CHEM 219 MODULE 5 ACTUAL EXAM
SCRIPT WITH SOLVED QUESTIONS AND
VERIFIED SOLUTIONS
◉ In what case would reaction not be able to proceed due to
collision theory and rate of reactions
Answer: If the activation energy of energy of the either of them is
high, then that reaction is unlikely to proceed because very few
particles will have enough energy for a successful collision
◉ What does it take for a reaction to be reversible in terms of
collision theory
Answer: For a reaction to be reversible, the activation energies of
both the forward and the reverse reaction must be low enough
that sufficient particles will have enough energy for a successful
collision
◉ How does forward and reverse reactions work in terms of
collision theory and rate of reaction
Answer: - Forward reaction start high then fall
- Reverse reactions start low then rise as the products being
produced increase
◉ What Happens to the Reactants Overtime in a forward reaction
Answer: - Concentration of reactants is decreasing over time
,- Reducing the number of reactant particles
◉ How Does the Concentration of reactants decreasing affect the
number of collisions between Reactants and Products?
Answer: Fewer particles mean fewer collisions
◉ Do more particles now satisfy the conditions of collision
Theory, when Concentration of reactants is decreasing over time
Answer: - Because concentration is lower, there are likely less
collisions
- Less reactant particles meet the conditions of collision theory
◉ What happens to the rate of a forward reaction?
Answer: Fewer successful collisions means a decrease in the rate
of the forward reaction
◉ What Happens to a reverse Reactants Overtime?
Answer: Number of product particles increase
◉ How Does the Number of product particles increasing affect the
number of collisions between Reactants and Products?
Answer: More particles means more collisions
◉ Do more particles now satisfy the conditions of collision Theory
in a reverse reaction
,Answer: More product particles meet the conditions of the
collision theory
◉ What happens to the rate of the reverse reaction
Answer: More successfully collisions means an increase in the rate
of the reverse reaction
◉ What factors affect Equilibrium
Answer: - Change in Temperature
- Change in Pressure and Volume (Only in Gaseous substances)
- Change in Concentration
- The equilibrium will change to counteract the disturbance and
re-establish the equilibrium
◉ Le Chatelier's Principle
Answer: - States that if a system is in equilibrium and it is
disturbed or changed in any way, then the system will adjust itself
to minimise the amount of change
- If equilibrium moves to the right, then the products are favoured
- If it moves left the reactants are favoured
◉ How does change in concentration affect equilibrium
Answer: - Adding additional reactant to a system will shift the
equilibrium to the right (Products)
, - Reducing concentration of any product will also shift
equilibrium to the right
- If we add additional product to a system, the equilibrium will
shift to the left (reactant)
- If we remove reactants from the system, will be shifted to the left
(reactant)
◉ Changes in concentration to a equilibrium reaction in terms of
the collision theory
Answer: This is supported through collision theory, as the
concentration of either the product/reactant will determine how
equilibrium will present itself
◉ How do changes in Pressure affect equilibrium
Answer: - Will result in an attempt to restore equilibrium by
creating more or less moles of gas
- If pressure increases or volume decrease the equilibrium will
shift to favour the side of reaction that involves fewer moles of gas
- If the volume of a system increases, or the pressure decrease the
production of additional moles of gas is forward
- When number of moles is equal on both sides there is no change
Only applies to Gases
◉ How do changes in Temperature affect equilibrium
Answer: - If we raise the temp. On an endothermic reaction, it is
like adding more reactant, therefore equilibrium will shift to right
SCRIPT WITH SOLVED QUESTIONS AND
VERIFIED SOLUTIONS
◉ In what case would reaction not be able to proceed due to
collision theory and rate of reactions
Answer: If the activation energy of energy of the either of them is
high, then that reaction is unlikely to proceed because very few
particles will have enough energy for a successful collision
◉ What does it take for a reaction to be reversible in terms of
collision theory
Answer: For a reaction to be reversible, the activation energies of
both the forward and the reverse reaction must be low enough
that sufficient particles will have enough energy for a successful
collision
◉ How does forward and reverse reactions work in terms of
collision theory and rate of reaction
Answer: - Forward reaction start high then fall
- Reverse reactions start low then rise as the products being
produced increase
◉ What Happens to the Reactants Overtime in a forward reaction
Answer: - Concentration of reactants is decreasing over time
,- Reducing the number of reactant particles
◉ How Does the Concentration of reactants decreasing affect the
number of collisions between Reactants and Products?
Answer: Fewer particles mean fewer collisions
◉ Do more particles now satisfy the conditions of collision
Theory, when Concentration of reactants is decreasing over time
Answer: - Because concentration is lower, there are likely less
collisions
- Less reactant particles meet the conditions of collision theory
◉ What happens to the rate of a forward reaction?
Answer: Fewer successful collisions means a decrease in the rate
of the forward reaction
◉ What Happens to a reverse Reactants Overtime?
Answer: Number of product particles increase
◉ How Does the Number of product particles increasing affect the
number of collisions between Reactants and Products?
Answer: More particles means more collisions
◉ Do more particles now satisfy the conditions of collision Theory
in a reverse reaction
,Answer: More product particles meet the conditions of the
collision theory
◉ What happens to the rate of the reverse reaction
Answer: More successfully collisions means an increase in the rate
of the reverse reaction
◉ What factors affect Equilibrium
Answer: - Change in Temperature
- Change in Pressure and Volume (Only in Gaseous substances)
- Change in Concentration
- The equilibrium will change to counteract the disturbance and
re-establish the equilibrium
◉ Le Chatelier's Principle
Answer: - States that if a system is in equilibrium and it is
disturbed or changed in any way, then the system will adjust itself
to minimise the amount of change
- If equilibrium moves to the right, then the products are favoured
- If it moves left the reactants are favoured
◉ How does change in concentration affect equilibrium
Answer: - Adding additional reactant to a system will shift the
equilibrium to the right (Products)
, - Reducing concentration of any product will also shift
equilibrium to the right
- If we add additional product to a system, the equilibrium will
shift to the left (reactant)
- If we remove reactants from the system, will be shifted to the left
(reactant)
◉ Changes in concentration to a equilibrium reaction in terms of
the collision theory
Answer: This is supported through collision theory, as the
concentration of either the product/reactant will determine how
equilibrium will present itself
◉ How do changes in Pressure affect equilibrium
Answer: - Will result in an attempt to restore equilibrium by
creating more or less moles of gas
- If pressure increases or volume decrease the equilibrium will
shift to favour the side of reaction that involves fewer moles of gas
- If the volume of a system increases, or the pressure decrease the
production of additional moles of gas is forward
- When number of moles is equal on both sides there is no change
Only applies to Gases
◉ How do changes in Temperature affect equilibrium
Answer: - If we raise the temp. On an endothermic reaction, it is
like adding more reactant, therefore equilibrium will shift to right
