If 2.500 g of Mg is burned in a constant volume calorimeter with a heat capacity of 1.10 kJ/degrees Celsius containing 1.500 L of water at 23.50 degrees Celsius and releases 37.33 kJ of heat, what is the final temperature of the calorimeter and water?
Please show your work and solve. Thank you.
We know that heat gained = heat lost and so
q(mg burned)=q(calorimeter) + q (water)
q mg released is 37.33 KJ.
So we can then say that -37.33KJ = mcDT(H2O) + mcDT(calorimeter) note that DT is delta temperature)
We have the volume of the water, which ...
This solution describes how to find temperature using mass and heat capacity.