Heat Capacity
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Two ideal polyatomic gases at temperatures and are mixed so that there is no loss of energy. If and , and , and be the degrees of freedom, masses, the number of molecules of the first and second gas respectively, the temperature of the mixture of these two gases is:
Gas at a pressure P0, in contained is a vessel. If the masses of all the molecules are halved and their speeds are doubled, the resulting pressure P will be equal to
4P0
2P0
P0
P02
What will be the amount of mercury, if the specific heat capacity of mercury is and heat capacity is ?
- 2.3 J
- 46 J
- 8.67 × 103 J
- 1.25 × 103 J
- 1.66
- 1.4
- 1.33
- 1.8
- γ−1γ
- γ
- γγ−1
- 1
Consider a gas with density ρ and ¯c as the root mean square velocity of its molecules contained in a volume. If the system moves as whole with velocity v, then the pressure exerted by the gas is
13ρ¯c2
13ρ(c+v)2
13ρ(¯c−v)2
13ρ(c−2−v)2
- 2α+5
- 5α+2
- 1+2α+5
- 1+5α+2
Given (γ=7/5)
- 30 cal
- 50 cal
- 70 cal
- 90 cal
- 500 K
- 833 K
- 300 K
- 0 K
- 1.6R
- 2.1R
- 6.25R
- 3.6R
- 1.96×10−9 sec−1
- 1.29×10−7 sec−1
- 1.69×10−10 sec−1
- 1.69×10−9 sec−1
- 19R6
- 17R6
- 15R6
- 3R2
- 2/5
- 3/5
- 3/7
- 3/4
- 3R/2
- 13R/6
- 5R/2
- 2R
- 1
- 2
- 3
- 4
- 5R2
- 3R2
- 7R2
- 9R2
The value of Cv for one mole of neon gas is
12R
32R
52R
72R
- 2R
- 1.5R
- R
- 2.5R
Gas at a pressure P0, in contained is a vessel. If the masses of all the molecules are halved and their speeds are doubled, the resulting pressure P will be equal to
4P0
2P0
P0
P02
molecules of gas are
- diatomic
- monoatomic
- triatomic
- polyatomic
- Molar heat capacity at no exchange condition, CA=0
- Molar heat capacity at constant temperature, CT→∞
- Molar heat capacity at constant pressure, Cp=γRγ−1
- Molar heat capacity at constant volume, Cv=Rγ
(Assume R=8 J/mol K)
- 525 K
- 550 K
- 600 K
- 625 K
- nB=4 moles
- nB=2 moles
- nB=7 moles
- nB=10 moles
Molar specific heat at constant volume Cv for a monoatomic gas is
32R
52R
3R
2R
- 2 p
- 75 p
- 2.63 p
- p
- 2R
- 1.5R
- R
- 2.5R
- 1.66
- 1.4
- 1.33
- 1.8