Question

A sample of methane gas having a volume of 2.80 L at 25C and 1.65 atm was mixed with a sample of oxygen having a volume of 35.0 L at 31C and 1.25 atm. The mixture was then ignited to form carbon dioxide and water. Calculate the volume of CO₂ formed at a pressure of 2.50 atm and a temperature of 125C.

Answer 1

The volume of CO₂ formed at a pressure of 2.50 atm and a temperature of 125°C is 3.48 L.

Step-by-step explanation:

To calculate the volume of CO₂ formed at a pressure of 2.50 atm and a temperature of 125°C, we can use the ideal gas law equation:

P₁V₁/T₁ = P₂V₂/T₂

Where P₁, V₁, and T₁ represent the initial pressure, volume, and temperature of the methane gas, and P₂, V₂, and T₂ represent the final pressure, volume, and temperature.

Let's substitute the given values into the equation:

(1.65 atm)(2.80 L)/(25 + 273) = (2.50 atm)(V₂)/(125 + 273)

Simplifying the equation, we find:

V₂ = (1.65 atm)(2.80 L)(398 K)/(2.50 atm)(398 K) = 3.48 L

Therefore, the volume of carbon dioxide formed at a pressure of 2.50 atm and a temperature of 125°C is 3.48 L.