Question

A gas occupies 5.00 L at 1.00 atm pressure. What would the volume be if the pressure were to increase to 4.00 atm, assuming the temperature and number of moles remains constant?

1) 5.00 L
2) 1.25 L
3) 20.0 L
4) 1.00 L

Answer 1

Using Boyle’s Law, which expresses the inverse relationship between pressure and volume for a gas at constant temperature and moles, the volume of a gas that occupies 1)5.00 L at 1.00 atm.

Step-by-step explanation:

To determine the new volume of a gas when pressure changes while the temperature and number of moles remain constant, we apply Boyle’s Law.

Which states that the pressure of a given mass of an ideal gas is inversely proportional to its volume at a constant temperature (P1V1=P2V2).

In this case, the initial conditions are a pressure (P1) of 1.00 atm and a volume (V1) of 5.00 L. When the pressure is increased to (P2) of 4.00 atm, assuming the temperature and the amount of gas remain unchanged, we need to find the new volume (V2).

Using the formula:

P1V1 = P2V2

1.00 atm × 5.00 L = 4.00 atm × V2

Now, solve for V2:

V2 = (1.00 atm × 5.00 L) / 4.00 atm = 1.25 L

Therefore, the new volume of the gas when the pressure increases to 4.00 atm is 1.25 L.