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Engineering Chemistry 1&2

Total questions: 75

Worksheet time: 49mins

Name
Class
Date
1.

Phase rule is introduced by

a)

Einstein

b)

Willard Gibbs

c)

CV Raman

d)

Aristotle

2.

An example for one component system is------ system

a)

water

b)

CaCO3

c)

NH4Cl

d)

Sulphur

3.

When ice is converted in to water, it requires-------

a)

temp

b)

pressure

c)

component

d)

medium

4.

If ice is directly converted in to water vapour, then the process is called

a)

freezing

b)

boiling

c)

sublimation

d)

vapourization

5.

If water is converted in to water vapour, then the process is called-------

a)

sublimation

b)

boiling

c)

freezing

d)

cooling

6.

The mathematical expression for Phase rule is

a)

F=C-P+2

b)

F=C+P+2

c)

P=F-P+2

d)

C=P-F+2

7.

2.A phase diagram shows the relationship between

a)

pressure, volume, and the three phases of matter

b)

temperature, pressure, and the three phases of matter

c)

temperature, volume, and the three phases of matter

d)

Non of the above

8.

4. How many components are present in the following systems?           

KCl + Water  →\rightarrow      KCl hydrate

a)

a) 3

b)

b) 2

c)

c) 1

d)

d) 4

9.

5. How many phases are present in following systems :

a mixture of N2, H2 and O2.

a)

a) 2, 2 , 1

b)

b) 1, 1 ,3

c)

c) 1, 1, 1

d)

d) 2, 2, 3

10.

6. What is meant by triple point ?

a)

Three phases are in equilibrium

b)

Three components are in equilibrium

c)

Degree of freedom is three

d)

Non of the above

11.

7.What is meant by invariant point ?

a)

Degree of freedom is zero

b)

Number of component is zero

c)

Number of phases is zero

d)

Non of the above

12.

↔\leftrightarrow  10. Determine the number of phases, components and number of degrees of freedom for the following systems : (i) N2(g) + O2(g)  ↔\leftrightarrow   2NO(g)

a)

a) p= 1, F =3

b)

b)P= 1, F =1

c)

c) p= 3, F =2

d)

d) p= 2, F =3

13.

A system containing liquid water and water vapour has the number of phases equal to

a)

2

b)

0

c)

1

d)

3

14.

A mixture of O2, N2 and CO2 is------ phase system

a)

1

b)

2

c)

3

d)

4

15.

A mixture of two miscible liquids has the number of phases equal to

a)

0

b)

1

c)

2

d)

3

16.

A mixture of two immiscible liquids constitutes a system having the number of phases equal to

a)

0

b)

1

c)

2

d)

3

17.

Decomposition of calcium carbonate represented by the equation CaCO3 (s) ----> CaO(s) + CO2(g) in a closed vessel constitutes a system with number of phases equal to

a)

0

b)

1

c)

2

d)

3

18.

The Gibbs phase rule equation is

a)

F+P = C+2

b)

F-P= C+2

c)

F+P=C+2

d)

F-C=P-2

19.

For one component system the phase rule is

a)

F=3-P

b)

F=2-P

c)

F=1-P

d)

F=4-P

20.

For one phase and one component system, the degrees of freedom is

a)

1

b)

2

c)

3

d)

4

21.

What letter on the diagram represents a gas?

a)

A

b)

B

c)

C

d)

D

22.

What letter on the diagram represents a liquid?

a)

A

b)

B

c)

C

d)

D

23.

What letter on the diagram represents the triple point?

a)

A

b)

B

c)

C

d)

D

24.

What is the melting point of this substance at 1 ATM of pressure?

a)

40

b)

60

c)

100

d)

110

25.

What is the boiling point of this substance at 1 ATM of pressure?

a)

40

b)

60

c)

100

d)

110

26.

What would the state of this substance be at 0.5 ATM of pressure at a 100 degrees Celsius?

a)

Solid

b)

Liquid

c)

Gas

d)

Michigan

27.

