1 Reaction between NaOH and HCl Trial 1 Calorimeter 1 Trial 2 Calorimeter 2

1 reaction between naoh and hcl trial 1 calorimeter 1

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1. Reaction between NaOH and HCl. Trial 1 Calorimeter #1 Trial 2 Calorimeter #2 Mass of entire solution, (g). Hint: Assume the density of both solutions = 1.0 g/mL Initial temperature of HCl prior to mixing, T i (ºC) T f after mixing (highest or lowest T over 3 minutes) (ºC) ΔT (ºC) q soln (kJ) q cal (kJ) q rxn (kJ) ΔH rxn (kJ) Average ΔH rxn (kJ) Show all calculations necessary to fill in the table above:
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2. Reaction between NaOH and NH 4 Cl. Trial 1 Calorimeter #1 Trial 2 Calorimeter #2 Mass of entire solution, (g). Hint: Assume the density of both solutions = 1.0 g/mL Initial temperature of NaOH prior to mixing, T i (ºC) T f after mixing (highest or lowest T over 3 minutes) (ºC) ΔT (ºC) q soln (kJ) q cal (kJ) q rxn (kJ) ΔH rxn (kJ) Average ΔH rxn (kJ) Show all calculations necessary to fill in the table above:
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3. Reaction between HCl and NH 3 . Trial 1 Calorimeter #1 Trial 2 Calorimeter #2 Mass of entire solution, (g). Hint: Assume the density of both solutions = 1.0 g/mL Initial temperature of HCl prior to mixing, T i (ºC) T f after mixing (highest or lowest T over 3 minutes) (ºC) ΔT (ºC) q soln (kJ) q cal (kJ) q rxn (kJ) ΔH rxn (kJ) Average ΔH rxn (kJ) Using Hess’s Law and your average ΔH rxn for reactions 1 and 2, what would you have expected ΔH rxn to equal Show all calculations necessary to fill in the table above:
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4. Heat of Solution for Dissolving Ammonium Nitrate. Trial 1 Calorimeter #1 Trial 2 Calorimeter #2 Mass of water, (g) (density = 1.0 g/mL) Initial temperature of water prior to mixing, T i (ºC) T f after mixing (highest or lowest T over 3 minutes) (ºC) ΔT (ºC) q soln (kJ) q cal (kJ) q rxn (kJ) ΔH rxn (kJ) Average ΔH rxn (kJ) Show all calculations necessary to fill in the table above:
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