CH3OH(g)+32O2(g)⟶CO2(g)+2H2O(l)Δ?=−764 kJ   How much methanol, in grams, must be burned to produce 657 kJ of heat? mass:

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When methanol, CH3OH, is burned in the presence of oxygen gas, O2, a large amount of heat energy is released. For this reason, it is often used as a fuel in high performance racing cars. The combustion of methanol has the balanced, thermochemical equation

 

CH3OH(g)+32O2(g)⟶CO2(g)+2H2O(l)Δ?=−764 kJ

 

How much methanol, in grams, must be burned to produce 657 kJ of heat?

mass:
 
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