What would the state of this substance be at 1 ATM of pressure at a 80 degrees Celsius?

a)

Solid

b)

Liquid

c)

Gas

d)

Michigan

28.

The average atmospheric pressure in Michigan is close to 1 ATM. What state would this substance be in if it was a nice summer day with a temperature of 80 o F (27 o C)?

a)

Solid

b)

Liquid

c)

Gas

d)

Michigan

29.
Water exists as a _____________ at 700 mmHg and 50 °C.
a)
solid
b)
liquid
c)
gas
d)
supercritical fluid
30.
What phase change(s) may occur at pressures below 4.58 mmHg?
a)
sublimation/deposition
b)
melting/freezing
c)
all phase changes are possible at these pressures
d)
vaporization/condensation
31.
The pressure is increased on a sample of water at 0 °C from 0 mmHg to 800 mmHg.  In order, what changes occur?
a)
deposition, melting
b)
sublimation, melting
c)
condensation, freezing
d)
deposition, freezing
32.
What is true regarding CO2 for temperatures above 31 °C?
a)
It can never be liquified.
b)
It decomposes.
c)
It has a high pressure.
d)
It is a plasma.
33.
At 10 atm, dry ice is heated from -100 °C to 30 °C.  What changes occur?
a)
freezing, then condensation
b)
melting only
c)
sublimation only
d)
melting, then boiling
34.
What state of matter is X?
a)
solid 
b)
liquid
c)
gas
d)
supercritical fluid
35.
What change occurs from F to E?
a)
sublimation
b)
deposition
c)
melting
d)
condensation
36.
What change occurs from C to D?
a)
condensation
b)
vaporization
c)
melting
d)
sublimation
37.
What is the normal boiling point of this substance?
a)
150 °C
b)
100 °C
c)
-50 °C
d)
0 °C
38.
What is the normal melting point of this substance?
a)
150 °C
b)
100 °C
c)
-50 °C
d)
0 °C
39.
Water exists as a _____________ at 3 mmHg and 50 °C.
a)
solid
b)
liquid
c)
gas
d)
supercritical fluid
40.
Which statement is true for carbon dioxide at -60 °C?
a)
All three phases are possible.
b)
It can exist as a solid or a gas, depending on pressure.
c)
It is a solid.
d)
With enough pressure it can be melted.
41.

What line segment represents only the solid state? (Diagram F)

a)

A-B

b)

B-C

c)

C-D

d)

D-E

42.

A substance's heating curve is shown in the graph. What is its boiling point? (Diagram B)

a)

100 C

b)

60 C

c)

80 C

d)

20 C

43.

-------------is the indicator used in EDTA method

a)

EAR

b)

EBT

c)

ESR

d)

Methyl Orange

44.

Chlorides and Sulphates causes -------------type of hardness

a)

Temporary Hardness

b)

Permanent Hardness

45.

Hard water is unfit for use in boilers for generating steam because

a)

a) Its boiling point is higher

b)

b) Steam is generated at higher temperature

c)

c) Water decomposes into O2 and H2

d)

d) It produces scales inside the boiler

46.

Calgon is a trade name given to

a)

a) Sodium silicate

b)

b) sodium hexameta phosphate

c)

c) Sodium meta phosphate

d)

d)

calcium phosphate

47.

Disinfection by ozone is due to liberation of

a)

a)Na3PO4

b)

b)Nascent Oxygen

c)

C)Mg3 (PO4)2

d)

d)H3PO4

48.

Tanin, Lignin are used for

a)

a) Phosphate conditioning

b)

b) carbonate conditioning

c)

Collidal Conditioning

49.

__________ is solid matter that settles at the bottom in the settling tank

a)

Sludge

b)

Sewage

c)

Biological

d)

Contaminants

50.

The permissible limit of free residual chlorine is

a)

0.02ppm

b)

0.2ppm

c)

1ppm

d)

2ppm

51.

