Question

A 96.2 mL sample of 1.00 M NaOH is mixed with 48.1 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 22.25 °C. After adding the NaOH solution to the coffee cup and stirring the mixed solutions with the thermometer, the maximum temperature measured is 30.90 °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.

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.

2.Is any NaOH or H₂SO₄ left in the Styrofoam cup when the reaction is over? (Y or N)

3. Calculate the enthalpy change per mole of H₂SO₄ in the reaction. (kJ/mol)

Answer 1