Thermodynamics Question

User Generated



Question 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

Student has agreed that all tutoring, explanations, and answers provided by the tutor will be used to help in the learning process and in accordance with Studypool's honor code & terms of service.

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.

Please let me know if you need any clarification. I'm always happy to answer your questions.

PurzZnguGhgbe (755)
Carnegie Mellon University

Excellent resource! Really helped me get the gist of things.