Liquid nitrogen has a density of 0.807 g/mL at -195.8 °C.If 1.00 L of N₂(l)is allowed to warm to 25°C at a pressure of 1.0 atm, what volume will the gas occupy? (R = 0.08206 L.atm/K.mol) A)59.1 L B)182 L C)705 L D)1.41 * 10³ L E)1.97 * 10⁴ L

Question

Quizplus · Accepted Answer

Using the combined gas law, we can calculate the final volume of the gas:

(P1V1/T1) = (P2V2/T2)

We know that P1 = P2 = 1.0 atm and T1 = -195.8 °C = 77.4 K. We also know that V1 = 1.00 L and we want to find V2 at 25 °C = 298 K.

Solving for V2:

V2 = (P1V1T2)/(P2T1)

V2 = (1.0 atm)(1.00 L)(298 K)/(1.0 atm)(77.4 K)

V2 = 705 L

Therefore, the best choice is C.

Liquid Nitrogen Has a Density of 0