Match the following (A) Isothermal process (i) q = ∆ U (B) Adiabatic process (ii) W = - P × ΔV (C) Isobaric process (iii) W = ∆ U (D) Isochoric process (iv) W = - nRTln V f V i

A - iv , B - iii , C - ii , D - i

A - iii , B - iv , C - i , D - ii

A - i , B - ii , C - iii , D - iv

A - ii , B - i , C - iv , D - iii

A piston filled with 0.04 mol of an ideal gas expands reversibly from 50.0 mL to 375 mL at a constant temperature of 3 7 . 0 ∘ C . As it does so, it absorbs 208 J of heat. The values of q and w for the process will be (R = 8.314 J/mol K) (ln7.5 = 2.01)

q = + 2 0 8 J , w ⁡ = - 2 0 8 J

q = + 2 0 8 J , w ⁡ = + 2 0 8 J

q = - 2 0 8 J , w ⁡ = - 2 0 8 J

EASY

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The work done by gravity is given by the formula, $Wg = - mg (∆ h)$ . The negative sign shows that the particle is dropping from a height $Δh$ in the direction of gravity.

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Important Questions on Chemical thermodynamics and energetics

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When 2 litre of ideal gas expands isothermally into vacuum to a total volume of

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Write the conditions for maximum work done by the system.

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92 g Na

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An ideal gas undergoes isothermal compression from

5 m^{3}

1 m^{3}

against a constant external pressure of

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. The heat released in this process is

24 J {mol}^{- 1} K^{- 1}

and is used to increase the pressure of

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increases by:

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Five moles of an ideal gas at

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is expanded into vacuum to double the volume. The work done is :

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The qualitative sketches I, II and III given below show the variation of surface tension with molar concentration of three different aqueous solutions of KCl,

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at room temperature. The correct assignment of the sketches is -

Question Image

HARD

Chemistry>Physical Chemistry>Chemical thermodynamics and energetics>Nature of Heat and Work

Match the following

(A)	Isothermal process	(i)	$q = ∆ U$
(B)	Adiabatic process	(ii)	$W = - P \times ΔV$
(C)	Isobaric process	(iii)	$W = ∆ U$
(D)	Isochoric process	(iv)	$W = - nRTln (\frac{V_{f}}{V_{i}})$

MEDIUM

Chemistry>Physical Chemistry>Chemical thermodynamics and energetics>Nature of Heat and Work

A piston filled with 0.04 mol of an ideal gas expands reversibly from 50.0 mL to 375 mL at a constant temperature of

37 . 0^{\circ} C

. As it does so, it absorbs 208 J of heat. The values of q and w for the process will be
(R = 8.314 J/mol K) (ln7.5 = 2.01)

MEDIUM

Chemistry>Physical Chemistry>Chemical thermodynamics and energetics>Nature of Heat and Work

The correct option for free expansion of an ideal gas under adiabatic condition is

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Chemistry>Physical Chemistry>Chemical thermodynamics and energetics>Nature of Heat and Work

A gas can expand from

100 mL

250 mL

under a constant pressure of

2 atm

. The work done by gas is

MEDIUM

Chemistry>Physical Chemistry>Chemical thermodynamics and energetics>Nature of Heat and Work

The combination of plots which does not represent isothermal expansion of an ideal gas is

$(A)$ Question Image

$(B)$

$(C)$

$(D)$

EASY

Chemistry>Physical Chemistry>Chemical thermodynamics and energetics>Nature of Heat and Work

Calculate the work done during compression of

2

mol of an ideal gas from a volume of

1 m^{3}

10

{dm}^{3}

300 K

against a pressure of

100 kPa

HARD

Chemistry>Physical Chemistry>Chemical thermodynamics and energetics>Nature of Heat and Work

A reversible cyclic process for an ideal gas is shown below. Here,

P, V, a n d T

are pressure, volume and temperature, respectively. The thermodynamic parameters

q, w, H a n d U

are heat, work, enthalpy and internal energy, respectively.

Question Image

The correct option(s) is (are)

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Chemistry>Physical Chemistry>Chemical thermodynamics and energetics>Nature of Heat and Work

A piece of ice falls from a height

h

so that it melts completely. Only one-quarter of the heat produced is absorbed by the ice and all energy of ice gets converted into heat during its fall. The value of

h

is:
(Latent heat of ice is

3.4 \times 10^{5} {J kg}^{- 1}

and

g = 10 {N kg}^{- 1}

)

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Chemistry>Physical Chemistry>Chemical thermodynamics and energetics>Nature of Heat and Work

The above

P - V

diagram represents the thermodynamic cycle of an engine, operating with an ideal mono-atomic gas. The amount of heat, extracted from the source in a single cycle, is:

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Chemistry>Physical Chemistry>Chemical thermodynamics and energetics>Nature of Heat and Work

The work done during combustion of

9 \times 10^{- 2}

kg

of ethane,

C_{2} H_{6} (g)

300 K

is (Given

R = 8 .314 {JK}^{- 1} {mol}^{- 1}

, atomic mass

C = 12, H = 1

)

MEDIUM

Chemistry>Physical Chemistry>Chemical thermodynamics and energetics>Nature of Heat and Work

A system consisting of 1 mol of an ideal gas undergoes a reversible process,

A \to B \to C \to A

(schematically indicated in the figure below). If the temperature at the starting point A is 300 K and the work done in the process

B \to C

is 1 L atm, the heat exchanged in the entire process in L atm is

Question Image

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Chemistry>Physical Chemistry>Chemical thermodynamics and energetics>Nature of Heat and Work

Calculation the maximum work done in expanding

16 g

of oxygen at

300 K

and occupying a volume of

5 {dm}^{3}

isothermally until volume becomes

25 {dm}^{3}

EASY

Chemistry>Physical Chemistry>Chemical thermodynamics and energetics>Nature of Heat and Work

An ideal gas is allowed to expand from

1 L

10 L

against a constant external pressure of

1

bar. The work done in

k J

is:

MEDIUM

Chemistry>Physical Chemistry>Chemical thermodynamics and energetics>Nature of Heat and Work

A gas is allowed to expand in a well-insulated container against a constant external pressure of

2.5 atm

from an initial volume of

2.50 L

to a final volume of

4.50 L .

The change in internal energy

ΔU

of the gas in joules will be

The work done by gravity is given by the formula, Wg=-mg(∆h). The negative sign shows that the particle is dropping from a height Δh in the direction of gravity.

Important Questions on Chemical thermodynamics and energetics

Learn and Prepare for any exam you want !

The work done by gravity is given by the formula, $Wg = - mg (∆ h)$ . The negative sign shows that the particle is dropping from a height $Δh$ in the direction of gravity.