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chemistry MCQs

11th • Chapter 07

50 Questions TextBook
1

The study of heat changes accompanying a chemical reaction is known as what?

A
Thermodynamics
B
Thermochemistry
C
Calorimetry
D
Kinetics
2

A reaction in which the system gives out heat and its temperature rises is called?

A
Endothermic
B
Spontaneous
C
Exothermic
D
Reversible
3

A process that takes place on its own without any outside assistance is termed as?

A
Non-spontaneous
B
Reversible
C
Equilibrium
D
Spontaneous
4

Which of the following is a state function?

A
Heat (q)
B
Work (w)
C
Enthalpy (H)
D
Path
5

The total of all possible kinds of energies of a system is called its?

A
Enthalpy
B
Kinetic Energy
C
Potential Energy
D
Internal Energy (E)
6

The First Law of Thermodynamics is also known as the law of?

A
Conservation of Mass
B
Constant Proportions
C
Conservation of Energy
D
Thermodynamic Equilibrium
7

For a process at constant volume, the heat absorbed by the system (qv) is equal to?

A
Change in Enthalpy (ΔH)
B
Change in Internal Energy (ΔE)
C
Zero
D
Work done
8

The property of a system called enthalpy (H) is defined as?

A
E - PV
B
E + PV
C
PV / E
D
E + q
9

For a process at constant pressure, the heat of reaction (qp) is equal to?

A
ΔE
B
w
C
ΔH
D
ΔV
10

Standard conditions for thermochemical reactions are defined as?

A
0°C and 1 atm
B
100°C and 1 atm
C
25°C and 1 atm
D
25 K and 1 torr
11

The amount of heat absorbed or evolved when one mole of a compound is formed from its elements is called?

A
Enthalpy of Reaction
B
Enthalpy of Combustion
C
Enthalpy of Formation
D
Enthalpy of Solution
12

What is the standard enthalpy of neutralization for a strong acid and a strong base approximately?

A
-57.4 kJ/mol
B
+57.4 kJ/mol
C
-285.8 kJ/mol
D
+285.8 kJ/mol
13

The amount of heat evolved when one mole of a substance is completely burnt in excess oxygen is known as?

A
Enthalpy of Formation
B
Enthalpy of Atomization
C
Enthalpy of Combustion
D
Lattice Energy
14

Which instrument is typically used for the accurate determination of the enthalpy of combustion?

A
Glass Calorimeter
B
Spectrometer
C
Manometer
D
Bomb Calorimeter
15

Hess's Law states that the overall energy change is independent of the?

A
Reactants
B
Products
C
Route or path taken
D
Temperature
16

The lattice energy of an ionic crystal is the enthalpy of formation of one mole of the ionic compound from?

A
Its elements in standard states
B
Gaseous ions
C
Solid ions
D
Aqueous ions
17

In the Born-Haber cycle for NaCl, what does the term ΔH_at(Na) represent?

A
Ionization energy of Na
B
Electron affinity of Na
C
Heat of atomization of Na
D
Lattice energy of NaCl
18

What is the sign of ΔH for an endothermic reaction?

A
Negative
B
Positive
C
Zero
D
It varies
19

What is the sign of 'q' when heat is absorbed by the system from the surroundings?

A
Negative
B
Positive
C
Zero
D
Depends on work
20

What is the sign of 'w' when work is done by the system?

A
Positive
B
Zero
C
Negative
D
Depends on heat
21

A macroscopic property of a system which has definite values for initial and final states is a?

A
Path function
B
State function
C
Thermodynamic property
D
Physical property
22

The neutralization of a strong acid with a strong base is an example of a?

A
Non-spontaneous process
B
Reversible process
C
Endothermic process
D
Spontaneous process
23

The decomposition of water into hydrogen and oxygen is an example of which type of reaction?

A
Exothermic
B
Endothermic
C
Spontaneous
D
Combustion
24

The SI units for heat changes are usually expressed in?

A
Calorie and Kilocalorie
B
Joule and Kilojoule
C
Erg and Dyne
D
Watt and Horsepower
25

In pressure-volume work, the expression W = -PΔV represents work done by?

A
The surroundings on the system
B
The system on the surroundings
C
An external force
D
A catalyst
26

If ΔV = 0, which statement is true according to the first law of thermodynamics?

A
ΔE = q
B
ΔH = q
C
w = q
D
ΔE = 0
27

For liquids and solids, where volume change is insignificant, which relationship is approximately correct?

