If 61.9 L of oxygen at 17.7 degrees C and an absolute pressure of 1.55 atm are compressed to 46.4 L and at the same time the temperature is raised to 49.3 degrees C, what will the new pressure be?
P V/T will remain the same. Solve for the final P. Be sure to convert temperatures to K, first.
1223456
8g of O2 under pressure of 1 atmosphere at 27degreesC . Find the volume
To find the new pressure, we can use the combined gas law equation:
(P1 x V1) / (T1) = (P2 x V2) / (T2)
In this equation:
P1 = Initial pressure = 1.55 atm
V1 = Initial volume = 61.9 L
T1 = Initial temperature = 17.7 degrees C + 273.15 (converted to Kelvin)
P2 = New pressure (what we are trying to find)
V2 = New volume = 46.4 L
T2 = New temperature = 49.3 degrees C + 273.15 (converted to Kelvin)
Let's plug in the values and solve for P2:
(1.55 atm x 61.9 L) / (17.7 + 273.15 K) = (P2 x 46.4 L) / (49.3 + 273.15 K)
(95.7645 atm.L) / (290.85 K) = (P2 x 46.4 L) / (322.45 K)
Cross multiplying:
95.7645 atm.L x (322.45 K) = (P2 x 46.4 L) x (290.85 K)
30923.73 atm.K.L = 14184.64 P2 L.K
Dividing both sides by 14184.64 L.K:
30923.73 / 14184.64 = P2
P2 ≈ 2.18 atm
Therefore, the new pressure will be approximately 2.18 atm.