Answer:
This question is incomplete
Explanation:
This question is incomplete but what you should know is that isopropanol (also referred to rubbing alcohol) has just one functional group. This functional group is called the hydroxyl group (-OH) and it's the reason the compound name ends with "ol". The hydroxyl group can be seen in the structure of the compound (Isopropanol) below
H OH H
| | |
H- C - C - C - H
| | |
H H H
If there is any functional group in isopropanol required for any form of interaction, that functional group will be the hydroxyl group because that's the only functional group isopropanol has.
NOTE: Functional group is an atom or group of atoms that determines the chemical properties of a compound.
Using pv=nRT
T= 22+273 K
P=1.15 Pa
R=8.31
V =5.5... (u did not write the unit so...)
Therefore n,mole= (1.15×5.5) ÷ (273+22)(8.31)
Answer:
Mass = 5.33 g
Explanation:
Given data:
Mass of Al = 2.80 g
Mass of Cl₂ = 4.15 g
Theoretical yield of AlCl₃ = ?
Solution:
Chemical equation:
2Al + 3Cl₂ → 2AlCl₃
Number of moles of Al:
Number of moles = mass/molar mass
Number of moles = 2.80 g/ 27 g/mol
Number of moles = 0.10 mol
Number of moles of Cl₂:
Number of moles = mass/molar mass
Number of moles = 4.15 g/71 g/mol
Number of moles = 0.06 mol
Now we will compare the moles of AlCl₃ with Al and Cl₂.
Cl₂ : AlCl₃
3 : 2
0.06 : 2/3×0.06 = 0.04
Al : AlCl₃
2 : 2
0.10 : 0.10
Number of moles of AlCl₃ produced by chlorine are less so it will be limiting reactant.
Mass of AlCl₃:Theoretical yield
Mass = number of moles ×molar mass
Mass = 0.04 mol × 133.34 g/mol
Mass = 5.33 g
The oxidation state of potassium ion K = +1
The oxidation state of oxygen ion O = -2
So, the oxidation state of O2 is = -2 x 2 = -4
Since, KBrO2 is neutral so,
(+1) + (x) + (-4) = Zero
-3 + X = Zero
So, X = +3
The oxidation state of individual bromine atom in KBrO2 is +3
Answer: The actual yield of 
is 60.0 g
Explanation:-
The balanced chemical reaction :
Mass of 
=
According to stoichiometry:
1 mole of gives = 1 mole of
1.51 moles of gives =
moles of
Theoretical yield of 
Percent yield of = 
Thus the actual yield of is 60.0 g
