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Elite Science-Chemistry online competition round 2

Total questions: 101

Worksheet time: 3hrs 39mins

Name
Class
Date
1.
a)

A

b)

B

c)

C

d)

D

2.
a)

A

b)

B

c)

C

d)

D

3.
a)

A

b)

B

c)

C

d)

D

4.
a)

A

b)

B

c)

C

d)

D

5.
a)

A

b)

B

c)

C

d)

D

6.
a)

A

b)

B

c)

C

d)

D

7.
a)

A

b)

B

c)

C

d)

D

8.
a)

A

b)

B

c)

C

d)

D

9.
a)

A

b)

B

c)

C

d)

D

10.
a)

A

b)

B

c)

C

d)

D

11.
a)

A

b)

B

c)

C

d)

D

12.
a)

A

b)

B

c)

C

d)

D

13.
a)

A

b)

B

c)

C

d)

D

14.
a)

A

b)

B

c)

C

d)

D

15.
     In the reaction Zn + H2O --> ZnO2 + H2
 which element, if any, is oxidized? 
a)
Zinc
b)
Hydrogen
c)
Oxygen
d)
None
16.
How would you write the electrons in the reaction O2 --> O2-2 ?
a)
+2e- on the products
b)
+2e- on the reactants
c)
+e- on the products
d)
+e- on the reactants
17.
Which of the following is the balanced half -reaction for the oxidation of Cu to Cu+2?
a)
Cu   --> Cu+2
b)
Cu + 2 e-   --> Cu+2
c)
Cu  --> Cu+2  + 2 e-
d)
Cu - 2e-  --> Cu+2
18.
Is calcium oxidized or reduced in the following reaction? 
2CaO--> 2Ca + O2
a)
Oxidized
b)
Reduced
19.
Reduction happens at the 
a)
anode
b)
cathode
c)
salt bridge
d)
voltmeter
20.

What does electrochemistry deal with?

a)

chemical reactions

b)

chemical formulas

c)

electricity

d)

Le Chat's Principle

21.
An iron nail is put into a solution of copper nitrate, iron is above copper in the activity series of metals, what will happen?
a)
iron will be reduced
b)
bubbles of oxygen gas will form on iron nail
c)
the iron nail will become copper plated
d)
no reaction occurs
22.
If Al is above Co in the activity series of metals, which of the following will occur if Al metal is put into a solution of cobalt nitrate?
a)
a redox reaction takes place
b)
the Al strip dissolves
c)
the Al strip becomes coated with cobalt
d)
all of the above
23.

The diagram shows a failed attempt to copper-plate a pan.

Which action will plate the pan with copper?

a)

cooling the copper sulfate solution in an ice bath

b)

heating the copper sulfate solution to boiling point

c)

increasing the voltage from 3V to 6V

d)

making the pan the cathode and the copper the anode

24.

Which products are formed at the anode and cathode when electricity is passed through molten

lead(II) bromide?

a)

A

b)

B

c)

C

d)

D

25.

The diagram shows an electrolysis circuit.

At which electrode is hydrogen formed?

a)

A

b)

B

c)

C

d)

D

26.

Which of these is an electrolyte? Tick all that apply.

a)

A molten ionic substance

b)

An aqueous solution of an ionic substance

c)

A molten giant covalent lattice

d)

An aqueous solution of a giant covalent lattice

27.

What is the charge on cations?

a)

Positive

b)

Negative

28.

When molten lead bromide is electrolyzed, the products are

a)

lead at the cathode and

bromine at the anode

b)

hydrogen at the cathode and

bromine at the anode

c)

bromine at the cathode and

hydrogen at the anode

29.

Which is the rule for deciding the product at the cathode?

a)

The more reactive metal/hydrogen ion remains in the solution.

b)

The less reactive metal/hydrogen ion remains in the solution.

30.

What is the rule for predicting the product of electrolysis of a solution at the anode?

a)

If a halide ion is present,

the halogen will be produced

b)

Oxygen is always produced

c)

Sodium hydroxide is produced

31.

What is the equation to show what happens to Cl- ions at the anode?

a)

Cl- --> Cl + e-   

b)

2Cl- --> Cl2 + 2e-   

c)

Cl2 + 2e-  -->  2Cl- 

32.

