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6-5. During the combustion of 10.0 g of octane, CH18, 479.0 kcal is released? Write a balanced equation for the combustion re

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Answer #1

2 C8H18 + 25 O2 = 18 H2O + 16 CO2

it is exothermic so sign is negative.

Moles in 10g = 10/molecular weight

= 10/114

= 0.087 moles

So 0.087 mole releases 479 kcal

1 mole will release= 479/0.087

= 5505.74 kcal

479 kcal is released from 10 g

1 kcal will be released from 10/479

450 k cal = (10/479)X 450

= 9.39 g

Moles = 9.39/114

= 0.082

10 g gives 479 kcal

1 g = 479/10

17 g = (479/10) X 17

= 814.3 kcal.

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