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QUIZ-2

Total questions: 60

Worksheet time: 38mins

Name
Class
Date
1.

One mole of an ideal gas expands against a constant external pressure of 1 atm from a volume of 10L to 30L. Calculate the work done by the gas in Latm.

a)

+20

b)

-20

c)

40

d)

-40

2.

What does Gibbs Free Energy tell us?

a)

How much energy is given off by a reaction.

b)

The tendency of a reaction to become "random"

c)

How spontaneous a reaction is.

3.

What information do we need to perform a calculation of Gibbs Free Energy?

a)

Enthalpy of the reaction.

b)

Entropy of the reaction.

c)

The temperature of the reaction in Kelvin.

d)

All of the above are needed.

4.

Which of the following would most likely lead to a spontaneous reaction.

a)

A high negative enthalpy.

b)

A low negative enthalpy.

c)

A high positive enthalpy.

d)

A low positive enthalpy.

5.

What are the best conditions to lead towards a spontaneous reaction?

a)

high negative enthalpy, high temp, high negative entropy

b)

high positive enthalpy, high temp, high negative entropy

c)

high negative enthalpy, low temp, high positive entropy

d)

high negative enthalpy, high temp, high positive entropy.

6.
Entropy increases from solid, liquid to gas. Why?
a)
Molecular disorder increases
b)
Molecular randomness decreases
c)
Molecules are more energetic
d)
Molecules are more reactive
7.

Which represents a decrease in entropy?

a)

sublimation of CO2

b)

boiling water

c)

condensation of steam on cold glass

d)

NaCl dissolving in water

8.

Which sample has the lowest entropy?

HINT - Look at the phase of each chemical....

a)

1 mole of KNO3(l)

b)

1 mole of KNO3(s)

c)

1 mole of H2O(l)

d)

1 mole of H2O(g)

9.

Which phase change represents a decrease in entropy?

a)

solid to liquid

b)

gas to liquid

c)

liquid to gas

d)

solid to gas

10.

6. The formation ½ A2 + 2 B2 + C --> CAB4 has an enthalpy of formation of -104 kJ and a change in entropy of -60.8 J/K at 30 °C. What is the free energy and spontaneity of the reaction?

a)

-85.6 kJ, spontaneous

b)

-18.3 kJ, not spontaneous

c)

+18.3 kJ, spontaneous

d)

+85.6 kJ, not spontaneous

11.

Predict the signs of ΔH , ΔS and ΔG for the reaction:

Mg(s) --> Mg(g)

a)

Δ H = - , Δ S = + and Δ G = - (all temperature)

b)

Δ H = + , Δ S = + and Δ G = - (At all temperature)

c)

Δ H = + , Δ S = + and Δ G = - (At low temperature)

d)

Δ H = + , Δ S = + and Δ G = - (At high temperature)

12.

Which reaction has the greatest increase in entropy of the system?

A. HCl (g) + NH3 (g) → NH4Cl (s)

B. (NH4)2Cr2O7 (s) → Cr2O3 (s) + N2 (g) + 4H2O (g)

C. CaCO3 (s) → CaO (s) + CO2 (g)

D. I2 (g) → I2 (s)

a)

A

b)

B

c)

C

d)

D

13.

Energy

a)

the capacity for doing work

b)

the heat coming from the sun

c)

the vitamins we get from food

d)

a unit for thermodynamics

14.

Heat Energy

a)

energy possessed within the object

b)

energy transfer from one system to the other

c)

energy resulted from the movement of molecules

d)

energy stored in a body

15.

Enthalpy

a)

A thermodynamic quantity used to describe heat changes taking place at constant pressure.

b)

A thermodynamic quantity used to describe heat conversion into a different form of energy.

c)

A thermodynamic quantity used to describe heat storage on a system.

d)

A thermodynamic quantity used to describe the movement of molecules resulting heat.

16.

The second law of Thermodynamics define

a)

Entropy

b)

Energy

c)

Enthalpy

d)

Heat

17.

_______ is an intensive property

a)

volume

b)

entropy

c)

area

d)

temperature

18.

Isolated system can exchange _____ with its surroundings.

a)

neither matter nor energy

b)

both matter and energy

c)

only matter

d)

only energy

19.

A system in which energy can cross the boundary but mass cannot is:

a)

an isolated system

b)

an open system

c)

a closed system

d)

an ideal system

20.

