Question

9. When 4.46 moles of ethylene, C2H4, burns in oxygen to give carbon dioxide and
water, how many grams of carbon dioxide are formed?
C2H4 + 3 O2 → 2 H2O + 2 CO2
How many grams of carbon dioxide are formed??

Answer 1

Answer:

4.46 moles of Ethylene will produce 392.48 grams of Carbon dioxide.

Explanation:

The reaction is as follows

C2H4 + 3 O2 → 2 H2O + 2 CO2

For complete combustion of Ethylene 1 mole of ethylene gives 2 moles of Carbon dioxide.

using unitary method

1 C2H4 => 2CO2

4.46 of C2H4  => 2*4.46 CO2

                         =  8.92 CO2

No of moles  = given mass(w) /molar mass(M)

Molar mass of CO2 = 44g

8.92 = W / 44

W = 8.92 * 44

    = 392.48g

So 4.46 moles of Ethylene will produce 392.48 grams of Carbon dioxide.

Answer 2

4.46 moles of ethylene burns in oxygen to give 393 g of carbon dioxide and water.

What is combustion?

Combustion, or burning, is a high-temperature exothermic redox chemical reaction between a fuel and an oxidant, usually atmospheric oxygen, that produces oxidized, often gaseous products, in a mixture termed as smoke.

Let's consider the reaction for the combustion of ethylene.

C₂H₄ + 3 O₂ → 2 H₂O + 2 CO₂

We can calculate the mass of CO₂ formed by the combustion of 4.46 moles of C₂H₄, considering the following relationships.

• The molar ratio of C₂H₄ to CO₂ is 1:2.
• The molar mass of CO₂ is 44.01 g/mol.

4.46 mol C₂H₄ × (2 mol CO₂/1 mol C₂H₄) × (44.01 g CO₂/1 mol CO₂) = 393 g CO₂

4.46 moles of ethylene burns in oxygen to give 393 g of carbon dioxide and water.

Learn more about combustion here: https://brainly.com/question/9425444