What are you trying to find?
<h3>
Answer:</h3>
The Equilibrium would shift to produce more NO
<h3>
Explanation:</h3>
The reaction is;
N₂(g) + O₂(g) ⇆ 2NO(g)
- When a reaction is at equilibrium then the forward reaction rate will be equivalent to the reverse reaction rate. Additionally, the concentration of the reactants and products are the same.
- From Le Chatelier's principle, additional reactants favor the formation of more products while additional products favor the formation of more reactants.
- For example, when more oxygen is added then more Nitrogen (II) oxide will be formed.
- Oxygen is a reactant and when increased it favors forward reaction which leads to the formation of more NO which is the product.
Answer: 0.52V
Explanation:
Ecell = Ecell(standard) - [(0.0592 logQ)/n]
Q = product of the quotient
n = no of electrons transferred = 2
Ecell = 0.63 - [(0.0592*Log(1 / 2.0 * 10-4) / 2]
Ecell = 0.63 - 0.0194
Ecell = 0.5205V
Answer:
It's Effective Collision.
Explanation:
Hope my answer has helped you!
