A cylindrical container of volume 4.0 × 10-3 m 3 contains one mole of hydrogen and two moles of carbon dioxide. Assume the temperature of the mixture is 400 K. The pressure of the mixture of gases is: [Take gas constant as 8.3 J mol -1 K -1 ]

Question

A cylindrical container of volume 4.0 × 10-3 m 3 contains one mole of hydrogen and two moles of carbon dioxide. Assume the temperature of the mixture is 400 K. The pressure of the mixture of gases is: [Take gas constant as 8.3 J mol -1 K -1 ] (A) 249 × 101 Pa (B) 24.9 × 103 Pa (C) 24.9 × 105 Pa (D) 24.9 Pa

Tardigrade Admin · Accepted Answer

V =4 × 10-3 m 3 n =3 moles T =400 K PV = nRT ⇒ P =( nRT / V ) P =(3 × 8.3 × 400/4 × 10-3) =24.9 × 105 Pa

Q. A cylindrical container of volume $4.0 \times 1 0^{- 3} m^{3}$ contains one mole of hydrogen and two moles of carbon dioxide. Assume the temperature of the mixture is $400 K$ . The pressure of the mixture of gases is:
[Take gas constant as $8.3 J m o l^{- 1} K^{- 1}$ ]

$249 \times 1 0^{1} P a$

$24.9 \times 1 0^{3} P a$

$24.9 \times 1 0^{5} P a$

$24.9 P a$

$V = 4 \times 1 0^{- 3} m^{3}$
$n = 3$ moles
$T = 400 K$
$P V = n RT$
$\Rightarrow P = \frac{n RT}{V}$
$P = \frac{3 \times 8.3 \times 400}{4 \times 1 0 ^{- 3}}$
$= 24.9 \times 1 0^{5} P a$

Q. A cylindrical container of volume 4.0×10−3m3 contains one mole of hydrogen and two moles of carbon dioxide. Assume the temperature of the mixture is 400K. The pressure of the mixture of gases is: [Take gas constant as 8.3Jmol−1K−1 ]

249×101Pa

24.9×103Pa

24.9×105Pa

24.9Pa