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Question 4 Part A Using the following equation for the combustion of octane, calculate the heat...

Question 4

Part A

Using the following equation for the combustion of octane, calculate the heat of reaction for 100.0 g of octane. The molar mass of octane is 114.33 g/mole.

2 C8H18 + 25 O2 → 16 CO2 + 18 H2O ΔH°rxn = -11018 kJ

Using the following equation for the combustion of octane, calculate the heat of reaction for 100.0 g of octane. The molar mass of octane is 114.33 g/mole.

2 C8H18 + 25 O2 → 16 CO2 + 18 H2O ΔH°rxn = -11018 kJ

-4.82 x 103 kJ
-9.64 x 103 kJ
-1.26 x 104 kJ
-4.82 kJ

Homework Answers

Answer #1

answer : ΔH°rxn = - 4.82 x 10^3 kJ

2 C8H18 + 25 O2 ---------------> 16 CO2 + 18 H2O                        ΔH°rxn = -11018 kJ

moles of octane = 100 / 114.33 = 0.875 mol

2 mol octane   --------------->    ΔH°rxn = -11018 kJ

0.875 mol octane   ------------------>   ??

   ΔH°rxn   = 0.875 x - 11018 / 2

ΔH°rxn = - 4.82 x 10^3 kJ

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