3. If 15.0 mL of a 1.5M HCl solution at 21.50C is mixed with 25.0mL of a 1.5M NaOH
solution at 21.50C that is in a calorimeter, and the final mixed solution temperature
rises to 28.50C, what is the ΔHrxn for 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 in temperature?
c. Calculate the amount of heat absorbed or lost for the HCl/NaOH solution.
Assume aqueous conditions. (Cwater = 4.18 J/g·K , d = 1.0 g/mL).
d. Calculate the amount of heat absorbed or lost by the calorimeter. The
calorimeter’s initial temperature is the same as the solution that is initially
inside it.
e. Determine the amount of heat absorbed or lost during this reaction.
f. Which of the reactants is the limiting reagent? Determine the moles of the
limiting reagent.
g. Determine the amount of heat given off per mole of limiting reagent (ΔHrxn).
Make sure to include an appropriate sign indicating whether it is an
endother
1 answer