The pressure inside a hydrogen-filled container was 2.10 atm at 21 C . What would the pressure be if the container was heated to 86 C?
Pfinal = ?? atm
It is 2.56
2.1/(274.15+21) = .0071150263
Answer x (274.15+86) = 2.56
Mastering Chemistry
answer is 2.63
To find the final pressure, we can use the combined gas law equation, which is:
(P1 * V1) / (T1) = (P2 * V2) / (T2)
Where:
P1 = initial pressure
V1 = initial volume (assumed constant in this case)
T1 = initial temperature
P2 = final pressure
V2 = final volume (assumed constant in this case)
T2 = final temperature
We have the initial pressure P1 = 2.10 atm, initial temperature T1 = 21°C = 21 + 273.15 K = 294.15 K, and the final temperature T2 = 86°C = 86 + 273.15 K = 359.15 K.
We can assume the volume of the container remains constant, so V1 = V2.
Plugging in the known values into the combined gas law equation, we have:
(2.10 atm * V1) / 294.15 K = (P2 * V1) / 359.15 K
Now, we can solve for P2 (final pressure):
P2 = (2.10 atm * 359.15 K) / 294.15 K
P2 = 2.57 atm (rounded to two decimal places)
Therefore, the final pressure inside the hydrogen-filled container, when heated to 86°C, would be approximately 2.57 atm.