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Crank
3 years ago
15

CaF2 + (NH4)2O --> 2 NH4F + CaO How many grams of NH4F can be formed from 34.6 grams of CaF2? (AKS 4f)

Chemistry
1 answer:
bixtya [17]3 years ago
5 0

Answer:

32.83 grams of NH₄F can be formed from 34.6 grams of CaF₂

Explanation:

The balanced reaction is:

CaF₂ + (NH₄)₂O ⇒ 2 NH₄F + CaO

By stoichiometry of the reaction (that is, the relationship between the amount of reagents and products in a chemical reaction), the following quantities participate in the reaction:

  • CaF₂: 1 mole
  • (NH₄)₂O: 1 mole
  • NH₄F: 2 mole
  • CaO: 1 mole

Being the molar mass of the compounds:

  • CaF₂: 78 g/mole
  • (NH₄)₂O: 52 g/mole
  • NH₄F: 37 g/mole
  • CaO: 56 g/mole

Then by stoichiometry, the following amounts of mass participate in the reaction:

  • CaF₂: 1 mole* 78 g/mole= 78 g
  • (NH₄)₂O: 1 mole* 52 g/mole= 52 g
  • NH₄F: 2 mole* 37 g/mole= 74 g
  • CaO: 1 mole* 56 g/mole= 56 g

You can apply the following rule of three: if 78 grams of CaF₂ form 74 grams of NH₄F by stoichiometry, 34.6 grams of CaF₂ will form how much mass of NH₄F?

mass of NH_{4} F=\frac{34.6 grams of CaF_{2} *74 grams ofNH_{4} F}{78grams of CaF_{2} }

mass of NH₄F= 32.83 grams

<u><em>32.83 grams of NH₄F can be formed from 34.6 grams of CaF₂</em></u>

<u><em></em></u>

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What is the percentage of s-character in an sp hybrid? O 25% 50% o 75% O 66%
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Explanation:

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Need help on last 3 questions
Olin [163]

Answer:

Explanation:

1)

Given data:

Initial volume of balloon = 0.8 L

Initial temperature = 12°C ( 12+273= 285 K)

Final temperature = 300°C (300+273 = 573 K)

Final volume = ?

Solution:

V₁/T₁ = V₂/T₂

V₂ = V₁T₂/T₁  

V₂ = 0.8 L .573 K / 285 K

V₂ = 458.4 L / 285

V₂ = 1.61 L

2)

Initial pressure = 204 kpa

Initial temperature = 29°C ( 29 + 273 = 302 K)

Final temperature = ?

Final pressure = 300 kpa

Solution:

P₁/T₁ = P₂/T₂

T₂ = T₁P₂/P₁  

T₂ = 302 K . 300 kpa / 204 kpa

T₂ = 90600 K/ 204

T₂ = 444.12 K

3)

Given data:

Initial volume = 14 L

Initial pressure = 2.1 atm

Initial temperature = 100 K

Final temperature = 450 K

Final volume = ?

Final pressure = 1.2 atm

Formula:  

P₁V₁/T₁ = P₂V₂/T₂  

P₁ = Initial pressure

V₁ = Initial volume

T₁ = Initial temperature

P₂ = Final pressure

V₂ = Final volume

T₂ = Final temperature

Solution:

V₂ = P₁V₁ T₂/ T₁ P₂  

V₂ = 2.1 atm × 14 L × 450 K / 100 K × 1.2 atm  

V₂ = 13230 L / 120

V₂ = 110.25 L

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