Answer:
The oxidation number of iron changes from 2+ to 0.
10 electrons are transferred in the reaction.
Explanation:
Step 1: Write the balanced redox reaction
5 Fe²⁺ + 2 Mn²⁺ + 8 H₂O ⇒ 2 MnO₄⁻ + 5 Fe + 16 H⁺
Step 2: identify both half-reactions
Reduction: 5 Fe²⁺ + 10 e⁻ ⇒ 5 Fe
Oxidation: 2 Mn²⁺ + 8 H₂O ⇒ 2 MnO₄⁻ + 16 H⁺ + 10 e⁻
Step 3: Identify the oxidation state change of iron
Iron changes from Fe²⁺ to Fe, that is, the oxidation number changes from 2+ to 0.
Step 4: Determine how many electrons are transferred in the reaction?
According to both balanced half-reactions, 10 electrons are transferred in the reaction.
Valence Electron is the outermost electrons, family(Alkali) 1 has 1 valence electrons and family(Alkaline) 2 has 2 valence electrons.
Hope this helps
In a chemical reaction, the equilibrium constant refers to the value of its reaction quotient at chemical equilibrium, that is, a condition attained by a dynamic chemical system after adequate time has passed, and at which its composition has no measurable capacity to undergo any kind of further modification.
The given reaction is: HCN (aq) + OH⁻ = CN⁻ (aq) + H2O (l)
The equilibrium constant = product of concentration of products / product of concentration of reactants
(Here, H2O is not considered as its concentration is very high)
So, Keq = [CN⁻] / [HCN] [OH⁻]
Answer:
both will be at liquid state. the particles will move rapidly in all directions and will collide with other particles in random motion
