A 7.12g sample was combusted in a calorimeter with a q of 525 J/°C. The 1251 mL of water temperature went from 7.1°C to 21.4°C. How much energy was released? [An explanation as to how the answer is gotten would be much appreciated as calorimetry isn't really one of my fortes...]​

Explanation:

A 7.12g sample was combusted in a calorimeter with a q of 525 J/°C. The 1251 mL of water temperature went from 7.1°C to 21.4°C. How much energy was released?

[An explanation as to how the answer is gotten would be much appreciated as calorimetry isn't really one of my fortes...]

ans 44.100 j

pop pop pop on a opp

"you start with 15.67 g mgco3-xh2o, when heated and all the water is removed, you are left with 7.58 g mgco3 only.

therefore, you had 15.67 - 7.58 = 8.09g h2o  

moles of each :

7.58g mgco3 = ? moles = 7.58g / 83.4g/mole = 0.09moles  

8 09g h2o = ? moles = 8.09g / 18g/mole = 0.44moles  

molar ratio between the two by dividing both numbers by the smallest number :

0.09 / 0.09 = 1  

0.44 / 0.09 = 4.8  

mgco3-5h2o"