Thermodynamics Question

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

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Final Answer

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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.

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Carnegie Mellon University

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