A certain chemical reaction releases 447. kJ of heat energy per mole of reactant

Question

A certain chemical reaction releases 447. kJ of heat energy per mole of reactant consumed. Suppose some moles of the reactant are put into a calorimeter (a device for measuring heat flow). It takes 3.26 J of heat energy to raise the temperature of this calorimeter by 1 degree C. Now the reaction is run until all the reactant is gone, and the temperature of the calorimeter is found to rise by 13.9 degree C. How would you calculate the number of moles of reactant that were consumed? Set the math up. But don't do any of it. Just leave your answer as a math expression. Also, be sure your answer includes all the correct unit symbols.

Explanation / Answer

when all the reactant is gone, the temperature rise is 13.9 deg.c

hence moles of reactant* specific heat of calorimeter* temperature difference = 44.7 kj

Assuming 1 mole of substance

1* specific heat* 13.9 = 447*1000 J

specific heat= 447*1000/13.9 = 3216 J/mole.deg.c

when 3.26 Joules of heat is supplied, the temperature rise is 1deg.c

moles* specific heat* temperature difference= 3.26

x* 3216*1= 3.26

x= 3.26/3216= 0.001 moles

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