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First Law of thermodynamics

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Previous Nature of heat and work

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Previous Nature of heat and work

Next specific and molar heat capacity

Question#1

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Question#2

The work done during the expansion of a gas from a volume of 4dm³ to 6dm³ against a constant external pressure of 3atm is ( 1L atm = 101.32 J ) [CBSE PMT 2004]

+ 304 J

–304 J

– 6 J

–608 J

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Question#3

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Question#4

Internal energy is [AFMC 2004]

Partly potential and partly kinetic

Totally kinetic

Totally potential

None of these

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Question#5

270 kJ

–900 kJ

–900 J

900 kJ

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Question#6

Heat of combustion of carbon is 110 kJ

Reaction is exothermic

Reaction needs no initiation

All of these are correct

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Question#7

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Question#8

Which of the following is correct regarding the internal energy of a substance [Pb. CET 2002]

It is a state function

It increases with increase in temperature

It can be calculated by experiment

It remains unaffected with change in temperature

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Question#9

One mole of an ideal gas is allowed to expand reversibly and adibatically from a temperature of 27^oC . If the work done during the process is 3 kJ , then final temperature of the gas is (C_V =20 J / K) [Pb. CET 2002]

100 K

150 K

195 K

255 K

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Question#10

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Question#11

Enthalpy (H) is equal to [MH CET 2004]

Internal energy (E)

Product of pressure (P) and volume (V) of gas

Internal energy (E)+PV

Work (W) done by a system

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Question#12

None of these

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Question#13

If gas, at constant temperature and pressure expands then its [MH CET 2003]

Entropy increases and then decreases

Internal energy increases

Internal energy remains the same

Internal energy decreases

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Question#14

Work done during isothermal expansion of one mole of an ideal gas from 10 atom. to 1 atm at 300K is [BHU 2004]

4938.8 J

4138.8 J

5744.1 J

6257.2 J

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Question#15

A system absorb 600J of heat and work equivalent to 300J on its surroundings. The change in internal energy is [Pb. PMT 2004]

300 J

400 J

500 J

600 J

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Question#16

The work done by a system is 8 joule, when 40 joule heat is supplied to it. What is the increase in internal energy of system [BHU 2001]

25 J

30 J

32 J

28 J

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Question#17

0, – 965.84 cal

– 965.84 cal, + 965.84 cal

+ 865.58 cal, – 865.58 cal

– 865.58 cal, – 865.58 cal

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Question#18

One mole of an ideal gas is allowed to expand freely and adiabatically into vacuum until its volume has doubled. A statement which is not true concerning this expression is [Pb. PMT 1998]

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Question#19

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Question#20

8.314 x 273 x (-2)

8.314 x 300 x (-2)

8.314 x 27 x (-2)

8.314 x 300 x (2)

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Question#21

According to Hess’s law, the heat of reaction depends upon [MP PMT 2003]

Initial condition of reactants

Initial and final conditions of reactants

Intermediate path of the reaction

End conditions of reactants

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Question#22

– RT

+ RT

– 3RT

+3RT

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Question#23

Hess law is based on [MH CET 2002]

Law of conservation of mass

Law of conservation of energy

Enthalpy is a state function

None of these

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Question#24

In a closed insulated container, a liquid is stirred with a paddle to increase its temperature. In this process, which of the following is true [CBSE PMT 2002]

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Question#25

-874 kJ

-871.53 kJ

-876.47 kJ

+ 874 kJ

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Question#26

In an adiabatic expansion of an ideal gas [KCET (Med.) 2001; MH CET 2000]

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Question#27

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Question#28

Joule-Thomson expansion is [JIPMER 2000]

Isobaric

Isoenthalpic

Isothermal

None of these

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Question#29

Work done during isothermal expansion of one mole of an ideal gas from 10 atm to 1 atm at 300 K is (Gas constant = 2) [AIIMS 2000]

938.8 cal.

1138.8 cal.

1381.8 cal.

1581.8 cal.

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Question#30

The enthalpy of neutralization of which of the following acids and bases is nearly -13.6 Kcal [Roorkee 1999]

HCN and NaOH

HCl and KOH

HCl and NaOH

HCl and NH4OH

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Question#31

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Question#32

The internal energy of a substance [KCET 1998; AFMC 2001; AIIMS 2001]

Increases with increase in temperature

Decreases with increase in temperature

Can be calculated by the relation E = mc²

Remains unaffected with change in temperature

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Question#33

An ideal gas at constant temperature and pressure expands, then its [BHU 1998]

Internal energy remains same

Internal energy decreases

Internal energy increases

Entropy first increases and then decreases

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Question#34

Hess law of heat summation includes [AFMC 1992]

) Initial reactants only

Initial reactants and final products

Final products only

Intermediates only

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Question#35

Exothermic

Endothermic

One with negligible enthalpy change

Highly spontaneous at ordinary temperature

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Question#36

In a reversible isothermal process, the change in internal energy is

Zero

Positive

Negative

None of these

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Question#37

Which of the following expressions represents the first law of thermodynamics [MP PET 1996, 2000; AFMC 1997; BHU 1999; AMU 2000; KCET (Med.) 2000, 01; CBSE PMT 2000; MP PMT 2002]

