When methanol, CH3OH, is burned in the presence of oxygen gas

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When methanol, CH3OH, is burned in the presence of oxygen gas

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

How much methanol, in grams, must be burned to produce 865 kJ of heat? mass:

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Answer 1

Answer #2

When 1 mole of methanol is burnt energy generated is 764 kJ of energy.

So when 933 kJ of energy is produced amount of methanol needed is 933/ 764 = 1.22 moles of methanol

Now

No of moles = amount of methanol (in grams)/ molecular mass

So amount of methanol= no of moles* molecular mass

= 1.22* 32= 39.04 grams of methanol must be burnt

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Answer 2

Answer #1

The solution is very simple, make sure you follow each step very carefully

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Answer 3

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When methanol, CH3OH, is burned in the presence of oxygen gas

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