A sample of nitrogen gas in a 1.86-L container exerts a pressure of 1.32 atm at 20 C.

What is the pressure if the volume of the container is maintained constant and the temperature is raised to 354 C?

(V1/T1) = (V2/T2)

To determine the pressure if the volume is constant and the temperature is raised, you can use the combined gas law equation: P₁ * V₁ / T₁ = P₂ * V₂ / T₂, where P₁, V₁, and T₁ are the initial pressure, volume, and temperature, and P₂, V₂, and T₂ are the new pressure, volume, and temperature.

Given values:
P₁ = 1.32 atm (initial pressure)
V₁ = 1.86 L (initial volume)
T₁ = 20 °C (initial temperature)

To use the combined gas law, we need to convert the initial temperature to Kelvin (K) by adding 273.15: T₁ = 20 + 273.15 = 293.15 K.

The final volume (V₂) is the same as the initial volume since it is maintained constant.

The final temperature (T₂) is 354 °C. To convert it to Kelvin, we add 273.15: T₂ = 354 + 273.15 = 627.15 K.

Now we can plug in the values into the formula:

P₁ * V₁ / T₁ = P₂ * V₂ / T₂

1.32 atm * 1.86 L / 293.15 K = P₂ * 1.86 L / 627.15 K

Simplifying the equation:

P₂ = (1.32 atm * 1.86 L * 627.15 K) / (1.86 L * 293.15 K)

P₂ = 2.8 atm

Therefore, the pressure of the nitrogen gas when the volume is maintained constant and the temperature is raised to 354 °C is approximately 2.8 atm.