12 Question (12 points) aSee page 236 A 110.2 mL sample of 1.00 M NaOH is mixed

Question

12 Question (12 points) aSee page 236 A 110.2 mL sample of 1.00 M NaOH is mixed with 55.1 mL of 1.00 MH2SO4 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 30.70 °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. 1st attempt Part 1 (4 points) i 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. 12:15 > 10 OF 15 QUESTIONS COMPLETED SUBMIT ANSWER ere to search

Explanation / Answer

part1)

The balanced equation is

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

Part 2)

NO

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

110.2x1.0 55.1 x 1.0 0 0 initial mmoles

110.2-55.1x2=0 55.1-55.1=0 110 - after reaction

Thus both acid ad base are completely consumed.

Part 3)

The heat liberatd in the process = mass of solution x specific heat of water x rise in temperature

= (110.2+55.1) g x 4.18J/g x (30.7-23.05)

=5285.80J

The m moles of H2SO4 used = 55.1 x1.0M

= 55.1 x10-3 mol

  55.1 x10-3 mol gives 5285.80 J heat

Thus for 1 mole of H2SO4 the heat liberated = 1 mol x 5285.80 J /  55.1 x10-3 mol

=95.931 kJ

Thus the enthalpy change for one moles of H2SO4 = 95.931 kJ/mol

Part 2)

No.

Related Questions

Navigate

• Browse (All)
• Browse 1
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.