Question

Determine the change in volume that takes place when a 2.00 L sample of N2 gas is heated from 250 C to 500 C.

Answer 1

The volume of a 2.00 L sample of N2 gas increases by approximately 0.95 L when heated from 250 °C to 500 °C at constant pressure, according to Charles's law.

Step-by-step explanation:

To determine the change in volume that occurs when a 2.00 L sample of N2 gas is heated from 250 °C to 500 °C without a change in pressure, we use Charles's law. Charles's law states that the volume of a gas is directly proportional to its temperature (in Kelvin) at constant pressure. This means we can set up the equation V1/T1 = V2/T2.

The temperatures need to be converted from Celsius to Kelvin:

• 
  
• T1 = 250 °C + 273.15 = 523.15 K
• 
  
• T2 = 500 °C + 273.15 = 773.15 K

Plugging in the values into Charles's law and solving for V2 (the new volume), we get:

V1/T1 = V2/T2

(2.00 L) / (523.15 K) = V2 / (773.15 K)

V2 = (2.00 L) * (773.15 K) / (523.15 K)

V2 ≈ 2.95 L

The change in volume is the final volume minus the initial volume:

ΔV = V2 - V1 = 2.95 L - 2.00 L ≈ 0.95 L

So, the volume of the gas increases by approximately 0.95 L when heated from 250 °C to 500 °C at constant pressure.

Answer 2

V₂ = 2.96 L

Step-by-step explanation:

Given data:

Initial volume = 2.00 L

Initial temperature = 250°C

Final volume = ?

Final temperature = 500°C

Solution:

First of all we will convert the temperature into kelvin.

250+273 = 523 k

500+273= 773 k

According to Charles's law,

V∝ T

V = KT

V₁/T₁ = V₂/T₂

V₂ = T₂V₁/T₁

V₂ = 2 L × 773 K / 523 k

V₂ = 1546 L.K / 523 k

V₂ = 2.96 L