During the workup portion of the reaction of alkenes with HBr as described in the experiment provided, a student transferred the
1 answer:
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Answer:
Explanation:
We classify the behaviours of electrolytes based on their electrolytic conduction. This is what makes them breaks down when in aqueous solutions with water.
A strong electrolyte is one that ionize completely when in aqueous solutions. Their ionization can be shown below using appropriate chemical notation:
An example of a strong electrolyte is NaCl:
NaCl → Na⁺
+ Cl⁻
Such reactions have a single forward arrow. Since they ionize complete, they have a large amoung of ions present in their aqueous form and would readily conduct.
A weak electrolyte is made up of compounds that ionize partially or slightly in their aqueous solution. The amount of ions produced per mole of compounds is relatively small compared to those of strong electrolytes. Examples ae organic acids, weak bases, and water. This ionization is shown below for methanoic acid:
HCOOH ⇄ HCOO⁻
+ H⁺
This sort of reaction is an equilibrium reaction. This is why we have the double arrow.
None electrolytes do not ionize at all in aqueous solutions and they produce no ions.
The chemical reaction in which number of atoms of each element present in the reactant side is equal to the number of atoms of that element in product side, such reactions are said to be a balanced chemical reaction.
The chemical symbol for sodium is .
The chemical symbol for fluorine gas is .
The chemical symbol for sodium fluoride is
The sodium fluoride is prepared from the reaction between sodium metal and fluorine gas can be written as:
The above reaction is not balanced as the number of fluorine atoms are not same on reactant and product side. So, in order to balance the reaction we will multiply with 2 on reactant side and
with 2 on product side. Thus, the balanced reaction will be:
Thus, the balanced chemical equation is .
Answer:
The balanced half-reaction for the reduction of dichromate ion to chromium ion in acidic aqueous solution:
Explanation:
The reaction :
Balancing of reaction in an acidic medium:
Step 1: Balance the atoms in the reaction:
Step 2: Balance oxygen atom by adding water on the side where no oxygen or less oxygen atom is present;
Step 3: Balance the hydrogen atom by adding hydrogen ions on the side where water is absent:
Step 4: Now balance charge by adding electrons on the side where more positive charge is present
The balanced half-reaction for the reduction of dichromate ion to chromium ion in acidic aqueous solution: