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initial temperature of 23.4 o C

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initial temperature of 23.4 o C

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  1. Thermochemistry Lab Problem: 2.552 g of KOH was dissolved in 95.0 mL of water with an initial temperature of 23.4 oC. The temperature rose to 70.5 oC. Given the density of water as 1.00g/mL and the specific heat of the solution as 4.18 J/g∙oC. Calculate the enthalpy of the reaction and the enthalpy in kJ per mole of KOH. Reaction: KOH(s) → K+(aq) + OH-(aq) Final temperature 70.5 oC initial temperature of 23.4 oC 95.5 mL of H2O and 2.552 g KOH

  2. Thermochemistry Lab Problem: 2.552 g of KOH was dissolved in 95.0 mL of water with an initial temperature of 23.4 oC. The temperature rose to 70.5 oC. Given the density of water as 1.00g/mL and the specific heat of the solution as 4.18 J/g∙oC. Calculate the enthalpy of the reaction and the enthalpy in kJ per mole of KOH. Reaction: KOH(s) → K+(aq) + OH-(aq) 1st find joules of energy released: (95.0 + 2.552)g (70.5-23.4)oC = J 19205 Assign sign: ∆HRXN = -19205 J 2nd: Now find kJ/mol KOH: 19205 J 422 2.552 g KOH Assign sign ∆H = -422 kJ/molKOH

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