# Work Done in Isothermal Reversible Process

## Trending Questions

**Q.**Two moles of an ideal gas initially at 270C and one atmospheric pressure are compressed isothermally and reversibly till the final pressure of the gas is 10 atm. Calculate q for the process.

- 11488 J
- −11488 J
- 12000 J
- −12000 J

**Q.**A given mass of gas expands reversibly from state A to state B by three paths 1, 2 and 3 as shown in the figure. If w1, w2, and w3 respectively are the work done by the gas along three paths, then:

- w1<w2>w3
- w1<w2<w3
- w1>w2>w3
- w1=w2=w3

**Q.**Which of the following is CORRECT regarding work in reversible isothermal compression?

- It is independent of volume of gas.
- It depends on number of moles of gas.
- It is independent of temperature of gas.
- All of the above

**Q.**For the cyclic process in the figure , which of the following is(are) correct :

- wAB=0 and wBC<0
- wBC>0 and wCA>0
- wcyclic>0
- wBC<0 and wCA>0

**Q.**Calculate q (in joules), for the reversible isothermal expansion of one mole of an ideal gas 27oC from a volume of 10 dm3 to a volume of 20 dm3.

- 1729 J
- 1504 J
- 1432 J
- 1830 J

**Q.**

When the total energy change in an isothermal cycle is zero, it represents

a reversible cycle

an adiabatic change

a thermodynamic equilibrium

an irreversible cycle

**Q.**How much work in kJ mol−1 unit is done by reversible and isothermal expansion of 1.2 mole of an ideal gas to 10 times of its original volume at 27oC ?

- 4.191
- 6.892
- −6.892
- −4.191

**Q.**Calculate the work done when 2 moles of hydrogen expand isothermally and reversibly at 25 ∘C from 15 to 45 litres.

- −1309 calories
- −14.36 calories
- −2872 calories
- −28.72 calories

**Q.**Consider an ideal gas that occupies 2.50 dm3 at a pressure of 3 bar. If the gas is compressed isothermally at a constant pressure Pext, so that the final volume becomes 0.5 dm3. Calculate the value of Pext and the work done respectively.

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

**Q.**One mole of an ideal gas at 300 K is expanded isothermally from an initial volume of 1 litre to 10 litres. The value of △U for this process is:

(R=2 cal mol−1K−l)

- 163.7 cal
- zero
- 138.1 cal
- 9 atm L

**Q.**Calculate the heat involved in a reaction for the isothermal expansion of one mole of a ideal gas at 27o C from a volume of 50 L to 100 L.

- Q = 159 J
- Q = 2294 J
- Q = 1729 J
- Q = 2197 J

**Q.**How much work in kJ mol−1 unit is done by reversible and isothermal expansion of 1.2 mole of an ideal gas to 10 times of its original volume at 27oC ?

- 4.191
- 6.892
- −6.892
- −4.191

**Q.**Calculate the magnitude of maximum work done (in J) in expanding 16 g of oxygen at 300 K and occupying a volume of 5 dm3 isothermally untill the volume becomes 25 dm3.

(Given log5=0.6989)

- 2159 J
- 2007 J
- 1055 J
- 2536 J

**Q.**The work done by 2 mole of an ideal gas at 300 K in a reversible isothermal expansion from 10 litres to 20 litres is

- – 3458 J
- + 3458 J
- – 1730 .4 J
- + 1730.4 J

**Q.**Which of the following is CORRECT regarding work in reversible isothermal compression?

- It is independent of volume of gas.
- It depends on number of moles of gas.
- It is independent of temperature of gas.
- All of the above

**Q.**A reversible cyclic process for an ideal gas is shown below. Here, P, V and T are pressure, volume and temperature, respectively. The thermodrynamic parameteres q, w and U are heat, work and internal energy respectively.

The incorect option(s) is(are):

- wAB=−P2(V2−V1)

- wBC=−P2(V2−V1)
- ΔUAB=0, ΔUCA=qCA
- wCA=0

**Q.**The work done by 200 calorie of heat in isothermal expansion of ideal gas is:

- −836.8 J
- −418.4 J
- −555.2 J
- 664.5 J

**Q.**A given mass of gas expands reversibly from state A to state B by three paths 1, 2 and 3 as shown in the figure. If w1, w2, and w3 respectively are the work done by the gas along three paths, then:

- w1<w2>w3
- w1<w2<w3
- w1>w2>w3
- w1=w2=w3

**Q.**Calculate q (in joules), for the reversible isothermal expansion of one mole of an ideal gas 27oC from a volume of 10 dm3 to a volume of 20 dm3.

- 1729 J
- 1504 J
- 1432 J
- 1830 J

**Q.**The work done in erg for the reversible expansion of 1 mole of an ideal gas from a volume of 10 litres to 20 litres at 25oC is

- 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

**Q.**5 moles of an ideal gas at 27∘C expands isothermally and reversibly from a volume of 6 L to 60 L. The work done in kJ is:

- -28.72 kJ
- -32.60 kJ
- 14.28 kJ
- 20.32 kJ

**Q.**Calculate the work done by 10 g of an ideal gas of molecular weight 44 in expanding reversibly and isothermally from a volume of 5 to 10 litre at 300 K.

- 93.93 cal
- −63.63 cal
- −93.93 cal
- 63.63 cal

**Q.**One mole of an Ideal gas was compressed isothermally and reversibly from 22.4×10−3m3 and one atmospheric pressure to 11.2×10−3m3(R=8.314J/K/mol). The work done on the system is

- - 1134 J
- 1134 J
- 1573 J
- Cannot be caluclated

**Q.**An ideal gas is allowed to expand against a constant pressure of 2 bar from 10 L to 50 L in one step. Calculate the magnitude of work done by the gas. If the same expansion were carried out reversibly, will the magnitude work done be higher or lower than the earlier case? (Given that, 1 L bar=100 J)

- 8 kJ, higher
- −8 kJ , higher
- −8 kJ, lower
- 8 kJ, lower

**Q.**A given mass of gas expands from state A to state B by three paths 1, 2 and 3 as shown in the figure below, If w1, w2 and w3 respectively, be the work done by the gas along three paths, then

- w1>w2>w3
- w1<w2<w3
- w1=w2=w3
- w1<w2;w1<w3

**Q.**The plots which does not represent isothermal expansion of an ideal gas is:

- A
- B
- C
- D

**Q.**One mole of an ideal gas is taken from a to b along two paths denoted by the solid and the dashed lines as shown in the graph below. If the work done along the solid line path is Ws and that along the dotted line path is Wd then the integer closest to the ratio WdWs is:

**Q.**

10 mole of ideal gas expands isothermally and reversibly from a pressure of 10 atm to 1 atm at 300 K. What is the heavisest mass which can lifted through a height of 100 meter by this gas?

31842 kg

58.55 kg

342.58 kg

None of these

**Q.**Calculate the magnitude of maximum work done (in kJ) in expanding 6 g of hydrogen at 300 K and occupying a volume of 10 dm3 isothermally untill the volume becomes 30 dm3.

(Given log5=0.6989)

- 7886 J
- 4521 J
- 8221 J
- 1005 J

**Q.**Carbon monoxide is allowed to expand isothermally and reversibly from 10 m3 to 20 m3 at 300 K and work obtained is 4.754 kJ. Calculate the number of moles of carbon monoxide

- 27.5 mol
- 5.5 mol
- 2.75 mol
- 55.0 mol