Under a pressure of 3,000 NM - 2 a gas has a volume of 250 cm square what will be its volume if the pressure is changed to 100mmhg at the same temperature?

To solve this problem, we can use the ideal gas law equation:

PV = nRT

Where:
P = pressure
V = volume
n = number of moles
R = ideal gas constant
T = temperature

Since the number of moles and temperature are constant, we can set up a ratio of the initial pressure and volume to the final pressure and volume:

(P1)(V1) = (P2)(V2)

(3000 N/m^2)(250 cm^3) = (100 mmHg)(V2)

Converting the pressure units to the same unit (N/m^2 = Pa, 1 mmHg = 133.322 Pa):

(3000 N/m^2)(250 cm^3) = (100 mmHg)(V2)
(3000 N/m^2)(250 cm^3) = (100 mmHg)(V2)
(3000 N/m^2)(250 cm^3) = (100 mmHg)(V2)
(3000 N/m^2)(250 cm^3) = (100 mmHg)(V2)

V2 = (3000 N/m^2)(250 cm^3) / (100 mmHg)
V2 = 750000 N·cm / 100 mmHg
V2 = 7500 cm^3

Therefore, the volume of the gas at a pressure of 100 mmHg will be 7500 cm^3.