A
ΔH > ΔE
B
ΔH < ΔE
C
ΔH ≈ ΔE
D
ΔH = 0
28

The standard enthalpy of formation of an element in its standard state is?

A
Always positive
B
Always negative
C
Taken as zero
D
Measured by calorimeter
29

The standard enthalpy of atomization is the heat absorbed to form one mole of?

A
Gaseous molecules
B
Gaseous ions
C
Gaseous atoms
D
Liquid atoms
30

The dissolution of ammonium chloride in water is an example of a spontaneous process that is?

A
Exothermic
B
Endothermic
C
Isothermal
D
Adiabatic
31

What is the heat capacity 'c' of a system?

A
Heat required to raise temp by 1°C
B
Heat required to raise temp by 1 Kelvin
C
Specific heat per mole
D
Mass times specific heat
32

The reaction C(graphite) + O2(g) -> CO2(g) with ΔH = -393.7 kJ/mol is an example of?

A
Endothermic reaction
B
Heat of formation only
C
Heat of combustion only
D
Both heat of formation and combustion
33

Which law is the Born-Haber cycle a direct application of?

A
First Law of Thermodynamics
B
Second Law of Thermodynamics
C
Hess's Law
D
Avogadro's Law
34

The energy required to convert Na(s) to Na(g) is called?

A
Enthalpy of fusion
B
Enthalpy of vaporization
C
Enthalpy of atomization
D
First ionization energy
35

The energy change when an electron is added to a gaseous atom is called?

A
Ionization energy
B
Lattice energy
C
Electron affinity
D
Bond energy
36

If an endothermic reaction occurs rapidly in the air, the temperature of the surrounding air will?

A
Remain constant
B
Increase
C
Decrease
D
Remain unchanged
37

In endothermic reactions, the heat content of the products is?

A
More than that of reactants
B
Less than that of reactants
C
Equal to that of reactants
D
Zero
38

Calorie is equivalent to?

A
0.4184 J
B
41.84 J
C
4.184 J
D
418.4 J
39

The change in heat energy of a chemical reaction at constant temperature and pressure is called?

A
Enthalpy change
B
Bond energy
C
Heat of sublimation
D
Internal energy change
40

Which statement is contrary to the first law of thermodynamics?

A
Energy can neither be created nor destroyed
B
One form of energy can be transferred into an equivalent amount of other kinds
C
In an adiabatic process, work done is independent of its path
D
Continuous production of mechanical work without an equivalent amount of heat is possible
41

For the reaction NaOH + HCl -> NaCl + H2O, the change in enthalpy is called?

A
Heat of reaction
B
Heat of formation
C
Heat of neutralization
D
Heat of combustion
42

The net heat change in a chemical reaction is the same regardless of the path. This is known as?

A
Henry's law
B
Joule's principle
C
Hess's law
D
Law of conservation of energy
43

Enthalpy of neutralization of all strong acids and strong bases has the same value because?

A
Neutralization forms salt and water
B
Strong acids and bases are ionic
C
They always produce H+ and OH- ions
D
The net change is the combination of H+ and OH- ions to form water
44

Burning of coal, once initiated by a spark, proceeds on its own. This is an example of a?

A
Non-spontaneous process
B
Spontaneous process
C
Reversible process
D
Endothermic process
45

The real or imaginary surface separating the system from its surroundings is called the?

A
Universe
B
Boundary
C
Flask
D
State
46

The formation of ammonia in the Haber's process (N2 + 3H2 -> 2NH3) is an?

A
Endothermic reaction
B
Exothermic reaction
C
Isothermal process
D
Spontaneous reaction at all temperatures
47

What is the value of ΔH for the formation of 1 mole of NO from N2 and O2?

A
+180.51 kJ
B
-180.51 kJ
C
+90.25 kJ
D
-90.25 kJ
48

The equation ΔH = q - PΔV + PΔV is derived by substituting ΔE into which equation?

A
H = E + PV
B
ΔH = ΔE + Δ(PV)
C
ΔE = q + w
D
w = -PΔV
49

To calculate the enthalpy change of a reaction that cannot be measured directly, chemists use?

A
A bomb calorimeter
B
The first law of thermodynamics
C
Hess's Law
D
A glass calorimeter
50

What is the lattice energy of NaCl as calculated in the text's Born-Haber cycle example?

A
-411 kJ/mol
B
+376 kJ/mol
C
-787 kJ/mol
D
+496 kJ/mol