Thermodynamics Part 3

The adiabatic relation between volume and temperature of an ideal gas is:

• V^(γ-1) T = constant

• V^(1+γ) T^γ = constant

• V^(1-γ) T^(γ+1) = constant

• V^(1-γ) T^(γ-1) = constant

For an ideal diatomic gas:

• Cv = 20.8 J/mol.K

• Cv = 28.5 J/mol.K

• Cv = 20.8 J/K

• Cv = 25.5 J/K

A diatomic gas, compressed isobarically, did 42 J of work. Which was the amount of heat given to the gas during such process?

• 147 J

• 137 J

• 127 J

• 117 J

The work done by an adiabatic expansion is written as:

• W=( P2V2-P1V1) / (1-γ)

• W=0

• W= (P2V2-P1V1) / ( γ-1)

• W=P2V2ln⁡(P1/P2)

A gaseous mixture consists of 16g of Helium and 16g of Oxygen. The ratio CpCv of the mixture is:

• 1.4

• 1.54

• 1.59

• 1.62

For a diatomic gas, the value of γ = CpCv is:

• 9/7

• 7/5

• 5/3

• 5/7

One mole of a monoatomic ideal gas is mixed with one mole of a diatomic ideal gas. The molar specific heat of the mixture at constant volume is:

• R

• 2R

• 0.5 R

• 4R

A monatomic gas is suddenly compressed to (18)th of its initial volume adiabatically. The ratio of its final pressure to the initial pressure is

• 32

• 8

• 132

• 18

Which of the following statements is correct

• Cp can never be less than Cv

• Cp Cv in some specific cases

• Cp may be less than Cv depending on the gas

• Cp may be equal to or less than Cv

1.80 mol of an ideal gas is taken from a volume of 3.00 m3 to a volume of 1.50 m3 via an isothermal compression at 30oC. How much energy is transferred as heat during the compression?

• - 3140 J

• - 3.14 J

• - 314 J

• - 31.4 J