Question

2C8H18 + 25O2 → 16CO2 + 18H2O ΔH° rxn = -11020 kJ/mol rxn Look at above...

2C8H18 + 25O2 → 16CO2 + 18H2O ΔH° rxn = -11020 kJ/mol rxn Look at above equation. How many kJ of heat will be released when 7.00 grams of C8H18 is combusted?

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Answer #1

Molar mass of C8H18 = 8*MM(C) + 18*MM(H)

= 8*12.01 + 18*1.008

= 114.224 g/mol

mass of C8H18 = 7.00 g

we have below equation to be used:

number of mol of C8H18,

n = mass of C8H18/molar mass of C8H18

=(7.0 g)/(114.224 g/mol)

= 6.128*10^-2 mol

From reaction,

when 2 mol of C8H18 is combusted, heat released = 11020 KJ

So,

for 6.128*10^-2 mol, heat released = 11020 KJ * 6.128*10^-2 / 2 = 338 KJ

Answer: 338 KJ

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