_____ is the amount of matter a body contains

a)

Gravity

b)

Volume

c)

Weight

d)

Mass

21.

Your enthalpy is +20 and your entropy is +5. Which temperature will give a spontaneous reaction?

a)

0

b)

4

c)

8

22.

Which combination of ΔH and ΔS NEVER has a spontaneous reaction?

a)

+ΔH and +ΔS

b)

+ΔH and -ΔS

c)

-ΔH and -ΔS

d)

-ΔH and +ΔS

23.

At what temperature would a given reaction become spontaneous if ΔH =+119kJ and ΔS=+263J/K.mol

a)

452 K

b)

-2210 K

c)

382 K

d)

-363 K

24.

How do you calculate Enthalpy of a reaction?

a)

a. ΔH = ΔHproducts - ΔHreactants

b)

b.ΔT = q / mC

c)

c. ΔG = ΔH -TΔS

d)

d. E = mc2

25.

 The SI unit of heat and energy is the __________.

a)

a. calorie

b)

b. heat

c)

c. joule

d)

d. watt

26.

What type of reaction is shown in the reaction pathway?

a)

a. endothermic reaction

b)

b. exothermic reaction

c)

c. both exothermic and exothermic

d)

d. none of these

27.

Entropy always increases when

a)

a. enthalpy decreases.

.

b)

b. temperature decreases.

c)

c. temperature increases.

d)

d. volume increases

28.

What is the difference between heat and enthalpy?

a)

a. Heat is always the energy in transit, in which 'crosses' the system boundaries. Whereas Enthalpy refers to initial heat content in a system.

b)

b. Heat is always the energy in transit, in which 'crosses' the system boundaries. Whereas Enthalpy refers to total heat content in a system

c)

c. Heat is sometimes transit in the system boundaries. Whereas Enthalpy refers to total heat content in a systemd

d)

d. Heat is always the energy in transit, in which 'crosses' the system boundaries. Whereas Enthalpy refers to final heat content in a system

29.

Predict the signs of ΔH , ΔS and ΔG for the reaction:

Mg(s) --> Mg(g)

a)

Δ H = - , Δ S = + and Δ G = - (all temperature)

b)

Δ H = + , Δ S = + and Δ G = - (At all temperature)

c)

Δ H = + , Δ S = + and Δ G = - (At low temperature)

d)

Δ H = + , Δ S = + and Δ G = - (At high temperature)

30.

1. Given the following information, calculate ΔG0 for the reaction below at 250C: (K = 0C + 273)

SnCl4(l) + 2 H20(l) → SnO2(S) + 4HCl(g),

ΔH0=133.0 kJ and ΔS0 =401.5 J/K

a)

-252.6 kJ

b)

-13.4 kJ

c)

13.4 kJ

d)

252.6 kJ

31.

Given their standard reduction potentials, which of the species is going to be oxidized?

Cu2+/Cu = 0.34V

Zn2+/Zn = -0.76V

a)

Cu

b)

Zn

c)

CuSO4

d)

ZnSO4

32.

Nernst equation FOR (i) Mg(s) | Mg2+(0.001M) || Al3+(0.0001 M) | Al(s)

a)

ECELL=E0CELL-0.0591/6 log[Mg2+]3/[Al3+]2

b)

ECELL=E0CELL-0.0591/6 log[Al3+]2/[Mg2+]3

c)

ECELL=E0CELL+0.0591/3 log[Mg2+]3/[Al3+]2

d)

ECELL=E0CELL-0.0591/3 log[Mg2+] /[Al3+]

33.

When across a period, the atomic size decreases so the first IE ___________.

a)

increases

b)

decreases

c)

constant

d)

i am not sure

34.

Factors affecting the ionisation energy:

a)

Atomic radius

b)

Effective nuclear charge

c)

Shielding effect

d)

All of the above

35.
Which of the following is true about a sulfur atom and a chlorine atom?
a)
Sulfur is larger and has higher ionization energy.
b)
Sulfur is larger and has lower ionization energy.
c)
Sulfur is smaller and has higher ionization energy.
d)
Sulfur is smaller and has lower ionization energy.
36.

The equation for the first ionisation energy of a sodium atom is:

a)

Na (g) -> Na+ (g) + e-

b)

Na+ (g) -> Na2+ (g) + e-

c)

Na (s) -> Na+ (g) + e-

d)

Na+ (g) + e- -> Na (g)

37.

