HARD
JEE Main
IMPORTANT
Earn 100

Find the work performed by one mole of a Van der Waals gas, during its isothermal expansion from volume V1 to V2, at a temperature T.

Important Questions on THERMODYNAMICS AND MOLECULAR PHYSICS

HARD
JEE Main
IMPORTANT
Problems in General Physics>Chapter 2 - THERMODYNAMICS AND MOLECULAR PHYSICS>THE FIRST LAW OF THERMODYNAMICS, HEAT CAPACITY>Q 2.58.

One mole of oxygen is expanded from a volume V1=1.00 L to V2=5.0 L, at a constant temperature T=280 K. Calculate:
(a) The increment of the internal energy of the gas:

(b) The amount of the absorbed heat. The gas is assumed to be Van der Wal's gas.

HARD
JEE Main
IMPORTANT
Problems in General Physics>Chapter 2 - THERMODYNAMICS AND MOLECULAR PHYSICS>THE FIRST LAW OF THERMODYNAMICS, HEAT CAPACITY>Q 2.59.

For a Van der Waal's gas, find,
(a) The equation of the adiabatic curve in the variables T, V,
(b) The difference of the molar heat capacities, Cp-CV, as a function of T and V.

HARD
JEE Main
IMPORTANT
Problems in General Physics>Chapter 2 - THERMODYNAMICS AND MOLECULAR PHYSICS>THE FIRST LAW OF THERMODYNAMICS, HEAT CAPACITY>Q 2.60.
Two thermally insulated vessels are interconnected by a tube, equipped with a valve. One vessel, of volume V1=10 l, contains v=2.5 moles of carbon dioxide. The other vessel, of volume V2=100 l, is evacuated. The valve having been opened, the gas adiabatically expanded. Assuming the gas to obey the Van der Waal's equation, find its temperature change accompanying the expansion.
HARD
JEE Main
IMPORTANT
Problems in General Physics>Chapter 2 - THERMODYNAMICS AND MOLECULAR PHYSICS>THE FIRST LAW OF THERMODYNAMICS, HEAT CAPACITY>Q 2.61.
What amount of heat has to be transferred to v=3.0 moles of carbon dioxide, to keep its temperature constant, while it expands into vacuum, from volume V1=5.0 l to V2=10 l ? The gas is assumed to be a Van der Waal's gas.
HARD
JEE Main
IMPORTANT
Problems in General Physics>Chapter 2 - THERMODYNAMICS AND MOLECULAR PHYSICS>KINETIC THEORY OF GASES, BOLTZMANN' S LAW AND MAXWELL'S DISTRIBUTION>Q 2.62.
Modern vacuum pumps permit the pressures down to p=4×10-15 atm, to be reached at room temperatures. Assuming that the gas exhausted is nitrogen, find the number of its molecules, per 1 cm3, and the mean distance between them, at this pressure.
HARD
JEE Main
IMPORTANT
Problems in General Physics>Chapter 2 - THERMODYNAMICS AND MOLECULAR PHYSICS>KINETIC THEORY OF GASES, BOLTZMANN' S LAW AND MAXWELL'S DISTRIBUTION>Q 2.63.
A vessel, of volume V=5.0 l, contains m=1.4 g of nitrogen at a temperature T=1800 K. Find the gas pressure, taking into account that, η=30% of molecules are dissociated into atoms at this temperature.
HARD
JEE Main
IMPORTANT
Problems in General Physics>Chapter 2 - THERMODYNAMICS AND MOLECULAR PHYSICS>KINETIC THEORY OF GASES, BOLTZMANN' S LAW AND MAXWELL'S DISTRIBUTION>Q 2.64.
Under standard conditions, the density of the helium and nitrogen mixture equals ρ=0.60 g l-1. Find the concentration of helium atoms in the given mixture.
HARD
JEE Main
IMPORTANT
Problems in General Physics>Chapter 2 - THERMODYNAMICS AND MOLECULAR PHYSICS>KINETIC THEORY OF GASES, BOLTZMANN' S LAW AND MAXWELL'S DISTRIBUTION>Q 2.65.
A parallel beam of nitrogen molecules moving with velocity v=400 m s-1, impinges on a wall at an angle θ=30° to its normal. The concentration of molecules in the beam n=0.9×1019 cm-3. Find the pressure exerted by the beam on the wall, assuming the molecules to scatter in accordance with the perfectly elastic collision law.