Work done in Isothermal Irreversible Process
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2 litres of an ideal gas at a pressure of 10atm expands isothermally into vacuum until its total volume is 10 litres. How much work is done? How much heat is absorbed? Consider the same expansion but this time the constant external pressure of 1 ATM?
Five moles of an ideal gas at and is expanded into the vacuum to double the volume. The work done is
Zero
- −600 J
- −608 J
- +304 J
- −304 J
- - 1382 cal
- - 1382 J
- - 13.82 cal
- - 1.382 cal
The pressure-volume work for an ideal gas can be calculated by using the expression W=∫VfVipexdV. The work can also be calculated from the pV-plot by using the area under the curve within the specified limits. When an ideal gas is compressed (a) reversibly or (b) irreversibly from volume Vi to Vf. Choose the correct option.
(a) W (reversible) = W (irreversible)
(b) W (reversible) < W (irreversible)
(c) W (reversible) = W (irreversible)
(d) W (reversible) = W (irreversible) +pex.ΔV
- For an isothermal process, q=+w
- For an isochoric process, ΔU=−q
- For an adiabatic process, ΔU=−w
- For a cyclic process, q=−w
-3435 J
3435 J
-3400 J
3400 J
One mole of an ideal gas expands reversibly at a constant temperature of from an initial volume of to a final volume of . What will be the work done in expanding the gas?
One mole of an ideal gas at 25∘C expands in volume from 1.0 L to 4.0 L at constant temperature. What work (in J) is done if the gas expands against vacuum ?
-4.0 X 102
4.0 X 102 J
0 J
- 3.0 X102
- T = 174.8 K, V = 64 L
- T = 165.4 K, V = 78.8 L
- T = 153 K, V = 57 L
- T = 161.2 K, V = 68.3 L
Given: 1 L.atm = 101.3 J
- 17 L.atm
- 10 L.atm
- 2026 J
- −2026 J
(ii) P, V1 to P, 2V1
The work done in the two cases respectively is:
- Zero, Zero
- Zero, −PV1
- −PV1, Zero
- −PV1, −P1V1
- 11.4 kJ
- -11.4 kJ
- 0 kJ
- 4.8 kJ
(Given: 1L.atm=101.3 J)
- −402 J
- −525.3 J
- −810.4 J
- −212.8 J
- Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
- Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
- Assertion is correct but Reason is incorrect
- Assertion is incorrect but Reason is correct
- 685.3 cal
- −848.2 cal
- 422.5 cal
- −240.5 cal
- 140 L atm
- 70 L atm
- 7.0 L atm
- 14.0 L atm
- 2.27 J
- Infinite
- 0 J
- 8.314 KJ
(Take 1Latm≃100J)
- −300 J
- 300 J
- −100 J
- −600 J
5 moles of an ideal gas at 270C expands isothermally and reversibly from a volume of 6L to 60L. The work done in kJ is :
- -14.7
- -28.72
- + 28.72
- - 56.72
(ii) P, V1 to P, 2V1
The work done in the two cases respectively is:
- Zero, Zero
- Zero, −PV1
- −PV1, Zero
- −PV1, −P1V1
(p:pressure, V:volume, T:temperature, H:enthalpy, S:entropy)
- Q = 2294 J
- Q = 2197 J
- Q = 1729 J
- Q = 159 J
- Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
- Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
- Assertion is correct but Reason is incorrect
- Both Assertion and Reason are incorrect
One mole of an ideal gas at 25∘C expands in volume from 1.0 L to 4.0 L at constant temperature. What work (in J) is done if the gas expands against vacuum ?
−4.0 × 102
−3.0 × 102
4.0 × 102 J
0 J
- ΔSsys=ΔSsurr
- ΔSsys=−ΔSsurr
- |ΔSsys|=|ΔSsurr|
- None of these
- More in the isothermal process
- More in the adiabatic process
- Equal in both processes
- Dependent on atomicity of gas
- w3>w1
- w1>w2
- w2>w4
- w4>w2