1.00 g/mL, that the specific heat of the mixed solutions is 4.18 J/(g·°C), and that no heat is lost to the surroundings.

Part 1

Write a balanced chemical equation for the reaction that takes place in the Styrofoam cup. Remember to include phases in the balanced chemical equation.

Part 2

Calculate the enthalpy change per mole of H2SO4 in the reaction.

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