Suppose that a sample of gas occupies 117 mL
of volume at 25�C and a pressure of 289 torr.
What would be the volume if the pressure
were changed to 490 torr at 25�C?
Answer in units of mL
To solve this problem, you can use the combined gas law, which states that the ratios of pressure and volume are equal to the ratio of their initial values. The combined gas law can be written as:
(P1 * V1) / (T1) = (P2 * V2) / (T2)
Where P1 and P2 are the initial and final pressures, V1 and V2 are the initial and final volumes, and T1 and T2 are the initial and final temperatures.
Given:
P1 = 289 torr
V1 = 117 mL
P2 = 490 torr
T1 = T2 = 25°C
Now let's substitute the given values into the formula:
(289 * 117) / (25 + 273) = (490 * V2) / (25 + 273)
Simplifying the equation:
(33813) / (298) = (490 * V2) / (298)
Cross multiplying the equation:
33813 * 298 = 490 * V2
V2 = (33813 * 298) / 490
V2 ≈ 20594.44 mL
Therefore, the volume of the gas would be approximately 20594.44 mL if the pressure were changed to 490 torr at 25°C.