Question

The pressure within a cylinder with a volume of 14.5L and 25°C is 530 torr. What is the new pressure when it is heated to 80°C and compressed to a volume of 5.7L?

Answer 1

To solve this problem, we can use the combined gas law, which relates the pressure, volume, and temperature of a gas:

P1V1/T1 = P2V2/T2

where P1, V1, and T1 are the initial pressure, volume, and temperature, and P2, V2, and T2 are the final pressure, volume, and temperature.

Substituting the given values into the equation, we get:

P1 = 530 torr

V1 = 14.5 L

T1 = 25°C + 273.15 = 298.15 K

V2 = 5.7 L

T2 = 80°C + 273.15 = 353.15 K

P1V1/T1 = P2V2/T2

530 torr × 14.5 L / 298.15 K = P2 × 5.7 L / 353.15 K

Simplifying the equation, we get:

P2 = (530 torr × 14.5 L × 353.15 K) / (298.15 K × 5.7 L)

P2 = 2929.37 torr

Therefore, the new pressure when the cylinder is heated to 80°C and compressed to a volume of 5.7L is approximately 2929.37 torr.

Step-by-step explanation: