The pressure inside a hydrogen-filled container was 2.10 at 21 . What would the pressure be if the container was heated to 85?
8.5 to get the answer use a simple math equation where 21x= 85*2.1. Resulting in 21x= 178.5. then solve that equation and get the answer 8.5...
When posting questions, be sure to include units.
Pressure can be in kPas, psi, psi guage (the latter is not proportional to temperature).
Temperature could have been in °K, °C (the latter is not proportional to pressure).
Hint: use the ideal gas law
PV=nRT
but be sure to convert all quantities to consistent units.
To determine the final pressure inside the hydrogen-filled container when it is heated to 85 degrees, we can use the ideal gas law equation:
PV = nRT
Where:
P = pressure
V = volume
n = number of moles
R = ideal gas constant
T = temperature
First, let's list the given information:
Initial pressure (P1) = 2.10 atm
Initial temperature (T1) = 21 degrees
We need to convert the temperatures to Kelvin since the ideal gas law requires temperature in Kelvin. To convert from Celsius to Kelvin, we add 273.15 to the Celsius temperature:
Initial temperature (T1) in Kelvin = 21 + 273.15 = 294.15 K
Next, we need to find the final temperature (T2) after the container is heated to 85 degrees Celsius:
Final temperature (T2) = 85 + 273.15 = 358.15 K
Since the number of moles (n), volume (V), and the gas constant (R) are not given, we can assume that they remain constant throughout the process. Therefore, we can rewrite the ideal gas law equation as:
P1/T1 = P2/T2
Now, we can plug in the values we have into the equation and solve for the final pressure (P2):
P1/T1 = P2/T2
2.10 atm / 294.15 K = P2 / 358.15 K
Cross-multiplying the equation:
P2 = (2.10 atm) * (358.15 K) / 294.15 K
P2 = 2.56 atm
Therefore, the pressure inside the container when heated to 85 degrees would be approximately 2.56 atm.