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How much oxygen is required for this reaction, if I give you 120g of ethane (C₂H₆)?
2C₂H₆ + 7O₂ -> 4CO₂ + 6H₂O
How much carbon dioxide does this produce?
Given: Assume the following molar masses, C:12g, H:1g, 0:16g.
Show your calculations.

Sagot :

MysticBraineridn

First, let's calculate the amount of oxygen required for the given reaction using the stoichiometry of the reaction.

1. Calculate the moles of ethane:

Molar mass of ethane (C₂H₆) = 2*12 + 6*1 = 24 + 6 = 30g/mol

Number of moles of ethane = Mass of ethane / Molar mass of ethane

Number of moles of ethane = 120g / 30g/mol = 4 moles

2. Now we can use the balanced chemical equation to find the amount of oxygen required:

In the balanced equation:

2 moles of C₂H₆ react with 7 moles of O₂

So, 4 moles of C₂H₆ will react with:

(4 moles C₂H₆) * (7 moles O₂ / 2 moles C₂H₆) = 14 moles O₂

So, 14 moles of O₂ are required for the reaction.

3. Now, let's calculate the amount of carbon dioxide produced:

According to the balanced chemical equation:

2 moles of C₂H₆ produce 4 moles of CO₂

So, 4 moles of C₂H₆ will produce:

(4 moles C₂H₆) * (4 moles CO₂ / 2 moles C₂H₆) = 8 moles CO₂

4. Finally, let's convert the moles of carbon dioxide to grams using the molar mass:

Molar mass of CO₂ = 12 (C) + 16 (O) + 16 (O) = 44g/mol

Mass of carbon dioxide produced = Number of moles of CO₂ * Molar mass of CO₂

Mass of carbon dioxide produced = 8 moles * 44g/mol = 352g

So, 14 moles of oxygen are required for the reaction, and the reaction produces 352g of carbon dioxide.

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