How many liters of CO2 and H2O - measured together at 710 K - can be produced from the combustion at 710 K of 5.75 L of CH4 and as much O2 as needed?

Combustion 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.

Step 1: Write the balanced combustion reaction.

CH₄(g) + 2 O₂(g) ⇒ CO₂(g) + 2 H₂O(g)

Step 2: Calculate the volume of CO₂ produced.

According to the balanced equation, the volume ratio of CH₄ to CO₂ is 1:1.

5.75 L CH₄ × 1 L CO₂/1 L CH₄ = 5.75 L CO₂

Step 3: Calculate the volume of H₂O produced.

According to the balanced equation, the volume ratio of CH₄ to H₂O is 1:2.

5.75 L CH₄ × 2 L H₂O/1 L CH₄ = 11.5 L H₂O

In the complete combustion of 5.75 L of CH₄ at 710 K, 5.75 L of CO₂ and 11.5 L of H₂O.

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