Question

A sample of nitrogen gas inside a sealed container with a volume of 6.0 liters and temperature of 100 K exerts a pressure

of 1.50 atm. What pressure will be exerted by the gas if the volume is decreased to 2.0 liters and the temperature
decreases to 75 K?
A. 3.4 atm
B. 0.22 atm
C. 1.5 atm
D. 3.0 atm

Answer 1

The relationship between pressure, volume, and temperature can be described by the ideal gas law:

PV = nRT

where P is pressure, V is volume, n is the number of moles of gas, R is the gas constant, and T is temperature.

Assuming that the number of moles, n, and the gas constant, R, remain constant, we can use the combined gas law to solve for the final pressure:

(P1V1)/T1 = (P2V2)/T2

Plugging in the given values, we get:

(1.50 atm x 6.0 L)/100 K = (P2 x 2.0 L)/75 K

Solving for P2, we get:

P2 = (1.50 atm x 6.0 L x 75 K)/(2.0 L x 100 K) ≈ 3.4 atm

Therefore, the answer is A. 3.4 atm.