When 33.5mL of 0.635 M H2SO4 is added to 33.5 mL of 1.27M KOH in a coffee cup ca

Question

When 33.5mL of 0.635 M H2SO4 is added to 33.5 mL of 1.27M KOH in a coffee cup calorimeter at 23.50 celcius, the temperature rises to 30.17 celcius. Calculate the deltaH of this reaction. (Assume that the total volume is the sum of the individual volumes and the density and specific heat capacity of the solution are the same as for pure water)

A) what is the deltaH per mole of H2SO4 reacted?(kJ/mol)
B)?what is the deltaH per mole of KOH reacted?(kJ/mol) When 33.5mL of 0.635 M H2SO4 is added to 33.5 mL of 1.27M KOH in a coffee cup calorimeter at 23.50 celcius, the temperature rises to 30.17 celcius. Calculate the deltaH of this reaction. (Assume that the total volume is the sum of the individual volumes and the density and specific heat capacity of the solution are the same as for pure water)

A) what is the deltaH per mole of H2SO4 reacted?(kJ/mol)
B)?what is the deltaH per mole of KOH reacted?(kJ/mol)

A) what is the deltaH per mole of H2SO4 reacted?(kJ/mol)
B)?what is the deltaH per mole of KOH reacted?(kJ/mol)

Explanation / Answer

dH = -q = -mCpdT

             = -(33.5 + 33.5)g x 4.184 J/oC x (30.17 - 23.50)

             = -1.87 kJ

A) dH per mole of H2SO4 = -1.87/(0.635 M x 33.5 ml)

                                          = -0.88 kJ/mol

B) dH per mole of KOH added = -1.87/(1.27 M x 33.5 ml)

                                                 = -0.044 kJ/mol

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