Question

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/mol. The molar mass of carbon dioxide is 44.0095 g/mol.

Answer 1

Answer: Heat associated with the formation of 100.0 g of carbon dioxide is 1563.2 kJ.

Explanation:

Reaction equation will be as follows.

    $2C_{8}H_{18} + 25O_{2} \rightarrow 16CO_{2} + 18H_{2}O$;  $\Delta H^{o}_{rxn}$ = -11018 kJ

Mass of $CO_{2}$ = 100 g

Hence, moles of $CO_{2}$ present will be calculated as follows.

       No. of moles = $\frac{mass}{\text{molar mass}}$

                             = $\frac{100 g}{44.0095 g/mol}$

                             = 2.27 mol

Therefore, heat produced by 2.27 mol for the given reaction will be calculated as follows.

         $2.27 mol \times \frac{11018 kJ}{16 mol CO_{2}}$

             = 1563.2 kJ

Thus, we can conclude that heat associated with the formation of 100.0 g of carbon dioxide is 1563.2 kJ.

Answer 2

The heat associated with the formation of 100.0 g of carbon dioxide will be "1563.2 kJ". To understand the calculation, check below.

Reaction equation

According to the question,

2C₈H₁₈ + 25O₂ $\rightarrow$ 16CO₂ + 18H₂O

Octane's Molar mass = 114.33 g/mol

CO₂ molar mass = 44.0095 g/mol

Mass of CO₂ = 100 g

Now,

No. of moles of CO₂ present,

= $\frac{Mass}{Molar \ mass}$

By substituting the values,

= $\frac{100}{44.0095}$

= 2.27 mol

hence,

The associated heat be:

= 2.27 × $\frac{11018}{16}$

= 1563.2 kJ

Thus the above answer is correct.

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