09 Question (3 points) B See page 393 A 92.2 ml sample of 1.00 M NaOH is mixed w

Question

09 Question (3 points) B See page 393 A 92.2 ml sample of 1.00 M NaOH is mixed with 46.1 mL of 1.00 M passes a calibrated thermometer. The temperature of each solution before mixing is 22.05 °C. After adding the NaOH solution to the coffee cup and stirring the mixed solutions with the thermometer, the maximum temperature measured is 31.10°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. H2SO, in a large Styrofoam coffee cup: the cup is fitted with a lid through which 3rd attempt Part 1 (1 point) 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. 9 OF 13 QUESTIONS COMPLETED 09:13 > VIEW SOLUTION XPS

Explanation / Answer

moles of acid H2SO4 = 92.2 x 1 / 1000 = 0.0922

moles of NaOH = 46.1 x 1.0 / 1000 = 0.0461

H2SO4     + 2 NaOH ------------------------> Na2SO4 + 2H2O

1                2

0.0461      0.0922                                                       0.0922

here both are consumed

moles of water fomred = 0.0922

total volume = 92.2 + 46.1 = 138.3 mL

mass of solution = volume x density

                          = 138.3 x 1

                         =138.3 g

dT = 31.10 -22.05 = 9.05 oC

Q = 138.3 x 4.184 x 9.05

Q = 5237 J

change in enthalpy per mole H2SO4 = - Q / n

                                                      = -5.237 / 0.0922

                                                  = - 56.8 kJ / mol

Related Questions

Navigate

• Browse (All)
• Browse
• Subjects

---

---

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