Question

If 15.0 mL of a 1.5M HCl solution at 22.5 degrees C is mixed with 25.0mL of a 1.5M NaOH solution at 21.5 degrees C that is in a calorimeter, and the final mixed solution temperature ends up at 28.5 degrees C,
1.)what is the balanced equation for this reaction?
2.) what is the source of the heat that is causing the increase in temperature?
3.) Calculate the amount of heat absorbed or lost for the HCl/NaOH solution. Assume aqueous conditions.(Cwater=4.18J/gxK, d=1.0g/mL)

Answer 1

1.
HCl + NaOH ==> NaCl + H2O

2.
H^+ + OH^= ==> H2O

3.
q = mass H2O x specific heat H2O x (Tfinal-Tinitial) assuming the calorimeter can be ignored. '

4. I'm surprised there is no 4th question to calculate kJ/mol for the heat of neutralization.

Answer 2

Sorry there is,
4.) Calculate the amount of het absorbed or lost by the calorimeter. The calorimeter's initial temperature is the same as the solution that is initially inside it.
5.) Determine the amount of heat absorbed or lost during this reaction.
6.)Which of the reactants is the limiting reagent? Determine the moles.
7.)Determine the amount of heat given off per mole of LR. Make sure to include an appropriate sign indicating whether it is an exothermic or endothermic process. Answer in kJ/mol

Answer 3

4. You don't have enough information to calculate the amount of heat absorbed/lost by the calorimeter. You need the calorimeter constant or data to calculate and you have neither.
5,6,7 depend upon 4.