Description
I am working through an experiment where 3.016g of NH4NO3(s) was dissolved in 50g of H2O in a coffee cup calorimeter. I determined the qrxn = 19.655 kJ/mol (qsoln + qcup). I am now asked to calculate the change in enthalpy for the reaction in moles using deltaHrxn = Sigma deltaHf(products) - Sigma deltaHf(reactants) and the deltaHf NH4NO3 is -495 kJ/mol. I am stuck here, blanking out on how to proceed
Explanation & Answer
Thank you for the opportunity to help you with your question!
The qrxn u calculated is the enthalpy change or the heat lost when the solute dissolved .it is therefore the sigma delta H of the product.divide it by the mol weight 80 to get the delta H in kj/mol unit.
Review
Review
24/7 Homework Help
Stuck on a homework question? Our verified tutors can answer all questions, from basic math to advanced rocket science!
Similar Content
Related Tags
Fences
by August Wilson
Sula
by Toni Morrison
Uncle Tom's Cabin
by Harriet Beecher Stowe
The Point of it All - A Lifetime of Great Loves and Endeavors
by Charles Krauthammer
How to Win at the Sport of Business
by Mark Cuban
Dracula
by Bram Stoker
No Exit
by Taylor Adams
One Flew Over the Cuckoos Nest
by Ken Kesey
Freakonomics
by Stephen J. Dubner and Steven D. Levitt