The temperature of oxygen is 810 torr at 298 K , what will the pressure be at 330 K?
Using Lussac's Law, would the answer be 896.98 torr? Thanks
constant volume
P1=P2*T1/T2
=810*330/298=yes
For Boyle, Lussac, and Charles Law, do I have to convert the units to the standard measurement? Like temperature to kelvin and pressure to atm? Thanks
Temperature must be in kelvins. The others do not have to be changed.
Bob, could you verify this answer for me too please? Thanks
P1 = 1.08 atm
V1 = 250 mL
T1 = 297 K
T2 = 310.2 K
P2 = 2.25 atm
Would V2 = 125.3 mL?
To find the pressure of oxygen at a different temperature, we can use Charles's Law, not Lussac's Law. Lussac's Law, also known as the Gay-Lussac's Law, involves the relationship between the pressure and temperature of a gas at constant volume. On the other hand, Charles's Law focuses on the relationship between the volume and temperature of a gas at constant pressure.
To determine the pressure of oxygen at 330 K, we need to follow these steps:
Step 1: Convert the temperatures to Kelvin
The given temperature of 298 K is already in Kelvin. Convert the temperature of 330 K to Kelvin by adding 273 to it:
330 K + 273 = 603 K
Step 2: Use Charles's Law formula
According to Charles's Law, the ratio of the temperature and pressure of a gas at constant volume is constant. This can be written as:
(P1 / T1) = (P2 / T2)
In this case, P1 is the initial pressure at 298 K (810 torr), T1 is the initial temperature (298 K), T2 is the final temperature (603 K), and P2 is the final pressure (which we want to find).
(P1 / T1) = (P2 / T2)
(810 torr / 298 K) = (P2 / 603 K)
Step 3: Solve for P2
To find P2, cross-multiply and solve for it:
[(810 torr) × (603 K)] / (298 K) = P2
Using a calculator or mathematical software, you'll get:
P2 ≈ 1,638.26 torr
Therefore, the pressure of oxygen at 330 K is approximately 1,638.26 torr, not 896.98 torr.