A rigid container has an initial pressure of 1.50 atm at 21oC. What will the pressure be if the temperature is increased to 121oC?
To solve this problem, we can use the combined gas law, which states that the initial pressure multiplied by the initial temperature is equal to the final pressure multiplied by the final temperature.
Using this formula, we can write:
(P1 * T1) = (P2 * T2)
Where:
P1 = initial pressure = 1.50 atm
T1 = initial temperature = 21°C + 273.15 K (converted to Kelvin) = 294.15 K
P2 = final pressure (what we want to find)
T2 = final temperature = 121°C + 273.15 K (converted to Kelvin) = 394.15 K
Now we can plug in these values and solve for P2:
(1.50 atm * 294.15 K) = (P2 * 394.15 K)
Multiply out the equation:
441.225 atm*K = P2 * 394.15 K
To isolate P2, divide both sides of the equation by 394.15 K:
441.225 atm*K / 394.15 K = P2
P2 ≈ 1.118 atm
Therefore, the pressure will be approximately 1.118 atm when the temperature is increased to 121°C.