Comprehensive Analysis of Chemical Kinetics & Equilibrium

This assignment delves into the fundamental principles of chemical kinetics and equilibrium. It addresses collision theory, activation energy, and molecular orientation as key factors influencing reaction rates. The exothermic nature of a specific reaction is identified, and the role of activation energy in chemical reactions is discussed. The assignment further explores the impact of catalysts on reaction rates, emphasizing how they lower activation energy. Factors affecting reaction rates, such as reactant concentration, physical state, surface area, temperature, and the presence of catalysts, are examined. The concept of equilibrium is explained, along with Le Chatelier's principle, to predict the effects of changes in pressure, reactant concentration, and the addition of catalysts on equilibrium reactions. The point at which equilibrium is reached is determined using a graph. Desklib provides students with access to this solved assignment and a variety of study resources to enhance their understanding.

1.
The three principles are:
Collision – collision between the molecules must be effective in such a way that they bring
chemical change.
Activation energy – the molecules should possess internal energy in order to have successful
collision.
Orientation – not only the collision and activation energy are required for an effective reaction
but also the orientation matters. The molecules must also collide in the proper orientation for a
reaction to occur.
2.
The reaction is classified as exothermic.
During the reaction, formation of products resulted in release of energy more than that of the
reactants, that is equal to -803kJ/mol.
Negative sign indicates that the energy is released.
Thus, this reaction is exothermic and generates 803 kJ of energy per mole.
3.
B
Activation energy – the molecules should possess internal energy in order to have successful
collision.
4.
D
Heat released.
5.

“H” represents the activated complex.
Because of the activated complex, the exothermic reactions do not occur spontaneously. The
activated complex is the step in the reaction when the compound is not stable.
6.
Sketch of the effect of the addition of a catalyst.
7.
The factors are:
Reactant concentration – concentration of reactants is directly proportional to the rate of reaction.

The physical state of the reactants and surface area – Surface area of the reactant molecules is
directly proportional to the rate of reaction.
Temperature – temperature is directly proportional to average kinetic energy of the reactant
molecules and is in turn proportional to the rate of reaction.
Presence of a catalyst – without being consumed a substance fastens the rate of reaction b
catalyst accelerates a reaction by participating in it without being consumed.
8.
Graph B represents the fastest reaction rate.
With the production of CO2 gas, its volume got increased at a rapid rate first and then tapered off
due to a greater number of collisions of reactant molecules at the beginning of the reaction than
at the end.
9.
Catalyst lowers the activation energy needed for the reaction to proceed, allowing participation
of more particles having activation energy required to increase the reaction rate.
10.
Crush reactant A into a powder.
Crushing the reactant A will result in increased surface area. As, surface area is proportional to
the rate of reation, the reaction will take place at a faster rate.
11.
The forward and reverse reactions occur at equal rates.
As there is no change in the concentration of the reactants and the products.
12.
Given the reaction: 2N2O(g) + O2(g) <-> 4NO(g)

a. increasing the pressure – No change – equilibrium reaction
There will be no change in either the forward or reverse reaction. So the amount of each
substance will be unchanged.
b. Removing O2 – shift right – reverse reaction takes place.
The equilibrium will shift to the left and reverse process will take place.
c. adding NO – shift left
The equilibrium will shift to the left and consume the NO to create more N2O and O2
d. adding N2O - shift left – forward reaction takes place
The equilibrium will shift left and the reactants will react to produce more of the NO
e. addition of a catalyst – No change – equilibrium reaction
The addition of a catalyst will have no effect on the equilibrium position as both the forward and
reverse reactions rates would be increased equally.
13.
At 1 second, the concentration of the reactants A and B are constant, therefore we can say that by
looking at the graph, the equilibrium is reached.