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anyanavicka [17]
3 years ago
9

When 2.94 g of a metal combined with fluorine gas, 7.47 g of a metal fluoride formed. Given this information, calculate the mass

%F in the metal fluoride that formed.
Chemistry
1 answer:
Nutka1998 [239]3 years ago
7 0

 The mass % F  in  the metal fluoride that is formed is  60.64%


 <u><em>calculation</em></u>

Step 1:  calculate the mass  of fluorine (F)

mass  of F =  mass  of  metal fluoride  -  mass of the metal

     = 7.47 g - 2.94 g= 4.53 g

Step 2:  calculate  the  % mass of F

Mass % of  F =  mass  of F / mass  of metal  fluoride  x 100

mass % of F  is therefore  =  4.53  g/ 7.47  x 100 = 60.64%

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3 years ago
What are the names of the following three compounds (see attached)
balu736 [363]

Answer:

1. 4-ethyl-1-heptene

2. 6-ethyl-2-octene

3. 1-butyne

Explanation:

The compounds are named according to IUPAC rules.

Compound 1:

  • Identify the longest carbon chain. This chain is called the parent chain.
  • Identify all of the substituents (groups appending from the parent chain).
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  • The double bond between C1 and C2, so take no. 1 and add the suffix ene to hept "1-heptene".
  • The ethyl group is the alkyl substituent on position 4.
  • So the name is 4-ethyl-1-heptene.

Compound 2:

  • Identify the longest carbon chain. This chain is called the parent chain.
  • Identify all of the substituents (groups appending from the parent chain).
  • The parent chain is numbered so that the multiple bonds have the lowest numbers (double has the priority over alkyl substituents).
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  • The double bond between C2 and C3, so take no. 2 and add the suffix ene to oct "2-octene".
  • The ethyl group is the alkyl substituent on position 6.
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  • Identify the longest carbon chain. This chain is called the parent chain.
  • Identify all of the substituents (groups appending from the parent chain), there is no substituents.
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7 0
2 years ago
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5 0
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One of relatively few reactions that takes place directly between two solids at room temperature is <img src="https://tex.z-dn.n
kolbaska11 [484]

Answer:

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b) 3.14g must be added

Explanation:

a) For the reaction:

Ba(OH)₂.8H₂O(s) + NH₄SCN(s) → Ba(SCN)₂(s) + H₂O(l) + NH₃(g)

As you see, there are 8 moles of water in reactants and 2 moles of oxygen in octahydrate, thus, water moles must be 10:

Ba(OH)₂.8H₂O(s) + NH₄SCN(s) → Ba(SCN)₂(s) +<em>10</em> H₂O(l) + NH₃(g)

To balance hydrogens, the other coefficients are:

Ba(OH)₂.8H₂O(s) + <em>2 </em>NH₄SCN(s) → Ba(SCN)₂(s) +<em>10</em> H₂O(l) + <em>2</em> NH₃(g)

b) As you see in the balanced reaction, 1 mole of barium hydroxide octahydrate reacts with 2 moles of NH₄SCN. 6.5g of Ba(OH)₂.8H₂O are:

6.5 g × (1mol / 315.48g) =<em> 0.0206moles of  Ba(OH)₂.8H₂O</em>. Thus, moles of NH₄SCN that must be used for a complete reaction are:

0.0206moles of  Ba(OH)₂.8H₂O × ( 2 mol NH₄SCN / 1 mol Ba(OH)₂.8H₂O) = <em>0.0412moles of NH₄SCN</em>. In grams:

0.0412moles of NH₄SCN × ( 76.12g / 1mol) = <em>3.14g must be added</em>

8 0
3 years ago
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