Suppose 25.0 mL of 0.500 M H,S0, is added to 50.0 mL of a 0.500 M KOH in a coffe

Question

Suppose 25.0 mL of 0.500 M H,S0, is added to 50.0 mL of a 0.500 M KOH in a coffee-cup calorimeter. The solution temperature, originally at 23.50°C, rises to 30.17 Assume the totalvolume is the s solution has a density of 1.00 g/ml and a specific heat of 4.18 J/gc.5cex A. Write a balanced equation for the reaction. 3. um ofthe individual volumes and the final 8. Use the density and volume of the solution to find the mass of the solution then calculate the heat released by the reaction. C. How much heat is transferred per mole of KOH?

Explanation / Answer

moles of acid H2SO4 = 25 x 0.50 / 1000 = 0.0125

moles of KOH = 25 x 0.5 / 1000 = 0.0125

balanced equation:

H2SO4     + 2 KOH ------------------------> K2SO4 + 2H2O

b)

total volume = 25+20 = 50 mL

mass of solution = volume x density

                          = 50 x 1

                         = 50 g

dT = 30.17 -23.50 = 6.67 oC

Q = 50 x 4.18 x 6.67

Q = 1394 J

heat released by the solution = 1394J = 1.394 kJ

c)

heat released per mole of KOH = - Q / n

                                                    = -1.394 / 0.0125

                                                   = - 112 kJ / mol

Related Questions

Navigate

• Browse (All)
• Browse S
• Subjects

---

---

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