a 30.0 L sample of nitrogen inside a rigid , metal container at 20.0 c is placed inside an oven whose temperature is 50.0 c the pressure inside the container at 20.0 c was at 3.00 atm . what is the pressure of the nitrogen after its temperature is increased?
Answers
Answer: 3.31 atm
Explanation:
Given data:
The initial temperature of the container, T₁ = 20℃ = 20+273 = 293 K
The initial pressure of nitrogen inside the container, P₁ = 3.00 atm
The final temperature inside the oven, T₂ = 50℃ = 50+273 = 323 K
To find: the Pressure of nitrogen after its temperature is increased
Let the final pressure of the nitrogen after its temperature is increased be denoted as “P₂”.
According to the Gay Lussac’s Law,
P₁ / T₁ = P₂ / T₂
⇒ 3.00/293 = P2/323
⇒ P₂ = 0.01023 * 323 = 3.307 atm ≈ 3.31 atm
Hence, the pressure of the nitrogen after its temperature is increased to 3.31 atm.
Explanation:
Answer: 3.31 atm
Explanation:
Given data:
The initial temperature of the container, T₁ = 20℃ = 20+273 = 293 K
The initial pressure of nitrogen inside the container, P₁ = 3.00 atm
The final temperature inside the oven, T₂ = 50℃ = 50+273 = 323 K
To find: the Pressure of nitrogen after its temperature is increased
Let the final pressure of the nitrogen after its temperature is increased be denoted as “P₂”.
According to the Gay Lussac’s Law,
P₁ / T₁ = P₂ / T₂
⇒ 3.00/293 = P2/323
⇒ P₂ = 0.01023 * 323 = 3.307 atm ≈ 3.31 atm
Hence, the pressure of the nitrogen after its temperature is increased to 3.31 atm.