The normal dose of chlorine during plain chlorination is

a)

0.5-1ppm

b)

0.1-0.2ppm

c)

0.1-0.5ppm

d)

1-2ppm

52.

What are pathogens?

a)

Chemicals

b)

Particles clumped together.

c)

All the organisms that live in bodies of water.

d)

Organisms that cause mild to severe disease.

53.

nascent oxygen act a disinfectant in ozonization

a)

True

b)

False

54.

caustic embrittlement is due to the presence of

a)

Na2CO3

b)

NaHCO3

55.

sludges are loose, slimy, non-adherent precipitates

a)

False

b)

True

56.

generation of wet steam in the boiler is called as....

a)

foaming

b)

priming

57.

The removal of salt from brackish or ocean water is known as:

a)

denitrification

b)

desalination

c)

re-salination

d)

hyper salination

58.

Ion-exchange resin is __________

a)

Soluble

b)

Organic polymer with porous structure

c)

Low molecular weight

d)

Linear

59.

Which of the following ion get released from the cation exchange column?

a)

Ca+2

b)

K+

c)

Na+

d)

H+

60.

Which of the following ion get released from the anion exchange column?

a)

SO4-2

b)

Cl–

c)

OH–

d)

CO3-2

61.

The residual hardness in ion-exchange process is ____________

a)

0-2 ppm

b)

10-15 ppm

c)

20-30 ppm

d)

5-10 ppm

62.

Lime Soda process uses

a)

Ca(OH)2Ca\left(OH\right)_2  

b)

Na2CO3Na_2CO_3  

c)

Both Of The Above

d)

None OF THe Above

63.

Alkalinity in water is due to

a)

OH−OH^-  

b)

HCO3−HCO_3^-  

c)

CO32−CO_3^{2^-}  

d)

All Of The Above

64.

Which is not used for disinfection of water

a)

Chlorination

b)

Ozonisation

c)

Electrodialysis

d)

Addition of KMnO4Addition\ of\ KMnO_4  

65.
The ions that cause hard water are;
a)
Calcium and Manganese ions
b)
Calcium and Magnesium ions
c)
Carbon and Magnesium ions
d)
Carbon and Manganese ions
66.
If water contains calcium and hydrogen carbonate ions, it is described as....
a)
temporarily permanently soft water
b)
Soft water
c)
Permanently hard water
d)
Temporary hard water
67.

Which of the following does not cause the permanent hardness in water?

a)

Nitrates

b)

Sulphates

c)

Chlorides

d)

Bicarbonates

68.

In _____________ when the water is heated then the soluble salts turns into insoluble ones and removed by filtration.

a)

Temporary hardness

b)

Permanent hardness

c)

Non-carbonate

d)

Non-alkaline

69.

Identify water softening methods from following

a)

Reverse Osmosis

b)

Deionisation

c)

Zeolite method

d)

electrodialysis

e)

activated sludge

70.

In lime soda method the principle is ----

a)

Convert soluble salt into insoluble precipitate

b)

substitute cations and anions of hardness producing salts

c)

replace cations by Na+

d)

none of the above

71.

Once the water softening is done, we need to throw resins.

a)

TRUE

b)

FALSE

72.
Water that runs over gypsum rock forms.....
a)
temporarily permanently soft water
b)
Soft water
c)
Permanently hard water
d)
Temporary hard water
73.
Water that runs over limestone rock forms.....
a)
temporarily permanently soft water
b)
Soft water
c)
Permanently hard water
d)
Temporary hard water
74.

The chemical formula of zeolite is ___________

a)

FeSO4.7H2O

b)

Na2Al2O

c)

Al2(SO4)3.18 H2O

d)

Na2O.Al2O3.xSiO2.yH2O

75.

Permanent hardness in water is caused by the presence of:

a)

Calcium bicarbonate

b)

Magnesium sulphate

c)

Both of them

d)

None of them

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