Positive ions (cations) will move towards the cathode (-) where they can ____.

a)

break apart

b)

lose electrons

c)

gain electrons

33.

Choose the half-equation that shows the change of an aluminum ion at the cathode.

a)

Al2+ + 3e- --> Al

b)

Al3+ + 3e- --> Al

c)

Al3+ --> Al + 3e-

34.
What is electrolysis?
a)
breaking down of a compound using a current
b)
making a compound using a current
35.
Explain why the electrolyte has to be a liquid.
a)
So the ions can move
b)
So the electrons can move
c)
So that it doesn't get too hot
d)
So the fish are ok
36.

What type of reactions can able to change products back to the their original form?

a)

Reversible reactions

b)

Irreversible reactions

c)

Combustion reactions

d)

Combination reactions

37.

Which of the following changes is irreversible change?

a)

Melting of ice cube

b)

Heating hydrated CuSO4

c)

Frying an egg

d)

Thermal decomposing NH4Cl

38.

Which of the following combination is correct?

a)

reversible ⇌

irreversible →

b)

reversible ←

irreversible →

c)

reversible ⇌

irreversible ←

d)

irreversible ⇌

reversible →

39.

If a reversible reaction is exothermic in the forward direction, it will be ...

a)

exothermic in the reverse direction

b)

endothermic in the forward direction too

c)

endothermic in the reverse direction

d)

not involve energy in reverse direction

40.
A substance that increases speed of chemical reaction without being being changed is called:
a)
Catalyst
b)
Acid
c)
Base
d)
pressure
41.
Increase in temperature of the reactants can do one of the following
a)
Slow collision frequency
b)
Allow less effective collision between the particles
c)
Cause particles to lose speed
d)
Increase collision between the particles thus increasing the rate.
42.

How does a catalyst work in speeding up a reaction?

a)

By lowering the activation energy or reaction

b)

by giving them more energy

c)

by making them more available

43.

Why does a higher concentration increase the rate of reaction?

a)

it increases the amount of reactants

b)

it lowers the activation energy

c)

it increases the energy of particle collisions

d)

it increases the frequency of particle collisions

44.

Why does a higher temperature increase the rate of a reaction?

a)

it increases both the frequency and energy of particle collisions

b)

it only increases the frequency of particle collisions

c)

it only increases the energy of particle collisions

d)

it reduces the activation energy of the reaction

45.

The ______________is required to break the bonds of the reactants.

a)

Carbonic energy

b)

Activation energy

c)

Plutonic energy

d)

Energi Gaib

46.
Why don't all collisions between particles cause a reaction?
a)
the particles also need to collide with a catalyst
b)
not all the particles collide with enough energy
c)
not all the particles collide at a high enough temperature
d)
the particles need to collide with each other twice
47.
What is the rate of reaction?
a)
How fast a reaction is 
b)
How big a reaction is
c)
How loud a reaction is
d)
How much gas a reaction produces
48.
Equilibrium is a __________ process
a)
Static
b)
Dynamic
c)
Probabilistic
d)
Fictitious
49.
The idea that when a system at equilibrium is stressed, it will react to relieve that stress and return to equilibrium is known as:
a)
Boyle's Law
b)
Le Chatelier's Principle
c)
Charles Law
d)
Denninger's Law
50.
At what time the reaction reached equilibrium?
a)
t1
b)
t2
c)
t3
d)
t4
51.
2NH3+22kJ↔N2+3H2
Which direction does the reaction shift if NH3 was removed?
a)
Shift right 
b)
Shift left
c)
No shift
d)
Shift both directions
52.
Increasing the temperature on a ________ reaction will increase the concentration of products.
a)
Endothermic
b)
Exothermic
c)
Isothermic
53.
 ΔH for an exothermic reaction will be 
a)
positive
b)
negative
c)
0
d)
undefined
54.
Which of the following is NOT true at equilibrium?
a)
The forward and reverse reactions proceed at the same rate.
b)
The concentrations of reactants and products do not change.
c)
The concentration of the reactants is equal to the concentration of the products.
d)
The forward and reverse reactions continue to occur.
55.
For the reaction...
N2 (g) +  3 H2 (g) <−> 2 NH3 (g)

If the pressure in the system is increased,  which substance will increase in concentration?
a)
N2
b)
H2
c)
N2 and H2
d)
NH3
56.

