Consider the compound NH4Cl, ammonium chloride, having a molar mass of 53.491 g/mol. Nicole weighs out 12.41g of NH4Cl and also 125.0 g of water for her calorimetry experiment. Nicole dissolves her ammonium chloride in the water and finds that the temperature of the water decreases from 23.7°C to 17.3°C. Assume the specific heat capacity of the water, Cs,water, is 4.184 J/(g °C) and that no energy is transferred to the calorimeter (qcal = 0 J). Using your result of 3344 J, calculate the enthalpy of reaction, ∆Hrxn, in units of kJ/mol. If the true value for ∆Hrxn is +14.8 kJ/mol, calculate Nicole’s percent error.

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Consider the compound NH4Cl, ammonium chloride, having a molar mass of 53.491 g/mol. Nicole weighs out 12.41g of NH4Cl and also 125.0 g of water for her calorimetry experiment. Nicole dissolves her ammonium chloride in the water and finds that the temperature of the water decreases from 23.7°C to 17.3°C. Assume the specific heat capacity of the water, Cs,water, is 4.184 J/(g °C) and that no energy is transferred to the calorimeter (qcal = 0 J).

  • Using your result of 3344 J, calculate the enthalpy of reaction, ∆Hrxn, in units of kJ/mol.
  • If the true value for ∆Hrxn is +14.8 kJ/mol, calculate Nicole’s percent error.

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