Solve the following problems using Calorimetry. A 100 mL sample of 0.500 M HCI a

Question

Solve the following problems using Calorimetry. A 100 mL sample of 0.500 M HCI at 21.36 degree C is added to 100.0ml. of 0.500M NaOH also at 21.36 degree C in a perfect calorimeter cup. After mixing, the temperature rises to 24.70 degree C. Assume the specific heat of the reaction is 4.18 J/g C, the density of the solution is 1.00 g/mL and the calorimeter absorbs a negligible amount of heat. Determine the Delta H Examine the application of the first law of thermodynamics to this system. 1st Law: Heat gained + heat lost = 0 What gained heat: _______________ What lost heat/energy: ______________ How much heat (q) (in J) is absorbed by the solution? What is the heat of this reaction in kJ/mole of the HCI.

Explanation / Answer

mass of the solution = Volume*density =200*1 =200 gm

deltaH=Q= heat abosrbed by calorimeter= mass* specific heat* temperature difference = 200*4.184*(24.7-21.36)=2794 Joules

since heat is evolved, deltaH=-2794 J

the reaction is HCl+ NaOH----> NaCl + H2O

moles of HCl in 100ml of 0.5M = Molarity* Volume(L)= 0.5*0.1=0.05=moles of fNaOH

enthalpy change/per moles = -2794/0.05=-55880 J/mole= -55.88 Kj/mole

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