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JAMB questions for "Chemistry :: Rates of chemical reaction"
Q1

Which of the following is used as a rocket fuel?

A

H2SO4

B

HCl

C

HNO3

D

CH3COOH

E
Q2

The final products of the reaction between methane and chlorine in the presence of ultraviolet light are hydrogen chloride and

A

tetrachlomethane

B

chloromethane

C

trichloromethane

D

dichloromethane  

E
Q3

The haloalkanes used in the dry - cleaning industries are

A

trichloroethene and tetrachloroethene

B

chloromethane and dichloromethane

C

trichloromethane and tetrachloromethane

D

chloroethene and dichloroethene

E
Q4

C(s) + H2O(g) → H2(g) + CO(g)  ΔG for the reaction above at 1300k is -43kJ. At this temperature, the reaction is

A

not feasible

B

at equilibrium

C

feasible

D

exothermic

E
Q5

A catalyst increases the rate of a chemical reaction by providing a path that

A

raises the activation energy

B

increases the temperature

C

lowers the activation energy

D

increases the concentration

E
Q6

Na2S2O3(aq) + 2HC(aq) → 2NaCl(aq) + H2O(l) + SO2(g) + S(s)

 

Which of the following would introduce the greatest increase in the rate of the chemical reaction above?

A

A decrease in temperature and an increase in the concentration of the reactants

B

An increase in temperature and a decrease in the concentration of the reactants

C

An increase in temperature and an increase in the concentration of the reactants 

D

A decrease in volume and an increase in the pressure of the reactants

E
Q7

H3PO4(aq) + H2O(l) ↔ H2PO4-(aq) + H3O+(aq) ΔH = -13kJ at 298K

 

In the reaction above, an increase in temperature would 

A

favour the forward reaction

B

favour the reverse reaction

C

have no effect on the reaction

D

slow down the reverse reaction

E
Q8

Cu2+(aq) + 4NH3(g) ↔ [Cu(NH3)4]2+(aq)

 

In the reaction above, what is the effect of precipitating  Cu2+ as CuS(s)?

