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Solved: Certain race cars use methanol (CH3OH, also called
Chapter 3, Problem 68P(choose chapter or problem)
Certain race cars use methanol (\(\mathrm{CH}_{3} \mathrm{OH}\), also called wood alcohol) as a fuel. The combustion of methanol occurs according to the following equation:
\(2 \mathrm{CH}_{3} \mathrm{OH}(l)+3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{CO}_{2}(g)+4 \mathrm{H}_{2} \mathrm{O}(l)\)
In a particular reaction, 9.8 moles of \(\mathrm{CH}_{3} \mathrm{OH}\) are reacted with an excess of \(\mathrm{O}_{2}\). Calculate the number of moles of \(\mathrm{H}_2\mathrm{O}\) formed.
Questions & Answers
QUESTION:
Certain race cars use methanol (\(\mathrm{CH}_{3} \mathrm{OH}\), also called wood alcohol) as a fuel. The combustion of methanol occurs according to the following equation:
\(2 \mathrm{CH}_{3} \mathrm{OH}(l)+3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{CO}_{2}(g)+4 \mathrm{H}_{2} \mathrm{O}(l)\)
In a particular reaction, 9.8 moles of \(\mathrm{CH}_{3} \mathrm{OH}\) are reacted with an excess of \(\mathrm{O}_{2}\). Calculate the number of moles of \(\mathrm{H}_2\mathrm{O}\) formed.
ANSWER:
Step 1 of 2
Here we have to calculate the number of moles of .
Given:
Moles of = 9.8 moles
The given equation for combustion of methanol is,