Byju's Answer

Standard XII

Chemistry

Gay Lussac's Law, Avagadro's Law

0.5 moles of ...

Question

0.5 moles of gas A and x moles of gas B exert a pressure of $200 P a$ in a container of volume $10 m^{3}$ at $1000 K$ .
Given R is the gas constant in $J K^{- 1} m o l^{- 1},$ x is:

\frac{2 R}{4 + 12}

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

\frac{2 R}{4 - R}

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

\frac{4 - R}{2 R}

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

\frac{4 + R}{2 R}

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

Open in App

Solution

The correct option is C $\frac{4 - R}{2 R}$
Total mole, $n_{T} = (0.5 + x)$
Ideal gas equation, $P V = n R T$
$200 \times 10 = (0.5 + x) \times R \times 1000$
$2 = (0.5 + x) R$
$\frac{2}{R} = \frac{1}{2} + x$
$\frac{4}{R} - 1 = 2 x$
$\frac{4 - R}{2 R} = x$
or, $x = \frac{4 - R}{2 R}$

Suggest Corrections

Similar questions

0.5

moles of gas

A

and

x

moles of gas

B

exert a pressure of

200 P a

in a container of volume

10 m^{3}

1000 K

. Given

R

is the gas constant in

J K^{- 1} m o l^{- 1}

, then

x

is:

Q. 1.25 moles of a gas A and y moles of a gas B exert a pressure of 300 Pa in a container of volume

10 m^{3}

1000 K

. Find the value of y in terms of R (where R is the gas constant in

J K^{- 1} m o l^{- 1}

)

0.5

moles of gas

A

and

X

moles of gas

B

exert a pressure of

200 P a

in a container of volume

10 m^{3}

1000 K

. Given

R

is the gas constant having the units

J K^{-} 1 m o l^{-} 1

X

is :

4.0 g of a gas occupies 22.4L at NTP. The specific heat capacity of the gas at constant volume is 5.0 JK-1mol-1. If the speed of sound in the gas at NTP is 952 ms-1, then the heat capacity at constant pressure is.

(Take gas constant R=8.3 JK-1mol-1)

Q. One mole of an ideal gas at

22.4 L

is expanded isothermally and reversibly at

300 K

to a volume of

224 L

at a constant pressure. Calculate the

Δ G

kJ

. (Given,

R = 8.314 {J K}^{- 1} {mol}^{- 1}

Join BYJU'S Learning Program

Select...

0.5 moles of gas A and x moles of gas B exert a pressure of 200Pa in a container of volume 10 m3 at 1000 K. Given R is the gas constant in JK−1 mol−1, x is:

The correct option is C 4−R2RTotal mole, nT=(0.5+x) Ideal gas equation, PV=nRT 200×10=(0.5+x)×R×1000 2=(0.5+x)R 2R=12+x 4R−1=2x 4−R2R=x or, x=4−R2R

0.5 moles of gas A and x moles of gas B exert a pressure of $200 P a$ in a container of volume $10 m^{3}$ at $1000 K$ .
Given R is the gas constant in $J K^{- 1} m o l^{- 1},$ x is:

The correct option is C $\frac{4 - R}{2 R}$
Total mole, $n_{T} = (0.5 + x)$
Ideal gas equation, $P V = n R T$
$200 \times 10 = (0.5 + x) \times R \times 1000$
$2 = (0.5 + x) R$
$\frac{2}{R} = \frac{1}{2} + x$
$\frac{4}{R} - 1 = 2 x$
$\frac{4 - R}{2 R} = x$
or, $x = \frac{4 - R}{2 R}$