Answer:
86.04 %
Explanation:
Data given:
mass of Al = 160.0 g
actual yield Al₂O₃= 260 g
Theoretical yield = ?
percent yield ofAl₂O₃ = ?
Solution:
First we have to find theoretical yield.
So,
we Look at the balanced reaction
4Al + 3O₂ -----—> 2Al₂O₃
4 mol 2 mol
As 4 mole of Al give 2 mole of Al₂O₃
Convert moles to mass
molar mass of Al = 27 g/mol
molar mass of Al₂O₃ = 2(27) + 3(16)
molar mass of Al₂O₃ = 54 + 48
molar mass of Al₂O₃ = 102 g/mol
Now
4Al + 3O₂ -----—> 2Al₂O₃
4 mol (27g/mol) 2 mol (102 g/mol)
108 g 204 g
108 grams of Al produce 204 g of Al₂O₃
So
if 108 grams of Al produce 204 g of Al₂O₃ so how many grams of Al₂O₃will be produced by 160 g of Al.
Apply Unity Formula
108 grams of Al ≅ 204 g of Al₂O₃
160 grams of Al ≅ X of Al₂O₃
Do cross multiply
mass of Al₂O₃= 204 g x 160 g / 108 g
mass of Al₂O₃ = 302.2 g
So the Theoretical yield of Al₂O₃ = 302.2 g
Now Find the percent yield of Al₂O₃
Formula Used
percent yield = actual yield /theoretical yield x 100 %
Put value in the above formula
percent yield = 260g / 302.2 g x 100 %
percent yield = 86.04 %
percent yield of Al₂O₃ = 86.04 %
b.an atom is solid material
c.electrons have a negative charge
d.electrons are arranged in layers
Answer:
The answer is A
Explanation:
Answer:The pure substance within chemistry is a very simple concept to grasp. Pure substances are defined as substances that are made of only one type of atom or only one type of molecule (a group of atoms bonded together). ... Purity can also have an important impact on the chemical properties of a substance.
Explanation:
The mole concept can be used to determine the number of ozone molecules are lost in the atmosphere.
The mole concept was introduced by Avogadro. The mole is the SI unit of amount of substance. According to Avogadro, one mole of a substance contains 6.02 × 10^23 atoms, ions, molecules etc. The mole concept is important in many chemical calculations. The quantity amount of substance is a measure of how many elementary entities of a given substance are in an object or sample.
To learn more about mole,refer here :
#SPJ2
Answer:
determining how many ozone molecules are lost in the atmosphere
Answer:
decomposistion,single replacement,double replacement,and sythesis
Explanation:
nmnbmm
Answer:
0.172 mol·L⁻¹
Step-by-step explanation:
1. Write the chemical equation for the reaction.
HBr + LiOH ⟶ LiBr + H₂O
===============
2. Calculate the moles of LiOH
c = n/V Multiply each side by V
n = Vc
V = 0.0375 L
c = 0.215 mol·L⁻¹
Moles of LiOH = 0.0375× 0.215
Moles of LiOH = 8.062 × 10⁻³ mol LiOH
===============
3. Calculate the moles of HBr
1 mol HBr ≡ 1 mol LiOH
Moles of HBr = 8.062 × 10⁻³× 1/1
Moles of HBr = 8.062 × 10⁻³ mol HBr
===============
4. Calculate the molar concentration of the HBr
V = 47.0 mL = 0.0470 L
c = 8.062 × 10⁻³/0.0470
c = 0.172 mol·L⁻¹
The molarity of the HBr solution is 0,172 M.
The neutralization reaction between LiOH and HBr is the following:
HBr(aq) + LiOH(aq) → LiBr(aq) + H₂O(l)