The pressure inside a hydrogen-filled container was 2.10 at 21 . What would the pressure be if the container was heated to 96?
Use the combined gas law:
P1V1/T1=P2V2/T2
temps need to be in Kelvins.
.46
2.74
To determine the pressure inside the hydrogen-filled container when it is heated to 96 degrees, we can make use of the ideal gas law equation, which states:
PV = nRT
Where:
P is the pressure of the gas
V is the volume of the gas
n is the number of moles of gas present
R is the ideal gas constant
T is the temperature of the gas in Kelvin
First, we need to convert the given temperatures from degrees Celsius to Kelvin. To convert Celsius to Kelvin, we add 273.15 to the Celsius value.
Given:
Initial temperature = 21 degrees Celsius
Final temperature = 96 degrees Celsius
Initial temperature in Kelvin = 21 + 273.15 = 294.15 K
Final temperature in Kelvin = 96 + 273.15 = 369.15 K
The initial pressure inside the container is given as 2.10 atm.
Now, let's assume the volume, number of moles, and the ideal gas constant remain constant. Substituting the values into the ideal gas law equation, we have:
P1V1/T1 = P2V2/T2
Where:
P1 = Initial pressure
V1 = Volume
T1 = Initial temperature
P2 = Final pressure (what we need to find)
V2 = Volume
T2 = Final temperature
Rearranging the equation to solve for P2, we get:
P2 = (P1 x V1 x T2) / (V2 x T1)
Substituting the given values:
P1 = 2.10 atm
T1 = 294.15 K
T2 = 369.15 K
Since the volume (V1 and V2) and the number of moles are assumed to be constant, we can cancel them out.
P2 = (2.10 atm x 369.15 K) / 294.15 K
Performing the calculation:
P2 = 2.642 atm
Therefore, the pressure inside the hydrogen-filled container would be approximately 2.642 atm when heated to 96 degrees Celsius.