Name: Factors Affecting the Internal Energy
Uploaded: 2019-07-19
Duration: 3 min 47 s
Description: The internal energy of a thermodynamic system is the energy contained within it. Let's watch the video to learn more about the internal energy of a system.

Question

Match the following:

A		B
(i)	Adiabatic process	(a)	Heat
(ii)	Isolated system	(b)	At constant volume
(iii)	Isothermal change	(c)	First law of thermodynamics
(iv)	Path function	(d)	No exchange of energy and matter
(v)	State function	(e)	No transfer of heat
(vi)	$∆ U = q$	(f)	Constant temperature
(vii)	Law of conservation of energy	(g)	Internal energy
(viii)	Reversible process	(h)	$p_{ext} = 0$
(ix)	Free expansion	(i)	At constant pressure
(x)	$∆ H = q$	(j)	Infinitely slow process which proceeds through a series of equilibrium states.
(xi)	Intensive property	(k)	Entropy
(xii)	Extensive property	(l)	Pressure
		(m)	Specific heat

Accepted Answer

(i)Adiabatic process : (e) No transfer of heat.

A process in which no heat exchange takes place is called adiabatic process.

(ii) Isolated system: (d) No exchange of energy and matter.

A system which cannot undergo exchange of matter or energy with the surroundings.

(iii) Isothermal process: (f) Constant temperature.

A process in which temperature of the system remains constant is isothermal.

(iv) Path function: Heat

A Path function is a function whose value depends on the path followed by the thermodynamic process irrespective of the initial and final states of the process.

(v). State function: (g) Internal energy; (k) Entropy ; (l) Pressure

A state function is a function whose value depends on the final and initial states of the thermodynamic process, irrespective of the path followed by the process.

(vi) $∆ U = q$ : (b)Constant volume

In this case change in internal energy, $∆ U = q$ , where no work is done at constant volume.

(vii) Law of conservation of energy: (c) First law of thermodynamics.

$∆ U = q + w$ is the mathematical statement of the first law of thermodynamics, which states that
the energy of an isolated system is constant. It is commonly stated as the law of conservation of energy.

(viii) Reversible process: (j)

When the difference between driving force and opposing force is very small and the process is carried out infinitesimally slowly, then the process is called reversible process.

(ix) Free expansion: (h)p_ext =0

Expansion of a gas in vacuum is called free expansion. No work is done during free expansion of an ideal gas whether the process is reversible or irreversible.

(x) $∆ H = q$ : (i) At constant pressure

At constant pressure $q$ is also called the heat of reaction or enthalpy of reaction.

(xi) Intensive property: (l) Pressure; (m) Specific heat

An intensive property is a property of matter that does not change as the amount of matter changes.

(xii) Extensive property: (a) heat (g) Internal energy; (k) Entropy

An extensive property is a property that depends on the amount of matter in a sample.

A B

(i) Adiabatic process (e) No transfer of heat.

(ii) Isolated system (d) No exchange of energy and matter.

(iii) Isothermal change (f) Constant temperature.

(iv) Path function (a) Heat

(v) State function
(g)

(k)

(l)

Internal energy

Entropy

Pressure

(vi) $∆ U = q$ (b) At constant volume

(vii) Law of conservation of energy (c) First law of thermodynamics

(viii) Reversible process (j) Infinitely slow process which proceeds through a series of equilibrium states.

(ix) Free expansion (h) $p_{ext} = 0$

(x) $∆ H = q$ (i)
At constant pressure

(xi) Intensive property
(l)

(m)

Pressure

Specific heat

(xii) Extensive property
(a)

(g)

(k)

Heat

Internal energy

Entropy

Reaction		Entropy change
(i)	A liquid vapourises	(a)	$∆ S = 0$
(ii)	The reaction is non-spontaneous at all temperatures and $∆ H$ is positive	(b)	$∆ S = positive$
(iii)	Reversible expansion of an ideal gas	(c)	$∆ S = negative$

$∆$ Parameters				Description
	$∆_{r} H^{-}$	$∆_{r} S^{-}$	$∆_{r} G^{-}$	Description
(i)	$+$	$-$	$+$	(a)	Non-spontaneous at high temperature.
(ii)	$-$	$-$	$+$ (at high T)	(b)	Spontaneous at all temperatures
(iii)	$-$	$+$	$-$	(c)	Non-spontaneous at all temperatures

NCERT Solutions for Chapter: Thermodynamics, Exercise 1: Matching Type

NCERT Chemistry Solutions for Exercise - NCERT Solutions for Chapter: Thermodynamics, Exercise 1: Matching Type

Questions from NCERT Solutions for Chapter: Thermodynamics, Exercise 1: Matching Type with Hints & Solutions

Learn and Prepare for any exam you want !

(i)	Entropy of vapourisation	(a)	decreases
(ii)	$K$ for spontaneous process	(b)	is always positive
(iii)	Crystalline solid state	(c)	lowest entropy
(iv)	$∆ U$ in the adiabatic expansion of ideal gas	(d)	$\frac{△ H_{vap}}{T_{b}}$