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dolphi86 [110]
3 years ago
6

Using the following equation for the combustion of octane calculate the heat associated with the formation of 100.0 g of carbon

dioxide. The molar mass of octane is 114.33 g/mole.
2C8H18 + 25O2 → 16 CO2 + 18 H2O

ΔH°rxn = -11018 kJ
Chemistry
1 answer:
natali 33 [55]3 years ago
8 0

Answer:

The right solution is "-602.69 KJ heat".

Explanation:

According to the question,

The 100.0 g of carbon dioxide:

= \frac{100.0 \ g}{114.33\  g/mole}

= 0.8747 \ moles

We know that 16 moles of CO_2 formation associates with -11018 kJ of heat, then

0.8747 moles CO_2 formation associates with,

= -\frac{0.8747}{16}\times 11018 \ KJ \ of \ heat

= -0.0547\times 11018

= -602.69 \ KJ \ heat

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260.34g

Explanation:

First, you need to know what angelic acid is comprised of. It is written as C₅H₈O₂.

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