A gas occupies 5.65 L at 808 torr and 17◦C. What volume will it fill if the pressure is changed to 730 torr and the temperature is raised to 51◦C?
(p1v1/t1) = (p2v2/t2)
Remember T must be in kelvin
How about ...
P1 = 808 Torr P2 730 Torr
V1= 5.65 L Liters V2 ???? liters
T1= 17-C Celcius T2 80 OC
273 Kelvin 273 K
290 Kelvin 353 K
Pressure Temperature
V2 = V1 (P1/P2) (T1/T2)
V2 = 5.65-L (808/730) (353/290) = 7.6-L
To solve this problem, we can use the combined gas law equation, which relates the initial and final conditions of pressure (P), volume (V), and temperature (T) for a gas.
The combined gas law equation is given as:
(P1 * V1) / (T1) = (P2 * V2) / (T2)
where:
P1 = initial pressure
V1 = initial volume
T1 = initial temperature
P2 = final pressure
V2 = final volume
T2 = final temperature
We have the following information:
P1 = 808 torr
V1 = 5.65 L
T1 = 17°C = 17 + 273.15 = 290.15 K
P2 = 730 torr
T2 = 51°C = 51 + 273.15 = 324.15 K
We need to find V2.
Now let's substitute the values into the combined gas law equation:
(808 torr * 5.65 L) / (290.15 K) = (730 torr * V2) / (324.15 K)
Now we can solve for V2:
V2 = [(808 torr * 5.65 L) / (290.15 K)] * [(324.15 K) / (730 torr)]
V2 ≈ 6.36 L
Therefore, the volume of the gas will be approximately 6.36 L when the pressure is changed to 730 torr and the temperature is raised to 51°C.