A

There will be no effect

B

The equilibrium will shift to the right

C

More NH3(g) concentrate will be generated

D

NH3(g) concentration will decrease

E
Q9

The tincture of iodine means iodine dissolved in

A

water

B

ethanol

C

bromine chloride

D

chlorine water

E
Q10

Dynamic equilibrium describes a situation where

A

a reaction gives back the reactants

B

the concentration of reactants and products is equal

C

both forward and reverse reactions proceed at the same rate

D

reactants are converted to products

E
Q11
Which of the following typically represents a photochemical reaction?
A
formation of water from hydrogen and oxygen molecules
B
conversion of dinitrogen  (IV) oxide to nitrogen (IV) oxide
C
Decomposition of calcium hydroxide o its oxide
D
conversion of silver halides to grey metallic silver
E
Q12
What is the molar mass of a substance, if 0.4 mole of the substance has a mass of 25.0g?
A
62.5g
B
40.0g
C
6.3g
D
2.5g
E
Q13
In the diagram below, which of the curves illustrates Arrhenius' law
A
R
B
X
C
Y
D
Z
E
Q14
In the reaction above, Y represents 
A
C2H5COOH
B
CH4
C
CH3OCH3
D
C2H4
E
Q15
The alkyl group that can be represented by the general formula
A
CnH2n
B
CnH2n-2
C
CnH2n+1
D
CnH2n+2
E
Q16
A chemical reaction is always associated with
A
a change in the nature of the reactants
B
the formation of new substances
C
a change in the volume of the reactants
D
an increase in the composition of one of the substances
E
Q17
Which of the following shows litle or no net reaction when the volume of the system is decreased?
A
2O3(g) ↔ 3O2(g) 
B
H2 + I2(g) ↔ 2HI(g)
C
2NO2(g) ↔ N2O4(g)
D
PCl5(g) ↔ PCl3(g) + Cl2(g)
E
Q18
N2O4(aq) ↔ 2NO2(aq)   In the endothermic reaaction above, more product formation will be favoured by
A
a decrease in pressure
B
a decrease in volume
C
an increase in pressure
D
a cinstant volume
E
Q19
Which of the following will change when a catalyst is added to a chemical reaction?
A
The potential energy of the product
B
The heat of reaction
C
The activation energy
D
The potential energy of the reactants
E
Q20
2HCl(aq) + CaCO3(aq) → CaCl2(s) + CO2(g) + H2O(l)   From the reaction above, which of the curves in the diagram represents the production of carbon (IV) oxide as dilute HCl is added?
A
M
B
P
C
L
D
N
E
Q21
CO(g) + H2O(g) → CO2(g) + H2(g)   From the reaction above, calculate the standard heat change if the standard enthalpies of formation of CO2(g), H2O(g) and CO(g) in kJ mol-1 are -394, -242 and -110 respectively.
A
+262 kJ mol-1
B
+42 kJ mol-1
C
-42 kJ mol-1
D
-262kJ mol-1
E
Q22
When sugar is dissolved, in tea, the reaction is always accompanied by
A
a minimum entropy change
B
no entropy change
C
positive change
D
negative entropy change
E
Q23
What mass of K2CrO4 is required to prepare 250cm3 of 0.020 mol dm-3 solution?   [K2CrO4 = 194.2g mol-1]
A
97.10 g
B
19.42 g
C
9.70 g
D
0.97 g
E
Q24
What volume of oxygen is produced from the decomposition of 2 moles of KClO3 at s.t.p?   [Molar volume of a gas at s.t.p = 22.4dm3]
A
33.6dm3
B
44.8dm3
C
67.2dm3
D
22.4dm3
E
Q25
The Arrhenius equation expresses the relationship between the speed of a reaction and its
A
molecular collisions
B
heat of reaction
C
catalyst
D
activation energy
E
Q26
PCl5(g) ↔ PCl3(g) + Cl2(g)   In the reaction above, a decrease in pressure will
A
decelerate the reaction
B
increase the yeild of PCl3
C
increase the yeild of PCl5
D
accelerate the reaction
E
Q27
In the diagram above, the curve that represents the production of oxygen gas from the decomposition of KClO3 in the presence of MnO2 catalyst is 
A
R
B
P
C
S
D
Q
E
Q28
In the reaction E + F ↔ G + H, the backward reaction is favoured if the concentration of 
A
F is increased
B
E is increased
C
E is reduced
D
G is reduced
E
Q29
A compound contains 31.91% potassium, 28.93% chlorine and the rest oxygen. What is the chemical formula of the compound?   [K = 39, Cl = 35.5, O = 16]
A
KClO4
B
KClO
C
KClO2
D
KClO3
E
Q30
A characteristic reaction of the compounds with the general formular CnH2n is
A
substitution
B
esterification
C
decarboxylation
D
polymerization
E
Q31
In which of these reactions does reduction take place?
A
2O2 → O2 + 4e-
B
Fe2+ - e- → Fe3+
C
2H+ + 2e- → H2
D
Cr - 2e- → Cr2+
E
Q32
Which of the following best explains the increase in the rate of a chemical reaction as the temperature rises?
A
a lower proportion of the molecules has the necessary minimum energy to react
B
the bonds in the reacting molecules are more readily broken
C
the collisions frequency of the molecules increases
D
the molecular collisions become more violent
E
Q33
In which of the following reactions has the oxidation number of nitrogen increased?
A
2NO(g) + Br2(l) → 2NOBr(l)
B
FeSO4(aq) + NO(g) → Fe(NO)SO4(s)
C
2NO(g) + Cl2(g) → 2NOCl(l)
D
2NO(g) + O2(g) → 2NO2(g)
E
Q34
Powdered marble reacts faster with hydrochloric acid solution than the granular form because the powdered form has
A
more molecules
B
more atoms
C
large surface area
D
relatively large mass
E
Q35
HCl(aq) + H2O(l) ↔ H3O+(aq) + Cl-   In the reaction above, Cl-(aq) is the
A
conjugate acid
B
acid
C
conjugate base
D
base
E
Q36
The partial pressure of oxygen in a sample of air is 452 mm Hg and the total pressure is 780 mm Hg. What is the mole fraction of oxygen?
