A 105.2 mL sample of 1.00 M NaOH is mixed with 52.6 mL of 1.00 M H2SO4 in a larg

Question

A 105.2 mL sample of 1.00 M NaOH is mixed with 52.6 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 21.65 °C. After adding the NaOH solution to the coffee cup and stirring the mixed solutions with the thermometer, the maximum temperature measured is 32.30 °C, Assume that the density of the mixed solutions is 1.00 g/mL, that the specific heat of the mixed solutions is 4.18J/gC), and that no heat is lost to the surroundings. 1st attempt Part 1 (1 point) Inl See Periodic Table 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 (1 point) Is any NaOH or H2SO4 left in the Styrofoam cup when the reaction is over? Choose one O A. Yes B. No Part 3 (1 point) ? See Hint Calculate the enthalpy change per mole of H2SO4 in the reaction. kJ/mol

Explanation / Answer

2NaOH(aq) + H2SO4(aq) ----> Na2SO4(aq) + 2H2O(l)

   2 mol NaOH = 1 mol H2SO4

Part 2

no of mol of naOH = 105.2*1/1000 = 0.1052 mol

no of mol of H2SO4 = 52.6*1/1000 = 0.0526 mol

answer: B.NO

part 3

heat released(q) = m*s*DT

                 = (105.2+52.6)*4.18*(32.3-21.65)

                 = 7.0 kj

DHrxn = -q/n = - 7/0.0526 = -133.08 kj/mol

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