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Chemistry Forums for Students => High School Chemistry Forum => Topic started by: petroleum on December 10, 2006, 12:57:36 PM

Title: Enthalpy Problem
Post by: petroleum on December 10, 2006, 12:57:36 PM

Could I get a solution to this question?

In a laboratory experiment in calorimetry, 100 mL of 0.500 M of acetic acid is mixed with 100 mL of 0.500 M sodium hydroxide in a calorimeter. The temperature rises from 25.00 C to 27.55 C. The heat capacity of the calorimeter is 150.48 J/C, and the density of the resulting solution is 1.034g/mL. Given that the specific heat capacity of 0.250 M of sodium acetate is 4.034 Jg-1C-1, calculate the enthalpy of neutralization of acetic acid.

Answer: -50.2kJ/mol

Title: Re: Enthalpy Problem
Post by: Borek on December 10, 2006, 03:11:16 PM

Please read forum rules (http://www.chemicalforums.com/index.php?page=forumrules).

Title: Re: Enthalpy Problem
Post by: petroleum on December 10, 2006, 04:34:49 PM

I waited for so long to get this crappy reply?

can you atleast help me with my question?

Title: Re: Enthalpy Problem
Post by: Donaldson Tan on December 10, 2006, 06:08:13 PM

Quote from: petroleum on December 10, 2006, 04:34:49 PM

I waited for so long to get this crappy reply?

We emphasis the Socrates' Method of Teaching here. Here's a hint for you

Enthalpy of Neutralisation = Heat Absorbed by Solution