Question

Propane (C3H8) is a fuel commonly burned for needs such as home heating and cooking food. When propane burns, it reacts with oxygen (O2). The products of the reaction are carbon dioxide (CO2) and water (H2O). If 44.1 g of propane react completely with 160.0 g of oxygen, 132.0 g of carbon dioxide are formed. What is the mass of the other product, water, formed in this reaction?

Answer 1

Answer:

this question is so hard

Explanation:

it was in my exam and I'm still trying to figure out if I should do calculation

or just answer it with words

Answer 2

The mass of the other product, water, formed in the reaction is 72.06 g

Stoichiometry

From the question, we are to determine the mass of water formed

First, we will write the balanced chemical equation for the reaction,

The balanced chemical equation for the reaction is

C₃H₈ + 5O₂ → 3CO₂ + 4H₂O

This means

1 mole of propane reacts with 5 moles of O₂ to produce 3 moles of CO₂ and 4 moles of H₂O

Now, we will determine the number of moles of CO₂ formed.

From the formula,

$Number\ of\ moles = \frac{Mass}{Molar\ mass}$

Molar mass of CO₂ = 44.01 g/mol

Then,

Number of moles of CO₂ formed = $\frac{132}{44.01}$

Number of moles of CO₂ formed = 3 moles

Considering the balanced chemical equation,

Since 3 moles of CO₂ was formed, then 4 moles of H₂O will be formed.

Now, for the mass of H₂O formed

Using the formula,

Mass = Number of moles × Molar mass

Molar mass of H₂O = 18.015 g/mol

Therefore,

Mass of water formed = 4 × 18.015

Mass of water formed = 72.06 g

Hence, the mass of the other product, water, formed in the reaction is 72.06 g.

Learn more on Stoichiometry here: https://brainly.com/question/26283699