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

Byju's Answer

Standard XII

Chemistry

Dalton's Law of Partial Pressures

A mixture con...

Question

A mixture contains $56 g$ of nitrogen, $44 g$ of ${C O}_{2}$ and $16 g$ of methane. The total pressure of the mixture is $720$ mm of Hg. The partial pressure of methane is:

Open in App

Solution

$_{n} N_{2} =$ moles of nitrogen $= \frac{56}{28} = 2$ mol (As moles= $\frac{M a s s}{Molar mass})$
$_{n} C O_{2} = \frac{44}{44} = 1$ mol
$_{n} C H_{4} = \frac{16}{16} = 1$ mol

Total pressure= $720 m m$ & we have (Partial pressure) $_{C H_{4}} = Total pressure \times X_{C H_{4}}$
$P_{C H_{4}} = 720 \times (\frac{1}{2 + 1 + 1})$
$= 720 \times \frac{1}{4}$
$= 180 m m$ of $H g$ .

Suggest Corrections

Similar questions

Q. Gaseous mixture of contains

56 g

N_{2},

44 g

{C O}_{2}

and

16 g

{C H}_{4} .

The total pressure of mixture is

720 a t m

H g

The partial pressure of

{C H}_{4}

is:

Q. A gaseous mixture containing equal amount of nitrogen and methane has total pressure

7.86

mm Hg at

300

K. Calculate the partial pressure (in mm Hg) of methane in the mixture.

A mixture contains 16g of oxygen, 28 g of nitrogen and 8g of methane. Total pressure of the mixture is 740 mm. What is the partial pressure of nitrogen in mm?

Q. A mixture contains 16 grams of oxygen, 28 grams of nitrogen and 8 grams of methane. Total pressure of the mixture is 740

m m

. What is the partial pressure of nitrogen in

m m

Q. A gaseous mixture contains 56

g

N_{2}

, 44

g

C O_{2}

and 16

g

C H_{4}

. The total pressure of the mixture is 720

m m

H g

. The partial pressure of

C H_{4}

m m

H g

is:

Join BYJU'S Learning Program

A mixture contains 56g of nitrogen, 44g of CO2 and 16g of methane. The total pressure of the mixture is 720 mm of Hg. The partial pressure of methane is:

nN2= moles of nitrogen=5628=2 mol (As moles= MassMolar mass)nCO2=4444=1 molnCH4=1616=1 molTotal pressure= 720mm & we have (Partial pressure)CH4=Total pressure×XCH4PCH4=720×(12+1+1) =720×14 =180mm of Hg .

A mixture contains $56 g$ of nitrogen, $44 g$ of ${C O}_{2}$ and $16 g$ of methane. The total pressure of the mixture is $720$ mm of Hg. The partial pressure of methane is: