In the reaction 2 c o2 → 2 co, how many moles of carbon are needed to produce 66.0 g of carbon monoxide

The solution would be like this for this specific problem:

Given:

66.0 g of carbon monoxide

reaction 2 C + O2 → 2 CO

 

mol e= mass / molar mass 
mole of 2CO = 66.0g / (12.011  15.999)g / mol 
mole of 2CO = 2.36 (CO and C has a 1:1 mole ratio) 

mole of 2CO = 2.36 -> mole of 1 CO = 2.36 / 2 = 1.18 

We got 2 moles of C, thus 1.18 x 2 = 2.36

So, we 2.36 moles of carbon are needed to produce 66.0 g of carbon monoxide in the reaction 2 C + O2 → 2 CO.   To add, Carbon nonmetallic and tetravalent, thus, making four electrons available to form covalent chemical bonds. 

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