Calculator Periodic Table Question 29 of 29 Mapo Sapling Learning The picture be

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Calculator Periodic Table Question 29 of 29 Mapo Sapling 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 "C After the stopcock is opened the gases mix and react No 2NC ? 2NO Which gases are present at the end of the experiment? NO NO2 What are the partial pressures of the gases? If the gas was consumed completely, put O for the answer Number Number Number atm P,, =110.477 atm Pa0.258 atm No No O Previous ? Give Up & View Solution # Try Again @ Next Exit xplanation

Explanation / Answer

The balanced equation is

2NO(g) + O2(g) ------ 2NO2(g)

Using the ideal gas equation

PV = nRT

number of moles of NO = 0.650 * 6/(0.0821 * 295) = 0.1610 moles

number of moles of O2 = 2.50 * 1.50/(0.0821 * 295) = 0.15483 moles

Now one mole of O2 reacts with 2 moles of NO, hence NO is the limiting reagent

Number of moles of NO left after reaction = 0

Number of moles of O2 left = 0.15483 - 0.1610/2 = 0.07433 moles

Number of moles of NO2 produced =0.1610 moles

Partial pressure of NO2 = 0.1610 x 0.0821 * 295 / 7.50

P = 0.520 atm NO2

Partial pressure of O2 = 0.07433 x 0.0821 * 295 / 7.50

P = 0.2400 atm O2

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