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Question#38

The heat Q for a reaction at constant volume is equal to

H_P - H_R

H_R - H_P

E_P - E_R

None of these

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Question#39

The enthalpies of the elements in their standard states are assumed to be

Zero at 298 K

Unit at 298 K

Zero at all temperatures

Zero at 273 K

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Question#40

The law of conservation of energy states that [NCERT 1984]

The internal energy of a system is constant

The heat content of a system is constant

Energy is neither created nor destroyed

There is an equivalence between energy and mass

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Question#41

The work done in ergs for the reversible expansion of one mole of an ideal gas from a volume of 10 liters to 20 litres at 25^oC is [CMC Vellore 1999]

2.303 x 298 x 0.082 log2

298 x 10⁷ x 8.31 x 2.303 log2

2.303 x 298 x 0.082 log0.5

8.31 x 10⁷ x 298 - 2.303 log0.5

2.303 x 298 x 2 log2

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Question#42

. During an isothermal expansion of an ideal gas its [CBSE PMT 1991]

Internal energy increases

Enthalpy decreases

Enthalpy remains unaffected

Enthalpy reduces to zero

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Question#43

Positive

Negative

Zero

None

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Question#44

Hess law is applicable for the determination of heat of [AIIMS 1998; Pb. PET/PMT 1999]

Reaction

Formation

Transition

All of these

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Question#45

None of these

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Question#46

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Question#47

Hess's law of constant heat summation in based on [MP PET 2001]

E = mc²

Conservation of mass

First law of thermodynamics

None of the above

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Question#48

“The resultant heat change in a reaction is the same whether it takes place in one or several stages.” This statement is called [MP PMT/PET 1988; MP PMT 1989]

Lavoisier and Laplace law

Hess's law

Joule's law

Le–chatelier's principle

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Question#49

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Question#50

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Question#51

The law of Lavoisier and Laplace illustrates [KCET 1989]

The principle of conservation of energy

Equivalence of mechanical and thermal energy

The principle of conservation of matter

Equivalence of mechanical and chemical energy

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Question#52

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Question#53

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Question#54

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Question#55

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Question#56

Which of the following is always negative for exothermic reaction?[BCECE 2005]

None of these

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Question#57

The relationship depends on the capacity of the vessel

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Question#58

The first law of thermodynamics is only

The law of conservation of energy

The law of conservation of mass

The law of conservation of momentum

Both (a) and (b)

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Question#59

The thermal energy at constant pressure is called MCDAT2020

Enthalpy

Internal energy

Heat capacity

Work done

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Question#60

An ideal gas at constant temperature and pressure expands, then its [BHU 1998]

Internal energy remains same

Internal energy decreases

Internal energy increases

Entropy first increases and then decreases

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Question#61

Which of the following expressions represents the first law of thermodynamics
[MP PET 1996, 2000; AFMC 1997; BHU 1999; AMU 2000;
KCET (Med.) 2000, 01; CBSE PMT 2000; MP PMT 2002]

ΔE = -q + W

ΔE = q - W

ΔE = q + W

ΔE = -q - W

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Question#62

During an isothermal expansion of an ideal gas its
[CBSE PMT 1991]

Internal energy increases

Enthalpy decreases

Enthalpy remains unaffected

Enthalpy reduces to zero

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Question#63

If ΔH is the change in enthalpy and ΔE the change in internal energy accompanying a gaseous reaction
[KCET 1989; CBSE PMT 1990]

ΔH is always greater than ΔE

ΔH < ΔE only if the number of moles of the products is
greater than the number of the reactants

ΔH is always less than ΔE

ΔH < ΔE only if the number of moles of the products is less than the number of moles of the reactants

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Question#64

For the reaction
N₂ + 3H₂ ? 2NH₃ ;ΔH= ? [Roorkee 2000; CBSE PMT 1991, 2002]

ΔE - RT

ΔE - 2RT

ΔE + RT

ΔE + 2RT

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Question#65

Which is not the correct relation between enthalpy (ΔH) and intrinsic energy (ΔE)
[EAMCET 1992]

ΔH = ΔE + PΔV

ΔH = ΔE + nRT

ΔE = ΔH + PΔV

ΔH = ΔE - PΔV

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Related MCQ's Catrgories

Basic concepts

System, surrounding and boundary

Homogenous and heterogenous thermodynamic systems

intensive and extensive properties

Nature of heat and work

First Law of thermodynamics

specific and molar heat capacity

Spontaneous and non spontaneous process

Exo and endothermic reactions

Heat of reaction

experimental determination of the heat of reaction

laplace and hess's law

born haber cycle

Home/ThermochemistryFirst Law of thermodynamics

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Home/Thermochemistry

First Law of thermodynamics