Answer: IN terms of the collision theory, increasing the concentration of a reactant increases in the number of collisions between the reacting species per second and therefore increases the reaction rate.
Explanation: hope u get it right
Answer:
Percentage dissociated = 0.41%
Explanation:
The chemical equation for the reaction is:

The ICE table is then shown as:

Initial (M) 1.8 0 0
Change (M) - x + x + x
Equilibrium (M) (1.8 -x) x x
![K_a = \frac{[C_3H_6ClCO^-_2][H^+]}{[C_3H_6ClCO_2H]}](https://tex.z-dn.net/?f=K_a%20%20%3D%20%5Cfrac%7B%5BC_3H_6ClCO%5E-_2%5D%5BH%5E%2B%5D%7D%7B%5BC_3H_6ClCO_2H%5D%7D)
where ;


Since the value for
is infinitesimally small; then 1.8 - x ≅ 1.8
Then;




Dissociated form of 4-chlorobutanoic acid = 
Percentage dissociated = 
Percentage dissociated = 
Percentage dissociated = 0.4096
Percentage dissociated = 0.41% (to two significant digits)
Unlikely. It's unlikely for ammonium ion
to accept a proton
and act as a Bronsted-Lowry Acid.
<h3>Explanation</h3>
What's the definition of Bronsted-Lowry acids and bases?
- Bronsted-Lowry Acid: a species that can donate one or more protons
in a reaction.
- Bronsted-Lowry Base: a species that can accept one or more protons

Ammonium ions
are positive. Protons
are also positive.
Positive charges repel each other, which means that it will be difficult for
to accept any additional protons. As a result, it's unlikely that
will accept <em>any</em> proton and act like a Bronsted-Lowry Base.
It is B, From the bottom of the pyramid to the top