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20 Physics -- Ideal Gas

Although the r.m.s speed of a gas molecules is of the order of the speed of sound in that gas, yet on opening a bottle of ammonia in one corner of a room, its smell takes time in reaching the other corner, Explain why?

Although the r.m.s speed of a gas molecules is of the order of the speed of sound in that gas, yet on opening a bottle of ammonia in one corner of a room, its smell takes time in reaching the other corner, Explain why?

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The speed of molecules follows directly from measuring the pressure and density-you don’t need to know the size of molecules. In standard kinetic theory collisions with other molecules have always been ignored because the molecules were tiny. Though they aren't. So the molecules are not going in straight line. Thus it takes time for the smell to spread in the room.

More questions on Ideal Gas

The fall in temperature of helium gas initially at 15oC when suddenly expanded to 8 times the original volume isa. 162oCb. 216oCc. 72oCd. 324oC   

What is the differences between real gases and ideal gases? Explain in basis with kinetic theory of gases.

Following are the differences betweenr real gases and ideal gases:

Real Gases Ideal Gases
Real gases follow gas laws under conditions of low pressure and high temperature. Ideal gases follow gas laws under all conditions of temperature and pressure.
They have intermolecular forces of attraction. They have negligible intermolecular force of attraction.
Collision of molecules of real gases are not perfectly elastic. Collisions of molecules of real gases are perfectly elastic.


In equations for ideal gas and thermodynamics , what is the difference between 'R' and 'r' . 

Value of R is a constant for all gases while value of r is a variable for all gases but a constant for a specific gas.

Explanation:

Starting with the Ideal gas equation,PV = nRT.

R in the above equation stands for Universal Gas Constant whose value is a constant 8.314 J/mol-K for all gases.

However, when we put n = M/m where M represents total mass of gas present and m the molar mass of the gas.

The value of R/m = r or r = R/m is defined as the specific gas constant for a gas. Clearly, r is a...

What mass of air exists in a 5 x 6 x 8 m³ room at 20°C? Take the average molecular mass of air to be 28 kg K-1 mol-1.

Mention the postulates of Kinetic theory of a gas and also explain the condition of a gas to behave as an ideal gas.

The postulates of kinetic theory of gas can be found hereState the main postulates for Kinetic theory (askmattrab.com).

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Helium gas occupies a volume of 0.04m^3 at a pressure of 2 x 10^5 Nm^-2 and temperature 300K. Calculate the mass of the helium and root mean square speed of its molecules. [ Relative molecular mass...

The pressure of a gas at -173C temperature is 1 atmosphere, keeping the volume constant, to what temperature should the gas be heated so that its pressure becomes 2 atm?

At Initial state

pi = 1atm

T0=-173oc =100k

vi=v

Finally

Pf= 2 atm

Tf = ?

Vf= v(constant)

By ideal gas law

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V = T/P = constant

Ti/pi= Tf/pf

Tf = Ti*Pf/pi

=100*2/1

= 200k = -73oc



Which has more molecules: a kilogram of hydrogen or a kilogram of oxygen?

A kilogram of hydrogen is having more molecules.

Explanation:
For hydrogen that value is 1.008. For oxygen it’s 16.00. That means however many times you can divide the mass by its molar mass, So for example 1000g (1kg) / 1.008 is approximately992 moles of hydrogen. And 1000g/16.00 is 62.5 moles of Oxygen. Now to put it all together, one mole is equal to 6.02x10^23 molecules so obviously since there are more moles of hydrogen, you would have a significantly larger amount of hydrogen.

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Now at T = 0 K, kinetic energy=0

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Why are gas laws not obeyed at low temperature and high pressure? 

The ideal gas law fails at low temperature and high-pressure becausethe volume occupied by the gas is quite small, so the inter-molecular distance between the molecules decreases.

Write the unit of Universal Gas Constant and give it's physical meaning.

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Shows the relationship between Two Specific Heat Capacity of a Gas .


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