A
0.203
B
0.579
C
2.030
D
5.790
E
Q37
X + Y → Z. The rate equation for the chemical reaction above is  -Δ[X]/Δt = K[X]2[Y]   The overall order of the reaction is
A
0
B
1
C
2
D
3
E
Q38
2SO2(g) + O2(g) ↔ 2SO3(g). In the chemical reaction above, the substance that will increase the rate of production of sulphur (VI) oxide is 
A
manganese (VI) oxide
B
finely divided iron
C
vanadium (V) oxide
D
nickel
E
Q39
The least reactive element is
A
W
B
X
C
Y
D
Z
E
Q40
2X(g) + Y(g) → Z(g). in the equation the rate of formation of Z is found to be independent of the concentration of Y and to quadrupe  when the concentration of X is doubled. The correct rate equation for the reaction is
A
R = k[X][Y]
B
R = k[X]2[Y]
C
R = k[X]0[Y]2
D
R = k[X]2[Y]0
E
Q41
If the rate law obtained for a given reaction is rate = k[X]n[Y]m, what is the overall order of the reaction?
A
nm
B
n/m
C
n + m
D
n - m
E
Q42
Which of the following is a redox reaction?
A
KCl(aq) + H2SO4(aq) → KHSO4(aq) + HCl(aq)
B
2FeBr2(aq) + Br2(g) → 2FeBr3(aq)
C
3AgNO3(aq) + FeCl3(aq) → 3AgCl(aq) + Fe(NO3)3(aq)
D
H2CO3(aq) → H2O(I) + CO2(aq)
E
Q43
It can be deduced that the rate of reaction
A
for path l is higher than path ll
B
for path ll is higher than path l
C
is the same for both paths at all temperatures
D
depends on the value of both x and y at all pressures
E
Q44
CHCI3 + Cl2 → HCl + CCl4. The reaction above is an example of
A
an addition reaction
B
a substitution reaction
C
a chlorination reaction
D
a condensation reaction
E
Q45
The reaction taking place in flask G is known as
A
hydrolysis
B
double decomposition
C
dehydration
D
pyrolysis
E
Q46
The standard enthalpies of formation of CO2(g), H2O(g) and CO(g) in kJ mol-1 are -394, -242 and -110 respectively. What is the standard ethalphy change for the reaction CO(g) - H2O(g) → CO2 + H2(g)
A
-42 kJ mol-1
B
42kJ mol-1
C
-262 kJ mol-1  
D
+262 kJ mol-1
E
Q47
In the diagram above, curve X represents the energy profile for a homogeneous gaseous reaction. Which of the following conditions would produce curve Y for the same reaction?
A
Increase in temperature
B
Increase in the concentration of a reactant
C
Addition of a catalyst
D
Increase in pressure
E
Q48
NaCl(s) + H2SO4(l) → HCl(g) + NaHSO4(s). In the reaction above, H2SO4behaves as
A
a strong acid
B
an oxidizing
C
a good solvent
D
a dehydrating agent
E
Q49
When dilute aqueous solutions of lead (II) nitrate and potassium bromide are mixed, a precipitate is observed. The products of this reaction are
A
PbO(s) + Br-(aq) + KNO3
B
Br2 + NO2(g) + PbO2(s) + Br2(s)
C
PbO(s) + K+(aq) + Br(aq) + NO3
D
PbBr2(aq) + K(aq) + NO3(aq)
E
Q50
H2S +SO2(g) → 3S(s) + 2H2O(l). The above reaction is
A
a redox reaction in which H2S is the oxidant and SO2 is the reductant
B
a redox reaction in which SO2 is the oxidant and H2S is the reactant
C
not a redox reaction because there is no oxidant in the reaction equation
D
not a redox reaction because there is no reductant in the reaction equation
E
Q51
Magnesium (IV) oxide is known to hasten the decomposition of hydrogen peroxide. Its main action is to
A
increase the surface are of the reactants.
B
increase the concentration of the reactants
C
lower the activation energy for the reaction
D
lower the heat of reaction, ΔH, for the reaction
E
Q52
MnO-4 + 8H+ + ne → Mn++ + 4H2O. Which of the value of n in the reaction above?
A
2
B
3
C
4
D
5
E
Q53
The data in the table above shows the rate of reaction of nitrogen (II) oxide with chlorine at 250C. It can be concluded that doubling initial concentration of NO increases the rate of reaction by a factor of
A
two
B
three
C
four
D
five
E
Q54
Which of the reactions below is OT an example of a redox reaction?   I.      Fe + 2Ag+ → Fe2+ + 2Ag ↓II.     2H2S + SO2 → 2H2O + 3S ↓ III.    N2 + O2 ↔ 2NO IV.     CaCO3 ↔ CaO + CO2 
A
I, II and III
B
II and III
C
III and IV
D
IV only
E
Q55
Which of the following represents the balanced equation for the reaction of copper with concentrated trioxonitrate (V) acid? 
A
Cu(s) + 2H(NO3)2(aq) → Cu(NO3)2 + H2(g)
B
Cu(s) + 4HNO3(aq) → Cu(NO3)2(aq) + 2H2O  + 2NO(g)
C
3Cu(s) + 8HNO3(aq) → 3Cu(NO3)2(aq) + 4H2O(l) + 2NO(g)
D
  3Cu(s) + 4HNO3(aq) → 3Cu(NO3)2(aq) + 2H2O(l) + 2NO(g)  
E
Q56
The ion that may be assumed to have negligible concentration in a sample of water that lathers readily with soap is
A
Mg2+
B
K+
C
CO32-
D
HCO3
E
Q57
The diagram above shows the reaction path of an exothermic reaction. The heat of reaction path of an exothermic reaction. The heat of reaction is represented by
A
I
B
II
C
III
D
IV
E
Q58
Which of the following will produce the greatest increase in the rate of the chemical reaction represented by the equation   Na2S2O3(aq) + 2HCl(aq) → 2NaCl(aq) + H2O(l) + SO2(aq) + S(s)
A
A decrease in temperature and an increase in the concentrations of the reactants.
B
An increase in the temperature and a decrease in the concentrations of the reactants.
C
A decrease in the temperature and a decrease in the concentrations of the reactants.
D
E
Q59
In the reaction C6H10O5(s) → conc H2SO4 ........
A
a reducing agent
B
an oxidizing agent
C
a dehydrating agent
D
a catalyst
E
Q60
above reaction is known as
A
photolysis
B
cracking
C
isomerization
D
reforming
E