What is the pressure of a fixed volume of hydrogen gas at 38.8°C if it has a pressure of 1.36 atm at 15.0°C?
(P1/T1) = (P2/T2)
so; 1.36/38.8=P1/150
0.52 is my answer?
To find the pressure of a fixed volume of hydrogen gas at a different temperature, you can use the combined gas law. The combined gas law states that the ratio of the initial pressure to the initial temperature is equal to the ratio of the final pressure to the final temperature.
To use the combined gas law, we need to convert the temperatures to Kelvin since temperature must be expressed in Kelvin in gas law calculations.
To convert the temperature given in °C to Kelvin, you add 273.15 to the Celsius temperature.
So, the initial temperature is 15.0°C + 273.15 = 288.15 K.
Next, we need to convert the final temperature to Kelvin.
The final temperature is 38.8°C + 273.15 = 312.95 K.
Now that we have the temperatures in Kelvin, we can use the combined gas law formula:
(P1 * V1) / T1 = (P2 * V2) / T2
Where:
P1 is the initial pressure (1.36 atm),
V1 is the volume (fixed, so it cancels out),
T1 is the initial temperature (288.15 K),
P2 is the final pressure (unknown),
V2 is the final volume (fixed, so it cancels out),
and T2 is the final temperature (312.95 K).
Substituting the known values into the equation:
(1.36 atm * V1) / 288.15 K = (P2 * V1) / 312.95 K
Since the volume is fixed, it cancels out, and we can solve for P2:
1.36 atm / 288.15 K = P2 / 312.95 K
Now, let's solve for P2:
P2 = (1.36 atm / 288.15 K) * 312.95 K
P2 ≈ 1.4806 atm
Therefore, the pressure of the fixed volume of hydrogen gas at 38.8°C is approximately 1.4806 atm.