A sample of gas with a volume of 14.9 liters at 2.6 atmospheres pressure and a temperature of 25°C is allowed to expand to a volume of 29.3 liters at a temperature of 15°C. What is the final pressure (atm)atof the gas?
See your other posts.
PV=nRT
14.9L*2.6atm=n*0.08206*(25+273.15)
n=1.583mol
PV=nRT
P*29.3L=1.583mol*(15+273.15)*0.08206
P=1.2778atm
To find the final pressure of the gas, we can use the combined gas law equation:
(P1 * V1) / (T1) = (P2 * V2) / (T2)
Where:
P1 and P2 are the initial and final pressures of the gas,
V1 and V2 are the initial and final volumes of the gas,
T1 and T2 are the initial and final temperatures of the gas.
Let's plug in the given values into the equation:
(P1 * 14.9 L) / (25°C + 273.15) = (P2 * 29.3 L) / (15°C + 273.15)
Simplifying the equation, we have:
(P1 * 14.9) / 298.15 = (P2 * 29.3) / 288.15
Now, let's solve for P2 (final pressure):
P2 = (P1 * 14.9 * 288.15) / (29.3 * 298.15)
Substituting the given values:
P2 = (2.6 atm * 14.9 * 288.15) / (29.3 * 298.15)
P2 ≈ 1.737 atm
Therefore, the final pressure of the gas is approximately 1.737 atm.