A rigid container of O2 has a pressure of 3.9 atm at a temperature of 700 K. What is the pressure at 273 K?
To find the pressure of a gas at a different temperature using the ideal gas law, we can use the following equation:
P1 / T1 = P2 / T2
Where P1 and T1 are the initial pressure and temperature, and P2 and T2 are the final pressure and temperature.
In this case, we have the initial pressure P1 = 3.9 atm and initial temperature T1 = 700 K. We want to find the final pressure at 273 K, so we have P2 = ? and T2 = 273 K.
Let's plug these values into the equation and solve for P2:
P1 / T1 = P2 / T2
3.9 atm / 700 K = P2 / 273 K
To isolate P2, we can cross-multiply:
(3.9 atm)(273 K) = (P2)(700 K)
1064.7 atm K = 700 P2
Divide both sides by 700:
P2 = (1064.7 atm K) / 700
P2 = 1.52 atm
Therefore, the pressure of the O2 in the container at 273 K would be approximately 1.52 atm.