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Chapter 8: Problem 1120

Which of the following is not a thermodynamical function. (A) Enthalpy (B) Work done (C) Gibb's energy (D) Internal energy

Short Answer

Expert verified
The non-thermodynamical function among the given options is (B) Work done, as it depends on the path taken and not solely on the state of the system.

Step by step solution

01

Define Enthalpy

Enthalpy (H) is a state function that describes the total energy of a system, including both its internal energy and the energy associated with its pressure and volume. Mathematically, it is defined as: \[H = U + PV\] where U is the internal energy, P is the pressure, and V is the volume of the system. Since enthalpy is a combination of state functions, it is also a state function.
02

Define Work Done

Work done (W) is not a state function. It refers to the energy transferred to or from a system due to an external force or pressure acting upon it. The work done depends on the path taken during the process and not just the initial and final states of the system. Mathematically, it can be expressed for a reversible process in a closed system as: \[W = -\int_{V_1}^{V_2} PdV\] where V1 and V2 are the initial and final volumes, and P is the pressure. Since work done depends on the path taken, it is not a state function.
03

Define Gibb's Energy

Gibb's energy (G) is a state function that represents the maximum work that a system can perform in a reversible process at constant temperature and pressure. Mathematically, it is defined as: \[G = H - TS\] where H is enthalpy, T is the temperature, and S is the entropy of the system. Since Gibb's energy is a combination of state functions, it is also a state function.
04

Define Internal Energy

Internal energy (U) is a state function that represents the total energy of a system, including the kinetic energy due to the motion of its particles and potential energy due to their interaction. It depends only on the state of the system and not the path taken.
05

Identify the Non-Thermodynamical Function

Based on the definitions provided in Steps 1-4, we can conclude that the option (B) Work done is not a thermodynamical function, as it depends on the path taken and not solely on the state of the system.

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Most popular questions from this chapter

For adiabatic Process which relation is true mentioned below ? \(\gamma=\left\\{\mathrm{C}_{\mathrm{p}} / \mathrm{C}_{\mathrm{v}}\right\\}\) (A) \(\mathrm{p}^{\gamma} \mathrm{V}=\mathrm{Const}\) (B) \(\mathrm{T}^{\gamma} \mathrm{V}=\mathrm{Const}\) (C) TV \(^{\gamma}=\) Const (D) \(\mathrm{TV}^{\gamma-1}=\) Const

Water of volume 2 liter in a container is heated with a coil of $1 \mathrm{kw}\( at \)27^{\circ} \mathrm{C}$. The lid of the container is open and energy dissipates at the rate of \(160(\mathrm{~J} / \mathrm{S}) .\) In how much time temperature will rise from \(27^{\circ} \mathrm{C}\) to $77^{\circ} \mathrm{C}\(. Specific heat of water is \)4.2\\{(\mathrm{KJ}) /(\mathrm{Kg})\\}$ (A) \(7 \mathrm{~min}\) (B) \(6 \min 2 \mathrm{~s}\) (C) \(14 \mathrm{~min}\) (D) \(8 \min 20 \mathrm{~S}\)

One mole of an ideal gas $\left(\mathrm{C}_{\mathrm{p}} / \mathrm{C}_{\mathrm{v}}\right)=\gamma$ at absolute temperature \(\mathrm{T}_{1}\) is adiabatically compressed from an initial pressure \(\mathrm{P}_{1}\) to a final pressure \(\mathrm{P}_{2}\) The resulting temperature \(\mathrm{T}_{2}\) of the gas is given by. (A) $\mathrm{T}_{2}=\mathrm{T}_{1}\left\\{\mathrm{p}_{2} / \mathrm{p}_{1}\right\\}^{\\{\gamma /(\gamma-1)\\}}$ (B) $\mathrm{T}_{2}=\mathrm{T}_{1}\left\\{\mathrm{p}_{2} / \mathrm{p}_{1}\right\\}^{\\{(\gamma-1) / \gamma\\}}$ (C) $\mathrm{T}_{2}=\mathrm{T}_{1}\left\\{\mathrm{p}_{2} / \mathrm{p}_{1}\right\\}^{\gamma}$ (D) $\mathrm{T}_{2}=\mathrm{T}_{1}\left(\mathrm{p}_{2} / \mathrm{p}_{1}\right)^{\gamma-1}$

Work done by \(0.1\) mole of a gas at \(27^{\circ} \mathrm{C}\) to double its volume at constant Pressure is \(\quad\) Cal. $R=2\left\\{(\mathrm{Cal}) /\left(\mathrm{mol}^{\circ} \mathrm{K}\right)\right\\}$ (A) 600 (B) 546 (C) 60 (D) 54

The Volume of air increases by \(5 \%\) in an adiabatic expansion. The percentage decrease in its Pressure will be (A) \(5 \%\) (B) \(6 \%\) (C) \(7 \%\) (D) \(8 \%\)
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