Relation between Cp and Cv
Trending Questions
Q. In an isobaric process, the ratio of heat supplied to the system (dq) and work done by the system (dW) for diatomic gas is:
- 5:7
- 1:1
- 7:5
- 7:2
Q. The value of γ on monoatomic, diatomic and triatomic gases is ___, ___ and ___ respectively.
1.33, 1.40, 1.66
1.66, 1.40, 1.33
None of these
2, 1.66, 1.5
Q. Cp is always greater than Cv.
True
False
Q.
In an isobaric process, the ratio of heat supplied to the system (dQ) and work done by the system (dW) for diatomic gas is
7 : 2
7 : 5
5 : 7
1 : 1
Q.
Which of the following relations is true?
Cp = Cv
Cp = Cv = 0
Cp > Cv
Cv > Cp
Q. For hydrogen gas, Cp−Cv = a and for nitrogen gas Cp−Cv = b, then the relation between a and b is:
(where Cp and Cv are specific heats defined per gram)
(where Cp and Cv are specific heats defined per gram)
- a=16b
- a=14b
- b=16a
- a=b
Q. To raise the temperature of 1 mole of a diatomic gas by 1 ∘C at constant pressure, the required amount of heat is 120 cal.
The amount of heat which goes as the internal energy is almost equal to:
The amount of heat which goes as the internal energy is almost equal to:
- 85.7 cal
- 58.8 cal
- 82.5 cal
- 80.2 cal
Q. The thermal dissociation equilibrium of CaCO3(s) is studied under different conditions
CaCO3(s)⇌CaO(s)+CO2(g)
For this equilibrium, the correct statement(s) is/are :
CaCO3(s)⇌CaO(s)+CO2(g)
For this equilibrium, the correct statement(s) is/are :
- ΔH is dependent on T
- K is independent of the initial amount of CaCO3
- K is dependent on the pressure of CO2, at a given T
- ΔH is independent of catalyst, if any
Q. A gas (Cv, m=52R) behaving ideally was allowed to expand reversibly and adiabatically from 1 litre to 32 litre. It's initial temperature was 327oC. The molar enthalpy change (in J mole−1) for the process is
- −1125 R
- −575 R
- −1575 R
- None of these
Q.
A mixture contains 1 mode of helium Cp = 2.5 R, Cv = 1.5 R) and 1 a mole of hydrigen (Cp = 3.5 R, Cv = 2.5 R) Calculate the values of Cp Cv Calculate the values of Cp Cv and γ for the mixture.
