Answer to Question #280868 in General Chemistry for Sib

Question

Combustion reactions are a notable source of carbon dioxide in the environment. Using the following

balanced equation, how many grams of carbon dioxide are formed when 100.00 g of propane (C3H8) is

burned? Express your answer to the correct number of significant figures. Be sure to show all steps

completed to arrive at the answer.

Answer 1

First begin by writing the correct balanced equation.

$C_{3}H_{8}+5H_2O\longrightarrow3CO_{2}+4H_2O$

According to the equation, one mole of propane which is 44g burns in air produce three moles of carbon (iv) oxide which is 132g.

The following relation can therefore be created.

$44g\space propane\equiv132g\space Carbon (i v) oxide$

100g of propane will therefore produce the following. $\frac{100}{44}×132=300g.$ Notice that it still obeys Gay Lussac's law.