Which of the following electron configurations gives rise to the largest increase between the second and third ionisation energies?

a)

1s2 2s2 2p2

b)

1s2 2s2 2p6 3s1

c)

1s2 2s2 2p6 3s2

d)

1s2 2s2 2p1

38.

Which electron configuration represents an element with the highest first ionization energy?

a)

2-1

b)

2-2

c)

2-8-1

d)

2-8-2

39.

Where is there a big jump of ionization energy increase for successive ionizations of the element Silicon(Si)?

a)

between 1 and 2

b)

between 6 and 7

c)

between 7 and 8

d)

between 4 and 5

40.

In general ionization energy ____ as you go down a group,

and ____ as you go across the periodic table.

a)

decreases, decreases

b)

decreases, increases

c)

increases, decreases

d)

increases, increases

41.

Which element has the greater ionization energy?

a)

Iodine (I)

b)

Chlorine (Cl)

42.
As you move across the periodic table atoms tend to get smaller because, ______________.
a)
the atoms have more mass.
b)
the atoms have less mass
c)
the atoms have more protons.
d)
the atoms have less electrons.
43.

Which statement correctly and completely identifies a trend?

a)

Atomic radius decreases across a period and increases down a group.

b)

Electronegativity decreases across a period and decreases down a group.

c)

Ionization energy increases across a period and increases down a group.

d)

Ionic radius increases across a period and increases down a group.

44.
Ionization energy is...
a)
the energy required to add an electron to a specific atom
b)
how much energy it takes to remove an electron from an atom
c)
the energy required to shield the outer electrons from the nucleus
d)
a measure of the ability of an atom to attract electrons
45.

What property is being measured in this diagram?

a)

Density

b)

Ionization Energy

c)

Atomic Radius

d)

Atomic Mass

46.

Atomic size generally increases as we move __________.

a)

down a group and from right to left across a period

b)

up a group and from left to right across a period

c)

down a group and from left to right across a period

d)

up a group and from right to left across a period

47.

What is the oxidation state of Fe in Fe2O3 ?

a)

+2

b)

-2

c)

0

d)

+3

48.

What is the oxidation state of Mn in KMnO4 ?

a)

+1

b)

+5

c)

+3

d)

+7

49.

What is the oxidation state of Cr in CrO42- ?

a)

+8

b)

+6

c)

-6

d)

-8

50.
 A lone pair is defined as
a)
A pair of bonding electrons
b)
One non-bonding electron
c)
A pair of non-bonding electrons
d)
A pair of electrons on the central atom
51.

What is the name of this VSEPR shape? (The dark shapes are lone electron pairs)

a)

trigonal planar

b)

tetrahedral

c)

bent

d)

linear

52.
According to VSEPR, molecules adjust their shapes to keep which of the following as far away as possible?
a)
Pairs of valence electrons
b)
Inner shell electrons
c)
Mobile Electrons
d)
Electrons closest to the nucleus
53.

The following species are exception to octet rule EXCEPT

a)

I3 −I_3^{\ -}  

b)

NH4 +NH_4^{\ +}  

c)

XeF4XeF_4  

d)

SF4SF_4  

54.

AB4E is a symbol for molecular shape __________________

a)

linear

b)

T-shaped

c)

seesaw

d)

trigonal bipyramidal

55.
Put these in increasing order:
F, N, B
a)
B < N < F
b)
B < F < N
c)
N < F < B
d)
F < N < B
56.
Choose the set that goes from lowest to highest electronegativity?
a)
Cu, Mg, Sr, Ca
b)
F, Cl, Br, Si
c)
Cs, Rb, Ca, Mg
d)
Zn, Cd, Ag, Cu
57.
 Which of the following generally applies to the noble gases? 
a)
high ionization energy, low electronegativity, high reactivity
b)
high ionization energy, high electronegativity, high reactivity
c)
low ionization energy, low electronegativity, low reactivity
d)
high ionization energy, low electronegativity, low reactivity 
58.

2. Which degradation is not part of ‘external’ corrosion?

a)

Soil corrosion

b)

CO2 corrosion

c)

Atmospheric corrosion

d)

Seawater corrosion

59.

4. What type of cracking is SCC (Stress Corrosion Cracking) ?

a)

Anodic type

b)

Cathodic type

c)

Mechanical damage

60.

Oxidation occurs at ...............................

a)

Anode

b)

Cathode

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