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Isooctane (C₈H₁₈; d = 0.692 g/mL) is used as the fuel in a test of a new automobile drive train.
(a) How much energy (in kJ) is released by combustion of 20.4 gal of isooctane to gases ΔH°rxn = - 5.44 × 10³ kJ /mol?

Answer :

In the burning of 20.4 gal of isooctane, 5620 KJ is produced.

Before we can solve, we must convert the volume to milliliters.

Since 1 gal is equal to 3.8 L, 20.4 gal is equal to 20.4-gal x 3.8 L, which is 77.52 L or 77520 ml

Following are the steps for calculating isooctane's mass from its density: Mass/volume equals density.

Volume x Density Equals Mass Mass = 77520 mL x 0.692 g/mL

Mass = 53643.84 g Isooctane molecular weight is calculated from; Mole number equals mass/mole mass Isooctane's molar mass is 114 g/m.470 moles are equal to 53643.84g divided by 114 g/mol.470 moles of isooctane yield 413 moles 5.44 103 kJ / 1 mole = KJ if 1 mole of isooctane produces 5620 kJ of heat.

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