a Sapling Learning macmillan learning The picture below shows two bulbs connecte

Question

a Sapling Learning macmillan learning 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 0.650 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 oc After the stopcock is opened the gases mix and react NO No g) O Which gases are present at the end of the experiment? NO O2 NO2 What are the partial pressures of the gases? If the gas was consumed completely, put 0 for the answer. Number Number Number 519 atm 224 atm atm NO NO Previous Give Up & View Solution Try Again Next Exit Explanation

Explanation / Answer

initially,

number of mol of NO,

nNO = P*V / (R*T)

     = 0.650*6.00 / (0.0821*295)

     = 0.161 mol

number of mol of O2,

nO2 = P*V / (R*T)

     = 2.50 *1.50 / (0.0821*295)

     = 0.155 mol

after reaction,

moles of NO2 formed = 0.161 mol

moles of O2 remaining = 0.155/2 =0.0775 mol

Total pressure P.

P*V = n*R*T

P*(6+1.5) = (0.161+0.0775)*0.0821*295

P = 0.77 atm

pO2 = nO2*P/total n

     = 0.0775*0.77/(0.0775+0.161)

     =0.25 atm

pNO2 = P – pO2

       = 0.77-0.25

       = 0.52 atm

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