Which of the following is true about the formation of bonds between molecules?

a)

Energy is given off when bonds are formed between molecules.

b)

Energy is absorbed by the molecule when bonds are formed.

c)

Energy is neither given off nor absorbed when bonds are formed.

57.
Which letter corresponds to the energy of the products?
a)
A
b)
B
c)
C
d)
D
58.
If ∆H is negative, the reaction is?
a)
exothermic
b)
endothermic
59.

Which reaction is endothermic?

a)

acid neutralising alkali causing a temperature increase

b)

adding magnesium to hydrochloric acid

c)

calcium carbonate decomposing when heated combustion of fossil fuels

60.
Is photosynthesis an exothermic or endothermic reaction?
a)
Endothermic
b)
Exothermic
c)
Neither
61.

What type of reaction is this?

a)

Exothermic

b)

Endothermic

c)

Energy Producing

d)

No way to tell

62.

The graph above is from which type of reaction?

a)

Endothermic reaction

b)

Exothermic reaction

63.

Which of the following energy changes corresponds to the activation energy required for the forward reaction to take place?

a)

A

b)

C

c)

B

d)

E

64.

Hydrogen gas burns in air to form water.

2H2 (g) + O2 (g) → 2H2O(I) ΔH= - 572 kJ

How much heat energy (in kJ) is given off if a rocket carrying 200.0 kg of hydrogen gas is burnt in excess oxygen?

a)

1.43 x 107

b)

2.86 x 107

c)

4.92 x 107

65.
a)

A

b)

B

c)

C

d)

D

66.
a)

A

b)

B

c)

C

d)

D

67.
a)

A

b)

B

c)

C

d)

D

68.
a)

A

b)

B

c)

C

d)

D

69.

Using the equations below:


C(s) + O2(g) → CO2(g) ∆H = –390 kJ

Mn(s) + O2(g) → MnO2(s) ∆H = –520 kJ


what is ∆H (in kJ) for the following reaction?


MnO2(s) + C(s) → Mn(s) + CO2(g)

a)

910

b)

130

c)

-130

70.

2 NO ⟶ N2 + O2 (ΔH = -180.5 kJ)

N2 + 2 O2 ⟶ 2 NO2 (ΔH = + 66.36 kJ)

Calculate the entalphy for :

2 NO + O2 ⟶ 2 NO2 (ΔH = ?)

Is the overall process exothermic or endothermic?

a)

-114.14 kJ,

exothermic

b)

+114.14 kJ, endothermic

c)

246.9 kJ, endothermic

d)

-246.9 kJ, exothermic

71.

For the reaction 2H2(g) + O2(g) → 2H2O(g) the bond enthalpies (in kJ/mol) are

H-H = x, O=O = y, O-H = z

Which calculation will give the value, in kJ/mol, of ΔH for the reaction?

a)

2x + y - 2z

b)

4z - 2x - y

c)

2x + y - 4z

d)

2z - 2x - y

72.
Using the table of average bond energies below the image, the ΔH for the reaction in kJ is.....
a)
+ 160 kJ
b)
-63 kJ
c)
- 160 kJ
d)
-217 kJ
73.

When the solids Ba(OH)2 and NH4SCN are mixed, a solution is produced and the temperature drops. Which statement about the energetics of this reaction is correct?

a)

The reaction is endothermic and ΔH is negative

b)

The reaction is endothermic and ΔH is positive

c)

The reaction is exothermic and ΔH is negative

d)

The reaction is exothermic and ΔH is positive

74.
Increase in temperature of the reactants can do one of the following
a)
Slow collision frequency
b)
Allow less effective collision between the particles
c)
Cause particles to lose speed
d)
Increase collision between the particles thus increasing the rate.
75.
Grinding a seltzer tablet into powder increases the rate of reaction due to increased
a)
concentration
b)
surface area
c)
temperature
d)
reactants
76.
Which factors increase the rate of a reaction.
a)
increasing temperature
b)
increasing concentration
c)
increasing surface area
d)
all of these
77.
A ______________ is a substance that increases the rate of a reaction without being used up during the reaction. 
a)
catalyst
b)
product
c)
reactant
d)
solute
78.
a)

A

b)

B

c)

C

d)

D

79.

