Work Done in Isothermal Reversible Process
Trending Questions
(R=2 cal mol−1K−l)
- 163.7 cal
- zero
- 138.1 cal
- 9 atm L
![](https://search-static.byjusweb.com/question-images/byjus/ckeditor_assets/pictures/846215/original_Dia_2428829.png)
- T1=T2
- T3>T1
- Wisothermal>Wadiabatic
- ΔUisothemal>ΔUadibatic
- 4.191
- 6.892
- −6.892
- −4.191
- 4.8 K
- 6.6 K
- 1.2 K
- 2.4 K
- q=−w=5.22 kJ and ΔU=0
- q=−w=6.22 kJ and ΔU=0
- w=q=5.22 kJ and ΔU=0
- w=q=ΔU=0
- 2.303×298×0.082 log 2
- −298×107×8.314×2.303 log 2
- −2.303×298×0.082 log 0.5
- 2.303×298×2 log 2
- −418.4 J
- 41.84 J
- −4.184 J
- None of these
- 820.8 cal
- −848.2 cal
- 84.7 cal
- −848.2 kcal
- −1309 calories
- −14.36 calories
- −2872 calories
- −28.72 calories
- −10 kJ
- −2 kJ
- −8 kJ
- −4 kJ
A balloon filled with helium ( and ) bursts. Immediately afterwards the expansion of helium can be considered as:
reversible isothermal
Irreversible isothermal
reversible adiabatic
irreversible adiabatic
- volume and temperature will be higher
- volume will be lower but the final volume will be higher
- volume and temperature will be lower
- temperature will be lower but the final volume will be higher
mol of an ideal gas expands reversibly and isothermally from to at . The heat exchange during the process is near?
- U increases but H decreases
- U and H are unchanged
- H increases but U decreases
- U and H increases
- 14.28 kJ
- 20.32 kJ
- -28.72 kJ
- -32.60 kJ
5.6 litre of helium gas at STP is adiabatically compressed to 0.7 litre. Taking the initial temperature to be T1, the work done on the gas is:
- 98RT1
- 98RT1
- 32RT1
- 158RT1
(Given γ=1.33 and CV=25.08 Jmol−1K−1 For CO2)
- −836.8 J
- −418.4 J
- −555.2 J
- 664.5 J
![](https://search-static.byjusweb.com/question-images/byjus/ckeditor_assets/pictures/863937/original_1.1.png)
- B and D
- A and D
- B and C
- A and C
![](https://search-static.byjusweb.com/question-images/byjus/ckeditor_assets/pictures/842337/original_image_3.png)
- w1<w2>w3
- w1<w2<w3
- w1>w2>w3
- w1=w2=w3
For an ideal gas, the work of reversible expansion under isothermal condition can be calculated by using the expression W=−nRT lnVfVi. A sample containing 1.0 mol of an ideal gas is expanded isothermally and reversible to ten times of its original volume, in two separate experiments. The expansion is carried out at 300 K and at 600 K respectively. Choose the correct option.
(a) Work done at 600 K is 20 times the work done at 300 K
(b) Work done at 300 K is twice the work done at 600 K
(c) Work done at 600 K is twice the work done at 300 K
(d) ΔU = 0 in both cases
- 27.5 mol
- 5.5 mol
- 2.75 mol
- 55.0 mol
- Always negative
- Always 100 calories per degree
- 0
- Always positive
A rigid diatomic ideal gas undergoes an adiabatic process at room temperature. The relation between temperature and volume of this process is constant, then is:
- −8 kJ, lower
- 8 kJ, lower
- 8 kJ, higher
- −8 kJ , higher
Given: 1 bar.L = 100 J
- 20 bar and 1000 J
- 15 bar and 3000 J
- 30 bar and 1500 J
- 10 bar and 3750 J
![](https://search-static.byjusweb.com/question-images/byjus/ckeditor_assets/pictures/867093/original_Untitled-1.png)
(ii) Area CBVfVi represents work done against a constant pressure Pf.
- work (i) = work (ii)
- work (i) > work (ii)
- work (i) < work (ii)
- Cannot be defined
What is reversible isothermal expansion? Give an example.
5 moles of an ideal gas expand isothermally and reversibly from a pressure of 10 atm to 2 atm at 300k. What is the largest mass which can be lifted through a height of 1 meter in this expansion?
- 2041 kg
- 2049 kg
- 2409 kg
- 4129 kg
- +8180 cal
- −8810 cal
- −8180 cal
- +8810 cal