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Standard XII

Chemistry

Work done in Isothermal Irreversible Process

An ideal gas ...

Question

An ideal gas undergoes a reversible isothermal expansion from state $I$ to state $I I$ followed by a reversible adiabatic expansion from state $I I$ to state $I I I$ The correct plot(s) representing the changes from state $I$ to state $I I I$ is(are)
$(p : pressure, V : volume, T : temperature, H : enthalpy, S : entropy)$

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Solution

The correct option is D
$(I) Reversible isothermal - ------------ \to expansion (I I) Reversible adiabatic - ----------- \to expansion (I I I)$
So, the correct option is/are:
Reversible isothermal process is isoenthalpic while reversible adiabatic process is isoentropic.

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Similar questions

Q. The correct figure representing isothermal and adiabatic expansion of an ideal gas from a particular initial state is:

Q. An ideal gas undergoes isothermal process from some initial state

i

to final state

f

. Choose the correct alternatives.

Q. For an ideal gas, an illustration of three different paths

A

(B + C)

and

(D + E)

from an initial state

P_{1}

V_{1}

T_{1}

to a final state

P_{2}

V_{2}

T_{1}

is shown in the given figure.
Path A represents a reversible Isothermal expansion from

P_{1}

V_{1} t o P_{2}, V_{2}

. Path

(B + C)

reperesents a reversible adiabatic expansion

(B)

from

P_{1} V_{1}

T_{1} t o P_{3}

V_{2}

T_{2}

followed by reversible heating the gas at constant volume (C) from

P_{3}

V_{2}

T_{2} t o P_{2}

V_{2}

T_{1}

. Path ?

(D + E)

represents a reversible expansion at constant pressure

P_{1} (D)

from

P_{1}

V_{1}

T_{1}

P_{1}

V_{2}

T_{3}

followed by a reversible cooling at constant volume

V_{2} (E)

from

P_{1}

V_{2}

T_{3} t o P_{2}

V_{2}

T_{1}

What is

q_{r e v}

, for path

(A)

Q. The incorrect figure(s) representing isothermal and adiabatic expansion of an ideal gas from a particular initial state is(are):

For an ideal gas, an illustration of three different paths

A

(B + C)

and

(D + E)

from an initial state

P_{1}

V_{1}

T_{1}

to a final state

P_{2}

V_{2}

T_{1}

is shown in the given figure.
Path

A

represents a reversible Isothermal expansion from

P_{1}

V_{1}

P_{2}, V_{2}

. Path

(B + C)

reperesents a reversible adiabatic expansion

(B)

from

P_{1} V_{1}

T_{1}

P_{3}

V_{2}

T_{2}

followed by reversible heating the gas at constant volume

(C)

from

P_{3}

V_{2}

T_{2}

P_{2}

V_{2}

T_{1}

. Path

(D + E)

represents a reversible expansion at constant pressure

P_{1} (D)

from

P_{1}

V_{1}

T_{1}

P_{1}

V_{2}

T_{3}

followed by a reversible cooling at constant volume

V_{2} (E)

from

P_{1}

V_{2}

T_{3}

P_{2}

V_{2}

T_{1}

. What is

Δ S

for path

(D + E) ?

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An ideal gas undergoes a reversible isothermal expansion from state I to state II followed by a reversible adiabatic expansion from state II to state III The correct plot(s) representing the changes from state I to state III is(are) (p:pressure, V:volume, T:temperature, H:enthalpy, S:entropy)