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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?

Mar 10

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Mar 10

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.

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.