home / study / science / chemistry / chemistry questions and answers / when 33.5

Question

home / study / science / chemistry / chemistry questions and answers / when 33.5 ml of 0.520 m h2so4 is added to 33.5 ml of 1.04 m koh in a coffee-cup calorimeter ... Question: When 33.5 mL of 0.520 M H2SO4 is added to 33.5 mL of 1.04 M KOH in a coffee-cup calorimeter at 23... When 33.5 mL of 0.520 M H2SO4 is added to 33.5 mL of 1.04 M KOH in a coffee-cup calorimeter at 23.50°C, the temperature rises to 30.17°C. Calculate H of this reaction per mole of H2SO4 and KOH reacted. (Assume that the total volume is the sum of the individual volumes and that the density and specific heat capacity of the solution are the same as for pure water: d = 1.00 g/mL and c = 4.184 J/g×K.)

_____ kJ/mol

_____ kJ/mol

Explanation / Answer

mmol of H2SO4 =MV = 33.5*0.52 = 17.42

mmol of KOH = MV = 33.5*1.04 = 34.84

now..

Qsolution = m*C*(Tf-Ti)

m = V1+V2 = 33.5+33.5 = 67 mL = 67 g

Q = (67)(4.184)(30.17-23.50) = 1869.78 J

now...

HRxn = -Qrxn/n

for H2SO4)

HRxn = -Qrxn/n = -1869.78 / (17.42) = -107.335 kJ/mol

for KOH

HRxn = -Qrxn/n = -1869.78 / (34.84) = -53.6676 kJ/mol

Related Questions

Navigate

• Browse (All)
• Browse H
• Subjects

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