Using the following equation for the combustion of octane,calculate the amount of grams of carbon dioxide formed from 100.0 g of octane.The molar mass of octane is 114.33 g mol^-1.The molar mass of carbon dioxide is 44.0095 g mol^-1. 2C₈H₁₈ + 25O₂ → 16CO₂ + 18H₂O
D_rH°= -11018 kJ

Question

Quizplus · Accepted Answer

To solve this problem, we need to use stoichiometry. From the balanced equation, we can see that for every 2 moles of octane burned, 16 moles of carbon dioxide are produced.

First, we need to convert the given mass of octane to moles:

100.0 g octane x (1 mol octane/114.33 g octane) = 0.874 mol octane

Next, we can use the mole ratio from the balanced equation to find the number of moles of carbon dioxide produced:

0.874 mol octane x (16 mol CO2/2 mol octane) = 6.992 mol CO2

Finally, we can convert moles of CO2 to grams:

6.992 mol CO2 x 44.0095 g CO2/mol = 307.9 g CO2

Therefore, the answer is B.

Using the Following Equation for the Combustion of Octane,calculate the Amount