Unit 6 - The Rate and Extent of Chemical Change Flashcards
How is rate of reaction
calculated?
Rate of reaction = amount of reactant used or product formed
time
Rate of reaction (mol/s) = Moles of reactant used or product formed
time
What are the various units for
rate of reaction?
Can include g/s or cm3
/s or mol/s
Generally, mass/time, volume/time, moles/time
Name three common ways of
measuring rate of reaction
- Loss in mass of reactants
- Volume of gas produced
- Time for a solution to become opaque
Describe measuring the rate
by monitoring mass loss
Place the reaction flask on a balance. In these reactions (e.g. metal carbonate +
acid) a gas is given off, so record the decrease in mass in time intervals (note
hydrogen is too light). Plot a graph of mass vs time
Describe measuring the rate
by monitoring the volume of a
gas
Connect a gas syringe to a reaction flask and measure the volume of a gas
formed in time intervals. Plot a graph of volume vs time.
Describe measuring the rate
by monitoring the
disappearance of a cross
Take a piece of paper and mark a cross (X) on it. Put the reaction flask on this
cross. Mix the reagents, and measure how long it takes for a cloudy mixture to
conceal a cross.
How to find a rate of reaction at
some time, t, from a graph of
amount of reactant vs time?
- Pick a point corresponding to the time t, and find the tangent to the curve at
this point. - The tangent is the gradient of this graph - it tells you how fast the reaction
proceeds at this point. The steeper the tangent line, the faster the rate.
Gradient of tangent can be expressed in change in y values over change in x
values.
State five factors affecting the
rate of a chemical reaction
- Concentration of reactants
- Pressure of gases (volume)
- Surface area
- Temperature
- Catalysts
What is the collision theory?
Chemical reactions can occur only when reacting particles collide with each other
with sufficient energy (more than or equal to activation energy).
Describe and explain the
effect of increasing
temperature on the rate of
reaction
T increases = faster reaction
As T increases, kinetic energy of particles increases, i.e. more energetic
collisions
Also, they move faster, so they collide more frequently
However, there is no straight line relationship between rate and temperature,
i.e. they are not directly proportional to each other
Describe and explain the effect
of increasing concentration on
the rate of reaction
concentration on the rate of reaction
Conc. increases = faster reaction,
More reactants = more frequent collisions
Describe and explain the effect
of increasing pressure of a gas
on the rate of reaction
Increasing the pressure of reacting gases, is the same as increasing
concentration. It increases the number of gas molecules in the same volume and
so increases the frequency of collisions and therefore increases the rate of
reaction.
Note that volume and pressure are inversely proportional to each other.
Increasing the volume retards the reaction.
Describe and explain the
effect of increasing surface
area
If solid reactants are in smaller pieces, they have a greater surface area.
Increasing the surface area of solid reactants increases the frequency of collisions
and so increases the rate of reaction, e.g. block of magnesium reacts slower with
acid then magnesium powder.
What is a catalyst and how
does it work? How does it
affect the reaction profile?
A catalyst changes the rate of reaction but is not used up. It increases rate of
reaction by providing a different pathway for the reaction that has a lower
activation energy. The reaction profile for a catalysed reaction will have a lower
maximum of the curve (lower activation energy).
What is an enzyme?
An enzyme is a molecule that acts as a catalyst in a biological system.
What is a reversible reaction?
A reversible reaction occurs when the products of a reaction can react backwards
to produce the original reactants
When is dynamic
equilibrium reached?
In a closed system, when the forward and reverse reactions occur at the same rate
and the concentrations of reactants and products remain constant.
Describe Le Chatelier’s
Principle
If a system is at equilibrium and a change is made to any of the conditions, then
the system responds to counteract change and restore the equilibrium.
Describe the effect of
changing the concentration of
reactant and product on the
position of the equilibrium
If the concentration of one of the reactants or products is changed, the system is
no longer at equilibrium and the concentrations of all the substances will change
until equilibrium is reached again. If the concentration of a reactant is increased,
more products will be formed until equilibrium is reached again. If the
concentration of a product is decreased, more reactants will react until equilibrium
is reached again.
Describe the effect of
changing temperature on the
position of the equilibrium
If the temperature of a system at equilibrium is increased:
* the relative amount of products at equilibrium increases for an endothermic
reaction
* the relative amount of products at equilibrium decreases for an exothermic
reaction
Describe the effect of
changing pressure on the
position of the equilibrium
An increase in pressure causes the equilibrium position to shift towards the side
with the smaller number of molecules as shown by the symbol equation for that
reaction. A decrease in pressure causes the equilibrium position to shift towards
the side with the larger number of molecules as shown by the symbol equation
for that reaction. Pressure has no effect on the reactions where the numbers of
gas molecules are equal on both sides of the equation.
Describe the effect of a
catalyst on the position of the
equilibrium
No effect.
It just speeds up both forward and backward reactions equally.
i.e. equilibrium is achieved faster.
