A 2.50 L sample of neon gas at 0.00 C and 1.00 ATM is compressed into a 1.00 L cylinder. what pressure will the gas exert in the cylinder at 25.0 C?

(P1V1/T1) = (P2V2/T2)

Remember T must be in kelvin.

To solve this problem, we can use the combined gas law which relates the initial and final conditions of a gas sample.

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.

Let's plug in the values given in the problem:

P1 = 1.00 ATM (initial pressure)
V1 = 2.50 L (initial volume)
T1 = 0.00 C + 273.15 = 273.15 K (initial temperature)

V2 = 1.00 L (final volume)
T2 = 25.0 C + 273.15 = 298.15 K (final temperature)

Now we can rearrange the equation to solve for P2 (final pressure):

P2 = (P1 * V1 * T2) / (V2 * T1)

Substituting the values we obtained:

P2 = (1.00 ATM * 2.50 L * 298.15 K) / (1.00 L * 273.15 K)

P2 = 2.749 ATM

Therefore, the gas will exert a pressure of 2.749 ATM in the cylinder at 25.0 C.