When 34.5 mL of 0.545 M H2SO4 is added to 34.5 mL of 1.09 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.) H per mole of H2SO4 reacted: kJ/mol H per mole of KOH reacted: kJ/mol
When 34.5 mL of 0.545 M H2SO4 is added to 34.5 mL of 1.09 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.)
H per mole of H2SO4 reacted:
kJ/mol
H per mole of KOH reacted:
kJ/mol
Given that :
The volume of H2SO4 = 34.5 mL
The molarity of H2SO4 = 0.545 M
The volume of KOH = 34.5 mL
The molarity of KOH = 1.09 M
Initial tempertaure = 23.50°C
Final temperature = 30.17°C
The density of water = 1.00 g/mol
The specific heat of water (c) = 4.184 J/g.K
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