A certain chemical reaction releases 480. 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 3.85 J of heat energy to raise the temperature of this calorimeter by 1 °C. Now the reaction is run until all the reactant is gone, and the temperature of the calorimeter is found to rise by 14.6 °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. moles consumed-

Explanation:

As we know that specific heat is the amount of energy required to raise the temperature by . So here, specific heat is given as 3.85 J. And, the change in temperature is .

Therefore, we will calculate the heat energy as follows.

                   q =      

                      =

                      = 56.21

Since, it is given that heat released for 1 mole\ is 480 kJ or 48000 J (as 1 kJ = 1000 J). Therefore, moles required to produce 56.21 of heat is calculated as follows.

                = moles

Thus, we can conclude that number of moles of reactant that were consumed are moles.

answer: i would say b.

explanation:

"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"