Answer:
Amount of heat released when 25.0 g of [tex]C_{3}H_{7}OH[/tex] (rubbing alcohol) is combusted equal to 98.7 kJ
Explanation:
According to balanced equation (as given in problem), combustion of 2 moles of rubbing alcohol release 474.28 kJ of heat.
Molar mass of [tex]C_{3}H_{7}OH[/tex] (rubbing alcohol) = 60.095 g/mol
We know, number of moles of a compound is the ratio of mass to molar mass of that compound.
So, 2 moles of [tex]C_{3}H_{7}OH[/tex] (rubbing alcohol) = [tex](2\times 60.095)g[/tex] [tex]C_{3}H_{7}OH[/tex] (rubbing alcohol) = 120.19 g of [tex]C_{3}H_{7}OH[/tex] (rubbing alcohol)
So, combustion of 120.19 g of rubbing alcohol release 474.28 kJ of heat.
Hence amount of heat released when 25.0 g of [tex]C_{3}H_{7}OH[/tex] (rubbing alcohol) is combusted = [tex](474.28\times \frac{25.0}{120.19})kJ=98.7kJ[/tex]
