You visited us 1 times! Enjoying our articles? Unlock Full Access!

Byju's Answer

Standard X

Chemistry

Mole Concept

Equal masses ...

Question

Equal masses of gaseous $N_{2}, N H_{3}$ and $N_{2} O$ are injected into an evacuated container to produce a total pressure of 3 atm. What is the correct order of partial pressure of these gases?

P_{N_{2}} = P_{N H_{3}} = P_{N_{2} O}

No worries! We‘ve got your back. Try BYJU‘S free classes today!

P_{N_{2}} < P_{N H_{3}} < P_{N_{2} O}

No worries! We‘ve got your back. Try BYJU‘S free classes today!

P_{N H_{3}} < P_{N_{2}} < P_{N_{2} O}

No worries! We‘ve got your back. Try BYJU‘S free classes today!

P_{N_{2} O} < P_{N_{2}} < P_{N H_{3}}

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

Open in App

Solution

The correct option is D $P_{N_{2} O} < P_{N_{2}} < P_{N H_{3}}$
Partial pressure = mole fraction $\times$ total pressure

$P_{N} = \frac{n_{N}}{n_{total}} \times 3 = \frac{[\frac{W_{N}}{M_{N}}]}{n_{t o t a l}} \times 3$

The gas which have higher molar mass, will exert lower partial pressure.

$P_{N H_{3}} > P_{N_{2}} > P_{N_{2} O}$

Suggest Corrections

Similar questions

Q. A container containing ammonia is allowed to decompose and the following equilibrium is established.

2 N H_{3} (g) ⇌ N_{2} (g) + 3 H_{2} (g)

.
Then, the equilibrium constant,

K_{p}

is expressed as:
(Where

p_{N_{2}}

= partial pressure of

N_{2}

and

p_{N H_{3}}

is the partial pressure of

N H_{3}

)

A mixture containing 1.6 g of $O_{2}$ , 1.4 g of $N_{2}$ and 0.4 g of $H e$ occupies a volume of $10 L$ at $27^{\circ} C$ . Calculate the partial pressure of each component of the mixture.

Q. A flask containing 0.50 atm of ammonia contains some solid

N H_{4} H S

which undergoes dissociation according to

N H_{4} H S (s) ⇌ N H_{3} (g) + H_{2} S (g) .

Calculate the pressure of

N H_{3}

and

H_{2} S

at equilibrium

K_{P} = 0.11) .

Also calculate the total pressure.

On a humid summer day, the partial pressure of water in the atmosphere is 18 mm Hg. The barometric pressure on this day is as high as 766 mm Hg, Calculate the partial pressures of nitrogen and oxygen if 78.0% of the dry atmosphere is composed of nitrogen molecules and 21.0% of oxygen? (1% of the dry atmosphere is composed of all other gases)

Q. Moles of

N_{2} = 0.4

and moles of

O_{2} = 0.1

Find

p_{N_{2}}

i.e. partial pressure of

N_{2}

at atmospheric pressure.

Join BYJU'S Learning Program

Equal masses of gaseous N2,NH3 and N2O are injected into an evacuated container to produce a total pressure of 3 atm. What is the correct order of partial pressure of these gases?

The correct option is D PN2O<PN2<PNH3Partial pressure = mole fraction × total pressure PN=nNntotal×3=[WNMN]ntotal×3 The gas which have higher molar mass, will exert lower partial pressure. PNH3>PN2>PN2O

Equal masses of gaseous $N_{2}, N H_{3}$ and $N_{2} O$ are injected into an evacuated container to produce a total pressure of 3 atm. What is the correct order of partial pressure of these gases?