We need help on a Gen Chem 1 Calorimetry and Enthalpy lab and the TA for the class wasn't much help at all.
1) Did the reaction absorb or release heat. Using the value of q you calculated, calculate del H of the reaction in kJ/mol of reactant. (start by calculation q for the reaction; don't forget the role of the calorimeter.) (our answer is -1.8kJ, but we know this must be incorrect since the TA got approx -51 kJ and then wouldn't show us what we did wrong.)
2)Write a balanced thermochemical equation for this reaction, including the value of del H
Reactant 1 (NaOH)
mass: 52.00g
volume: 50.0mL.
moles: 1.3 mol
Reactant 2 (HCl; density=1.017g/mL)
mass: 50.85g
volume: 50.00mL
moles: 1.4 mol
Solution:
mass: 102.85g
volume: 100 mL
Tinitial: 24.1C
Tfinal: 29.0C
delT: 4.9C
c for Sol: 3.97 J/g*C
q= 2000J (calculated using q=mc(del)T
We need help on a Gen Chem 1 Calorimetry and Enthalpy lab and the TA for the class wasn't much help at all.
1) Did the reaction absorb or release heat. Using the value of q you calculated, calculate del H of the reaction in kJ/mol of reactant. (start by calculation q for the reaction; don't forget the role of the calorimeter.) (our answer is -1.8kJ, but we know this must be incorrect since the TA got approx -51 kJ and then wouldn't show us what we did wrong.)
2)Write a balanced thermochemical equation for this reaction, including the value of del H
Reactant 1 (NaOH)
mass: 52.00g
volume: 50.0mL.
moles: 1.3 mol
Reactant 2 (HCl; density=1.017g/mL)
mass: 50.85g
volume: 50.00mL
moles: 1.4 mol
Solution:
mass: 102.85g
volume: 100 mL
Tinitial: 24.1C
Tfinal: 29.0C
delT: 4.9C
c for Sol: 3.97 J/g*C
q= 2000J (calculated using q=mc(del)T
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