Boyle's law states that for a fixed amount of gas, the volume of the gas at a constant temperature is inversely proportional to the pressure. If a certain gas occupies 9.84 liters at a pressure of 50 centimeters of mercury (cm Hg) what is the approximate pressure when the volume is increased to 12 liters ?

The answer is 41cmHg of pressure.

Step-by-step explanation:

If the volume of the gas is inversely proportional to the pressure that the gas exerts within the defined space that it is in, then for a gas that has a 50cmHg pressure at 9.84 liters of volume, the pressure it will have at 12 liters of volume can be found as Pfinal = (9,84 x 50) / 12 = 41cmHg of pressure for the same gas.

I hope this answer helps

The approximate pressure when the volume is increased to 12 liters is 41 cm Hg

Step-by-step explanation:

As stated in the question, Boyle's law states that for a fixed amount of gas, the volume of the gas at a constant temperature is inversely proportional to the pressure. It could also be stated as "the pressure of a given mass of an ideal gas is inversely proportional to its volume at a constant temperature"

Mathematically, P ∝ (1/V)

This means that,

the pressure of a gas tends to increase as the volume of the container decreases, and also the pressure of a gas tends to decrease as the volume of the container increases.

From the Mathematical expression, P ∝ (1/V).

Hence, P = k(1/V)

Where P is the pressure, V is the volume and k is the proportionality constant

Therefore,

PV = k

We can then write that

P1V1 = P2V2 = P3V3 = ...

Hence, P1V1 = P2V2

Where P1 is the initial pressure of the gas

P2 is the final pressure of the gas

V1 is the initial volume of the gas

and V2 is the final volume of the gas

From the question,

P1 = 50 cm Hg

V1 = 9.84 liters (L)

P2 = ??

V2 = 12 liters (L)

Using the equation, P1V1 = P2V2

50 × 9.84 = P2 × 12

Therefore, P2 = (50 × 9.84)/12

P2 = 492/12

P2 = 41 cm Hg

Hence, the approximate pressure is 41 cm Hg