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The State of a Gas

The energy ta...

Question

The energy taken by system is $δ Q$ , work done by system is $δ W$ and increase in internal energy is $d U$ , the quantity which does not depend on path is :

A

d U

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B

δ Q

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C

δ Q

&

δ W

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D

δ W

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Solution

The correct option is A $d U$
Internal energy is a state function which means it is independent of the path undertaken.

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Similar questions

Q. Match the thermodynamic processes taking place in a system with the correct conditions.
In the table,

Δ Q

is the heat supplied,

Δ W

is the work done and

Δ U

is the change in internal energy of the system.

Process	Condition
(i) Adiabatic	(A) $Δ W = 0$
(ii) Isothermal	(B) $Δ Q = 0$
(iii) Isochoric	(C) $Δ U \neq 0$ , $Δ W \neq 0$ , $Δ Q \neq 0$
(iv) Isobaric	(D) $Δ U = 0$

Δ U_{1}

Δ U_{2}

be the change in internal energy in process A and B respectively,

Δ Q

be the net heat given to the system in process (A+B) and

Δ W

be the net work done by the system in the process (A+ B).
i)

Δ U_{1} + Δ U_{2} = 0

Δ U_{1} - Δ U_{2} = 0

Δ Q + Δ W = 0

Δ Q + Δ W = 0

Q. Refer to figure. Let ∆U₁ and ∆U₂ be the change in internal energy in processes A and B respectively, ∆Q be the net heat given to the system in process A + B and ∆W be the net work done by the system in the process A + B.

(a) ∆U₁ + ∆U₂ = 0.
(b) ∆U₁ − ∆U₂ = 0.
(c) ∆Q − ∆W = 0.
(d) ∆Q + ∆W = 0

Q. The figures given below show different processes (relating pressure

P

V

) for a given amount for an ideal gas.

Δ W

is work done by the gas and

Δ Q

is heat absorbed by the gas.

\begin{matrix} Column I & Column II 1. In Fig (i) & (p) Δ Q > 0 2. In Fig (i i) & (q) Δ W < 0 3. In Fig (i i i) & (r) Δ Q < 0 4. In Fig (i v) & (s) Δ W > 0 \end{matrix}

Q. An ideal gas undergoes the process

1 ⟶ 2

as shown in the figure, the heat supplied and work done in process is

Δ Q

Δ W

respectively. the ratio

Δ Q : Δ W

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