if the pressure of 1.50L of hydrogen gas at 100 degrees celsius decreases from .500atm to .115atm,what is the final volume. assume temp remains the same
Use P1V1 = P2V2
1.50
To determine the final volume, you can use the combined gas law equation, which relates the initial pressure, initial volume, final pressure, and final volume of a gas at constant temperature. The equation can be written as:
(P1 * V1) / T1 = (P2 * V2) / T2
Where:
P1 = initial pressure
V1 = initial volume
T1 = initial temperature
P2 = final pressure
V2 = final volume
T2 = final temperature
Since the problem states that the temperature remains the same, we can substitute T1 and T2 with the same value.
(P1 * V1) / T = (P2 * V2) / T
Now let's substitute the given values into the equation:
(P1 * V1) / T = (P2 * V2) / T
(0.500 atm * 1.50 L) / (100°C + 273.15 K) = (0.115 atm * V2) / (100°C + 273.15 K)
Now we can solve for V2 (final volume):
(0.500 atm * 1.50 L) / (100°C + 273.15 K) = (0.115 atm * V2) / (100°C + 273.15 K)
0.75 atm / 373.15 K = 0.115 atm * V2 / 373.15 K
0.75 atm = 0.115 atm * V2
V2 = 0.75 atm / 0.115 atm
V2 = 6.52 L
Therefore, the final volume is approximately 6.52 liters.