Post a New Question


posted by .

A calorimeter contains 21.0 mL of water at 12.0 degress Celsius. When 2.40g of X (a substance with a molar mass of 50.0 g/mol ) is added, it dissolves via the reaction
X(s)+H2O(l) --> X (aq)

and the temperature of the solution increases to 29.5 degress celsius.
Calculate the enthalpy change, H , for this reaction per mole of X .

Assume that the specific heat and density of the resulting solution are equal to those of water [4.18 J/(g* degress celsius and 1.00 g/mL ] and that no heat is lost to the calorimeter itself, nor to the surroundings.

Express your answer numerically in kilojoules per mole.

  • Chemistry -

    Please note that we don't do students' homework for them. Our tutors try to give you the information to help you complete your assignment on your own. If there's not a tutor with this specialty online right now, be sure to go back into your textbook or use a good search engine.

    Once YOU have come up with attempted answers to YOUR questions, please re-post and let us know what you think. Then someone here will be happy to comment on your thinking.


  • Calorimetry -

    thats not really helpful to students who need chistry least the tudors will give you a generic format to get you started. saying you don't do homework doesnt benfit have wasted our time

  • Calorimetry -

    -30.2 kJ/mol

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

More Related Questions

Post a New Question