What can be said about the green line?

a)

it is a faster rate of reaction

b)

It produces same volume of product as red line

c)

Half the volume of reactants has been used

80.

Which would not speed up a chemical reaction?

a)

Using a large beaker

b)

Increasing the concentration

c)

Decreasing particle size

d)

adding a catalyst

81.

Which would have the slowest rate of reaction

a)

Magnesium ribbon 1M HCl at 20 degrees

b)

Magnesium powder 1M HCl at 20degrees

c)

Magnesium ribbon 0.5M HCl at 10degrees

d)

Magnesium powder 0.5M HCl at 10degrees

82.

Which graph shows the effect of increasing temperature on the rate of reaction of calcium carbonate with dilute hydrochloric acid?

a)
b)
c)
d)
83.

P, Q, R and S are pieces of apparatus.

Which row describes the correct apparatus for the measurement made?

a)

A

b)

B

c)

C

d)

D

84.
In an experiment, a 2 g lump of zinc and 2 g of powdered zinc are added separately to equal volumes of dilute sulphuric acid. The solid line on the graph shows the volume of gas given off when the 2 g lump is used. Which dotted line is obtained when the zinc is powdered? 
a)
A
b)
B
c)
C
d)
D
85.
a)

A

b)

B

c)

C

d)

D

86.
a)

A

b)

B

c)

C

d)

D

87.
a)

A

b)

B

c)

C

d)

D

88.
a)

A

b)

B

c)

C

d)

D

89.
a)

A

b)

B

c)

C

d)

D

90.
In which experiment is the rate of reaction between hydrochloric acid and calcium carbonate slowest? 
a)
A
b)
B
c)
C
d)
D
91.

AgNO3 + NaCl → AgCl + NaNO3

What would you expect to happen if we decrease the temperature of this reaction container?

a)

The energy of the reactants would decrease.

b)

The would be more product produced.

c)

The number of particles of

AgNO3 and NaCl would decrease.

d)

The number of collisions in the reactants would increase.

92.

Which of the following is true?

a)

The reaction rate of the diagram on the left would be greater because there are more collisions that will happen because of greater surface area.

b)

The reaction rate of the diagram on the right would be greater because there are more collisions that will happen because of lesser surface area.

c)

The reaction rate of the diagram on the right would be greater because there are more collisions that will happen because of greater surface area.

d)

The reaction rate of the diagram on the left would be greater because there are more collisions that will happen because of lesser surface area.

93.
The picture below is an example of _________________.
a)
osmosis
b)
isotonic
c)
diffusion
d)
active transport
94.
Atoms have no electric charge because they...
a)
have an equal number of charged and non charged particles
b)
have neutrons in their nuclei
c)
have an equal number of electrons and protons
d)
have an equal number of neutrons and protons
95.
NaHCO3 is an example of —
a)
an abbreviation
b)
a compound
c)
a mixture
d)
an element
96.
When an atom loses an electron, it becomes a:
a)
positive ion
b)
negative ion
c)
neutral ion
d)
neutral atom
97.
How are covalent bonds explained?
a)
When one atom takes the other atom's electron
b)
When the atom shares an electron with an another atom
c)
When the two nucleus merge
d)
When the neutrons leave the nucleus
98.

What happens to the reactivity of the alkali metals as you move down the group?

a)

increases

b)

decreases

99.
Which gas in our atmosphere is most abundant?
a)
Argon
b)
Oxygen
c)
Nitrogen
d)
Carbon Dioxide
100.

A(n) ______ is a substance with a pH less than 7

a)

Acid

b)

Alkali

c)

Base

d)

Buffer

101.

The laboratory test for oxygen is that

a)

it relights a glowing splint

b)

it relights a burning splint

c)

it changes lime water to milky

d)

it makes a glowing splint go out

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