Map The picture below shows two bulbs connected by a stopcock. The large bulb, w

Question

Map The picture below shows two bulbs connected by a stopcock. The large bulb, with a volume of 6.00 L contains nitric oxide at a pressure of 0.600 atm, and the small bulb, with a volume of 1.50 L, contains oxygen at a pressure of 2.50 atm. The temperature at the beginning and the end of the experiment is 22 C. After the stopcock is opened, the gases mix and react: NO Which gases are present at the end of the experiment? NO 02 ? NO2 What are the partial pressures of the gases? If the gas was consumed completely. put 0 for the answer. Number Number Number Pso, atm atm atm NO

Explanation / Answer

(6.00 L) x (0.600 atm) = 3.60 L·atm of NO

(1.50 L) x (2.50 atm) = 3.75 L·atm of O2

3.60 liter-atmospheres of NO would react completely with 3.60 x (1/2) = 1.80 liter-atmospheres of O2, but there is more O2 present than that, so O2 is in excess and NO is the limiting reactant.
Supposing the reaction goes to completion, at the end of the experiment there will be O2 and NO2 present.

(3.60 L·atm NO) x (2 mol NO2 / 2 mol NO) = 3.60 L·atm NO2

(3.75 L·atm O2 initially) - (1.80 L·atm O2 reacted) = 1.95 L·atm O2 left over

Supposing the volume of the stopcock is negligible:
(3.60 L·atm NO2) / (6.00 L + 1.95 L) = 0.45 atm NO2
(1.95 L·atm O2) / (6.00 L + 1.95 L)    = 0.25atm O2
0 atm NO

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