The balanced equation for combustion in an acetylene torch is shown below: 2C2H2 + 502 4CO2 + 2H2O
The acetylene tank contains 35.0 mol C2H2, and the oxygen tank contains 84.0 mol O2-
How many moles of O2 are needed to react completely with 35.0 mol C2H2?
mol O2

"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"

the answer is minerals.

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