The picture below shows two bulbs connected by a stopcack. The 7.50-L bulb conta

Question

The picture below shows two bulbs connected by a stopcack. The 7.50-L bulb contains nitric oxide at a pressure of 0.340 atm, and the 2.50-L bulb contains oxygen at a pressure of 0.510 atm No After the stopcock is opened, the gases mix and react to produce nitrogen dioxide. 2NO Considering that the volume remains unchanged during the experiment, how does the total pressure in the bulbs change if the reaction is allowed to go to completion? O There is not enough information to determine how the total pressure wll change. O The total pressure will remain constant O The total pressure will decrease. O The total pressure will increase.

Explanation / Answer

OPtion C

The reaction is

2NO +O2 ------------> 2NO2

moles of NO takne = PV/RT asuming the temperature to be constant

= 7.5L x 0.34 atm /RT

= 2.55 /RT

moles of O2 taken = 2.5/0.51/RT

= 1.275 /RT

2NO +O2 ------------> 2NO2

2.55/Rt 1.275/Rt 0 initial moles

0 0 2.55/RT after reaction

However as the valve is opened , the total volume is increased to 7.5 + 2.5 = 10L

Thus the moles of NO2 (both NO and O2 completely reactd) = P x 10L /RT = 2.55?RT

Thus pressure after reaction = 2.55/10 = 0.255atm

Thus the pressure is decreased

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