Step-by-step explanation:
To find the pressure of the gas at 20.0 °C, we can use the combined gas law, which states:
(P1 * V1) / (T1) = (P2 * V2) / (T2)
Where:
P1 = Initial pressure
V1 = Initial volume
T1 = Initial temperature
P2 = Final pressure (what we're trying to find)
V2 = Final volume (assuming the volume remains constant)
T2 = Final temperature
Given:
P1 = 4.40 atm
T1 = 60.0 °C = 333.15 K (converting to Kelvin)
T2 = 20.0 °C = 293.15 K (converting to Kelvin)
Since the volume is assumed to remain constant (rigid container), we can simplify the equation as follows:
P1 / T1 = P2 / T2
Now, we can substitute the given values and solve for P2:
(4.40 atm) / (333.15 K) = P2 / (293.15 K)
Cross-multiplying:
P2 = (4.40 atm) * (293.15 K) / (333.15 K)
≈ 3.874 atm
Therefore, the pressure of the gas at 20.0 °C is approximately 3.874 atm.