May 29, 2024, 04:24:27 AM
Forum Rules: Read This Before Posting


Topic: Regarding Enthalpy Topic  (Read 4717 times)

0 Members and 1 Guest are viewing this topic.

Offline Zhadows

  • Very New Member
  • *
  • Posts: 2
  • Mole Snacks: +0/-0
Regarding Enthalpy Topic
« on: December 21, 2007, 06:56:43 PM »
Question goes like this:

When 25.0 ml of 1.0M H2SO4 is added to 50.0 ml of 1.0M NaOH at 25 CelSius in a calorimeter, the temperature of the aqueous solution increases to 33.9 Celsius. Assuming that the Specific heat of the solution is 4.18 J/(G*Celsius), that its density is 1.00 g/ml, and that the calorimeter itself absorbs a negligible amount of heat, calculate the [delta h=change in heat] in Kj for the reaction:

H2SO4 (aq) + 2 NaOH (aq) => 2 H2O(l) = Na2SO4


Problem:
Well, I compared my answer to the actual one which is [ -1.1 x 10^2] and I was off...

I utilized the equation q=c*m*delta T => [4.18]*[75g]*[33.9-25], managed to get 2.8*10^3

Any help would be appreciated.


Offline Borek

  • Mr. pH
  • Administrator
  • Deity Member
  • *
  • Posts: 27689
  • Mole Snacks: +1803/-410
  • Gender: Male
  • I am known to be occasionally wrong.
    • Chembuddy
Re: Regarding Enthalpy Topic
« Reply #1 on: December 21, 2007, 07:33:05 PM »
This is correct amount of heat, but not "per mole" of reaction.
ChemBuddy chemical calculators - stoichiometry, pH, concentration, buffer preparation, titrations.info

Sponsored Links