please reply with (I don\'t know the answer) if you are not 100% sure about your

Question

please reply with (I don't know the answer) if you are not 100% sure about your answer. PLEASE DO THAT.

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Sapling Learning macmilan learning 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 following balanced, thermochemical equation: AH-764 kJ How much methanol (in grams) must be burned to produce 967 kJ of heat? Number

Explanation / Answer

when 1 mol of methanol reacts, heat produced = 764 KJ
So,
for 967 KJ, moles of methanol reacting = 967/764 = 1.266 mol

Molar mass of CH3OH,
MM = 1*MM(C) + 4*MM(H) + 1*MM(O)
= 1*12.01 + 4*1.008 + 1*16.0
= 32.042 g/mol

mass of CH3OH,
m = number of mol * molar mass
= 1.266 mol * 32.042 g/mol
= 40.6 g

Answer: 40.6 g

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