The capacity of a vessel is 3 litre- It contains 6 gm oxygen- 8 gm nitrogen and 5 gm CO 2 mixture at 27- C- If R -8-31 J - mole - - kelvin- then the pressure in the vessel in N - m 2 will be approx-A- 5 - 105B- 5 - 104C- 106D- 105

The correct option is A Dalton’s law P=P_1+P_2+P_3=μ_1RT/V+μ_2RT/V+μ_3RT/V=RT/V[μ_1+μ_2+μ_3]=RT/V [m_1/M_1+m_2/M_2+m_3/M_3 ] =8.31× 300/3× 10^ 3 [ 6/32+8/28 ...

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

Byju's Answer

Standard XII

Physics

Pressure

The capacity ...

Question

The capacity of a vessel is 3 litre. It contains 6 gm oxygen, 8 gm nitrogen and 5 gm $C O_{2}$ mixture at $27^{\circ} C$ . If R = 8.31 J/mole $\times$ ´ kelvin, then the pressure in the vessel in $N / m^{2}$ will be (approx.)

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

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

Open in App

Solution

The correct option is A

Dalton’s law
$P = P_{1} + P_{2} + P_{3} = \frac{μ_{1} R T}{V} + \frac{μ_{2} R T}{V} + \frac{μ_{3} R T}{V} = \frac{R T}{V} [μ_{1} + μ_{2} + μ_{3}] = \frac{R T}{V} [\frac{m_{1}}{M_{1}} + \frac{m_{2}}{M_{2}} + \frac{m_{3}}{M_{3}}]$
= $\frac{8.31 \times 300}{3 \times 10^{- 3}} [\frac{6}{32} + \frac{8}{28} + \frac{5}{44}] = 498 \times 10^{3} ≅ 500 \times 10^{3} ≅ 5 \times 10^{5} N / m^{2}$

Suggest Corrections

Similar questions

Q. One half mole each of nitrogen, oxygen and carbon dioxide are mixed in enclosure of volume

5

litres and temperature

27^{o}

C. The pressure exerted by mixture is

(R = 8.31 J m o l^{- 1} K^{- 1})

A vessel of volume 4 litres contains a mixture of 8gms of O $_{2}$ , 14 gms of N $_{2}$ and 22 gms of CO $_{2}$ at 27 $^{0}$ C. The pressure exerted by the mixture is

Q. For 10 minute each, at

0^{\circ} C

, from two identical holes nitrogen and an unknown gas are leaked into a common vessel of 4 litre capacity. The resulting pressure in the vessel is 2.8 atm and the mixture contains 0.4 mole of nitrogen. What is the molar mass of unknown gas ?

Q. At atmospheric pressure, a litre vessel contains a mixture of Helium and Nitrogen. If partial pressure of Nitrogen is 500 mm, the partial pressure of Helium will be:

Q. A vessel contain a mixture of 7 g of nitrogen and 11 g of carbondioxide at temperature T = 290 k. If pressure of the mixture is 1 atm

(= 1.01 \times 10^{5} N / m^{2})

, calculate its density:

(R = 8.31 J / m o l - K)

Join BYJU'S Learning Program

The capacity of a vessel is 3 litre. It contains 6 gm oxygen, 8 gm nitrogen and 5 gm CO2 mixture at 27∘C. If R = 8.31 J/mole ×´ kelvin, then the pressure in the vessel in N/m2 will be (approx.)

The correct option is A Dalton’s law P=P1+P2+P3=μ1RTV+μ2RTV+μ3RTV=RTV[μ1+μ2+μ3]=RTV[m1M1+m2M2+m3M3] =8.31×3003×10−3[632+828+544]=498×103≅500×103≅5×105N/m2

The capacity of a vessel is 3 litre. It contains 6 gm oxygen, 8 gm nitrogen and 5 gm $C O_{2}$ mixture at $27^{\circ} C$ . If R = 8.31 J/mole $\times$ ´ kelvin, then the pressure in the vessel in $N / m^{2}$ will be (approx.)