A cylinder of volume V contains N molecules of a classical monatomic ideal gas a

Question

A cylinder of volume V contains N molecules of a classical monatomic ideal gas at temperature T. What is total average kinetic energy of this gas? What is the pressure of this gas? The gas now expands to twice its volume at constant temperature T. What is the change in total average kinetic energy of this gas? How much work is done on the piston as the gas expands to twice its volume at constant temperature T? How much heat energy must have flowed into the gas as it expands to twice its volume at constant temperature T? Now suppose that the gas had been expanded by only a very small amount, from V to V + delta V, but with no heat allowed into the gas. Because the gas does work on the piston its energy and its temperature drops from T to T- delta T What is the value of delta T/T units of delta V/V?

Explanation / Answer

volume of the gas v

temperature of the gas T

no of molecules is N

a)

total average K.E=3/2*K*T

here, K is Boltzmann constant

b)

Pressure P=1/3*(M/V)*(Vrms)^2

here, M is total mass of the gas

c)

total average K.E=3/2*K*T

d)

use,

W=n*R*T*ln(V2/V1)

here,

n is no of mole of the gas

R is the universal gas constant

but

V2=2*v1

===>

W=n*R*T*ln(2*V1/V1)

W=0.69*n*R*T

Related Questions

Navigate

• Browse (All)
• Browse A
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.