If 15.0 mL of a 1.5M HCl solution at 21.50C is mixed with 25.0mLof a 1.5M NaOH solution at 21.50C that is in a calorimeter, and thefinal mixed solution temperature rises to28.50C, what is theΔHrxnfor this process?Assume that Ccalorimeter= 35.5J/0C.
a.What is the balanced equation for the reaction?
b.What is the source of the heat that is causing the increase intemperature?
c.Calculate the amount of heat absorbed or lost for the HCl/NaOHsolution. Assume aqueous conditions.(Cwater= 4.18 J/g·0C, d =1.0g/mL)
d.Calculate the amount of heat absorbed or lost by thecalorimeter. The calorimeter’s initial temperature is the same asthe solution that is initially inside it.
e.Determine the amount of heat absorbed or lost during thisreaction.
f.Which of the reactants is the limiting reagent? Determine themoles of the limiting reagent.
g.Determine the amount of heat given off per mole of limitingreagent(ΔHrxn).Make sure to include an appropriate sign indicatingwhether it is an endothermic (+) or exothermic (-) process. Provideyour answer in units of kJ/mol.
