Explain the following observation in terms of the collision theory, restricting each to about 25 words.
NO(g) + O3(g)--> NO2(g) + O2(g)
(a) An increase in temperature increases the reaction rate.
(b) Compressing the gases into a smaller volume increases the reaction rate.
(c) Adding a small amount of a nickel catalyst to the reaction vessel increases the rate without increasing the temperature.
a. Increasing T increases the energy of the molecules which increases the probability that a reaction will take place when a collision takes place.
b. Compressing the gas into a smaller volume increases the concn of the gases and that increases the change of a collision.
c. Adding a Ni catalyst provides a surface to which the molecules can form an intermediate. It effectively lowers the activation energy for the reaction.
Did you get the formal charge question taken care of? Do you understand how to assign formal chargers.
what is the mean of non integer coefficients in the chemical reactions and why is used?
(a) An increase in temperature increases the reaction rate because it provides more kinetic energy to the molecules, increasing their collision frequency and the chance of successful collisions.
To explain this observation using collision theory, we know that reacting molecules must collide with sufficient energy (activation energy) and proper orientation for a successful reaction. When temperature is increased, the average kinetic energy of the molecules increases, which means they move faster and collide more frequently. This higher collision frequency leads to a greater number of successful collisions, thereby increasing the reaction rate.
(b) Compressing the gases into a smaller volume increases the reaction rate because it increases the pressure, leading to more frequent collisions between the reactant molecules.
According to collision theory, increasing the pressure on a gas increases the concentration of molecules in a given volume, which in turn increases the frequency of collisions. When gases are compressed into a smaller volume, the available space for gas molecules to move decreases, leading to a higher concentration and more collisions. This increased collision frequency increases the reaction rate.
(c) Adding a small amount of a nickel catalyst to the reaction vessel increases the rate without increasing the temperature because it provides an alternative reaction pathway with a lower activation energy.
In collision theory, a catalyst is a substance that speeds up a reaction without being consumed itself. When a catalyst is present, it lowers the activation energy required for the reaction to occur. By providing an alternative pathway for the reaction, the catalyst allows more reactant molecules to possess the necessary energy and orientation for a successful collision. Thus, the reaction rate increases even though the temperature remains the same.