37.9 liters of NO at 725 torr and 146°C are decomposed by the reaction 2 NO → N₂ + O₂.What volume of nitrogen,measured at 755 torr and 22.0°C,will be produced?

Question

Quizplus · Accepted Answer

We can use the combined gas law to solve this problem:

(P1V1/T1) = (P2V2/T2)

We need to find the volume (V2) of nitrogen produced, which means we are solving for V2. We are given:

P1 = 725 torr (pressure of NO)
V1 = 37.9 L (volume of NO)
T1 = 146°C = 419 K (temperature of NO)
P2 = 755 torr (pressure of N2)
T2 = 22.0°C = 295 K (temperature of N2)

We can solve for V2 by plugging in the values:

(725 torr)(37.9 L)/(419 K) = (755 torr)(V2)/(295 K)

Solving for V2 gives:

V2 = (725 torr)(37.9 L)(295 K)/(755 torr)(419 K) = 12.8 L

Therefore, the answer is C.

379 Liters of NO at 725 Torr and 146°C Are