The volume of a gas is 450 mL when its pressure is 1.00 atm. If the temperature of the gas does not change, what is the pressure when its volume is

changed to 2.00 L?

2.25 atm

vhcc

0.225atm

top one

fr

To solve this problem, we can use the ideal gas law equation, which states: PV = nRT, where:

- P is the pressure of the gas
- V is the volume of the gas
- n is the number of moles of the gas
- R is the ideal gas constant
- T is the temperature of the gas in Kelvin

Since we are told that the temperature of the gas does not change, we can assume that T is constant.

Let's start by converting the initial volume from milliliters (mL) to liters (L):
450 mL = 0.450 L

We can rewrite the ideal gas law equation as: P1 * V1 = P2 * V2, where:
- P1 is the initial pressure (1.00 atm)
- V1 is the initial volume (0.450 L)
- P2 is the final pressure (unknown)
- V2 is the final volume (2.00 L)

Now we can solve for P2 by plugging in the known values:
1.00 atm * 0.450 L = P2 * 2.00 L

Next, we isolate P2 by dividing both sides of the equation by 2.00 L:
(1.00 atm * 0.450 L) / 2.00 L = P2

Simplifying the equation:
0.450 atm = P2

Therefore, the pressure (P2) when the volume of the gas is changed to 2.00 L is 0.450 atm.