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WorksheetsRate of reaction and Equilibrium
Total questions: 15
Worksheet time: 15mins
Name
Class
Date
1.
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)
Increases the frequency of collision between particles
2.
Which of the following slows down the rate of a chemical reaction?
a)
Place the reactants in hot water
b)
Place the products in ice bath
c)
Place the reactants in a ice bath
d)
Keep stirring the reactants with a stirring rod
3.
If more reactants are used in a chemical reaction, more products will be produced. This is because
a)
More reactants cause the reaction to heat up
b)
More reactants take up the same volume
c)
More reactants have more particles to react to form more products
d)
Too many products can slow down the reaction
4.
What makes an effective collision?
a)
When molecules collide.
b)
When molecules collide with the proper orientation.
c)
When molecules collide with proper orientation and enough kinetic energy.
d)
High Temperature.
5.
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.
6.
For the reaction...
SO2 + O2 <=> SO3
If the concentration of SO2 is increased, the equilibrium position of the reaction will shift ___________.
SO2 + O2 <=> SO3
If the concentration of SO2 is increased, the equilibrium position of the reaction will shift ___________.
a)
to the left
b)
to the right
c)
to the left and right
d)
neither left nor right
7.
For the reaction...
N2 + O2 <=> 2NO
If O2 is removed, the concentration of N2 will _______.
N2 + O2 <=> 2NO
If O2 is removed, the concentration of N2 will _______.
a)
increase
b)
decrease
c)
remain the same
d)
double
8.
For the reaction...
N2 (g) + 3 H2 (g) <=> 2 NH3 (g)
If the pressure in the system is increased, which substance(s) will increase in concentration?
N2 (g) + 3 H2 (g) <=> 2 NH3 (g)
If the pressure in the system is increased, which substance(s) will increase in concentration?
a)
N2 (as 2 mol gas → 4 mol gas)
b)
H2 (as 2 mol gas → 4 mol gas)
c)
N2 and H2 (as 2 mol gas → 4 mol gas)
d)
NH3 (as 4 mol gas → 2 mol gas)
9.
Identify the labels (a) and (b) on the graph.
a)
a is concentration of reactants and b is the concentration of product
b)
a is concentration of product and b is the concentration of reactant
c)
a is the volume of reactants and b is the volume of product
d)
a the mass of reactants and b is the mass of product
10.
When the system X + 2 Y <=> Z has reached equilibrium, which of the following is TRUE?
a)
Forward reaction and Backward reaction stop.
b)
Forward reaction has sped up and backward reaction has slowed down.
c)
Forward and backward reactions occur at the same rate.
d)
Forward reaction has slowed down and backward reaction has sped up.
11.
For the reaction...
N2 + O2 <=> 2NO: Δ H = +182 kJ mol-1.
If the temperature is increased the equilibrium position will shift _______.
N2 + O2 <=> 2NO: Δ H = +182 kJ mol-1.
If the temperature is increased the equilibrium position will shift _______.
a)
to the left
b)
to the right
c)
to the left and right
d)
neither left nor right
12.
Under certain conditions, cyclohexane can react to form benzene and hydrogen according to the equation:
C6H12(g) → C6H6(g) + 3H2(g); ΔH=+206 kJ mol-1
Which two changes could be used to increase the rate of reaction?
C6H12(g) → C6H6(g) + 3H2(g); ΔH=+206 kJ mol-1
Which two changes could be used to increase the rate of reaction?
a)
Add a catalyst and reduce the temperature
b)
Add a catalyst and decrease the pressure
c)
Increase the temperature and the external pressure
d)
Add a catalyst and decrease the concentration of cyclohexane
13.
The main reason for the use of catalysts in most industrial processes is to
a)
reduce greenhouse gas emissions
b)
reduce the energy requirement for a reaction
c)
reduce waste production
d)
increase the yield of product
14.
Which of the following changes that can be made to a chemical reaction will result in a greater proportion of successful collisions between reactant particles?
I. addition of a catalyst
II. grinding reactant lumps into a powder
III. increasing the concentration of reactants
I. addition of a catalyst
II. grinding reactant lumps into a powder
III. increasing the concentration of reactants
a)
I only
b)
II and III only
c)
I and II only
d)
I, II and III
15.
N2O4(g) ⇌ 2NO2(g) ΔH = -58.0 kJ mol-1
N2O4(g) is colourless and NO2(g) is brown
If the pressure was increased, the brown colour would
N2O4(g) is colourless and NO2(g) is brown
If the pressure was increased, the brown colour would
a)
disappear completely
b)
deepen / get darker
c)
stay the same
d)
fade / get lighter brown
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