Post a New Question

chemistry

posted by .

When 50.0mL of 1.20 M of HCl (aq)is combined with 50.0mL of 1.30 M of NaOH (aq) in a coffee-cup calorimeter, the temperature of the solution increases by 8.01 Degrees C. What is the change in enthalpy for this balanced reaction?

HCl(aq) + NaOH(aq) --yields-- NaCl(aq) + H20(l)

Assume that the solution density is 1.00 g/mL and the specific heat capacity of the solution is 4.18 J/ g x Degrees C

  • chemistry -

    q = [mass H2O x specific heat H2O x (Tfinal-Tinitial)
    Solve for q = delta H in joules.
    Then delta H/0.06 mol = delta H in J/mol. Most of these are given in kJ/mol; I recommend you convert to kJ/mol.

  • chemistry -

    since q= 100 mL x 4.18 x 8.01
    =3348.18/.06= 55803. J
    to kJ= 55.803 should be the final answer, right? Because the answer key on my quiz says it's -55.8 kJ. I'm so confused because I thought for sure it would positive, especially since in the equation it says increases by 8.01, meaning it would be endothermic (+)? Am I missing something here?

  • chemistry -

    it's because the reaction is exothermic reaction so the answer should be negative, because in exothermic reaction the heat is released to the surrounding

Answer This Question

First Name
School Subject
Your Answer

Related Questions

More Related Questions

Post a New Question