Here is your answer
Since, carbon atoms are triple bonded.
So functional group present in the compound is ALKYNE
HOPE IT IS USEFUL
Answer:
35.9 ml
Explanation:
Start with the balanced equation:
3CuCl2(aq)+2Na3PO4(aq)→Cu3(PO4)2(s)+6NaCl(aq)
This tells us that 3 moles of CuCI2 react with 2 moles Na3PO4-
∴ 1 mole CuCl2 will react with 2/3 moles Na3PO4
We know that concentration = moles/volume i.e:
c= n/v
∴n=c×v
∴nCuCl2=0.107×91.01000=9.737×10−3
I divided by 1000 to convert ml to L
∴nNa3PO4=9.737×10−3×23=6.491×10−3
v=nc=6.491×10−30.181=35.86×10−3L
∴v=35.86ml
Answer:
Reduction
Explanation:
The oxidation reduction reactions are called redox reaction. These reactions are take place by gaining or losing the electrons and oxidation state of elements are changed.
Oxidation:
Oxidation involve the removal of electrons and oxidation state of atom of an element is increased.
Reduction:
Reduction involve the gain of electron and oxidation number is decreased.
In given reaction fluorine gas gain two electron and form fluoride ions.
F₂(g) + 2e⁻ → 2F⁻(aq)
The given reaction is reduction because oxidation state is decreased from zero to -1.
Answer:
If a sample of 2 moles of nitric oxide gas was reacted with excess oxygen, 2 moles of nitrogen dioxide would be produced.
Explanation:
The balanced reaction is:
2 NO + O₂ → 2 NO₂
By stoichiometry of the reaction (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of each compound participate in the reaction:
-
NO: 2 moles
- O₂: 1 mole
- NO₂: 2 moles
The limiting reagent is one that is consumed first in its entirety, determining the amount of product in the reaction. When the limiting reagent is finished, the chemical reaction will stop.
The limiting reagent is one that is consumed first in its entirety, determining the amount of product in the reaction. When the limiting reagent is finished, the chemical reaction will stop. By reaction stoichiometry, <u><em>
if a sample of 2 moles of nitric oxide gas was reacted with excess oxygen, 2 moles of nitrogen dioxide would be produced.
</em></u>
<u><em></em></u>
