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Nookie1986 [14]
3 years ago
12

How many moles of nitrogen trifluoride (NF3) can be produced from 9.65 mole of Fluorine gas (F2)

Chemistry
1 answer:
user100 [1]3 years ago
4 0

Answer:

6.43 moles of NF₃.

Explanation:

The balanced equation for the reaction is given below:

N₂ + 3F₂ —> 2NF₃

From the balanced equation above,

3 moles of F₂ reacted to produce 2 moles of NF₃.

Finally, we shall determine the number of mole of nitrogen trifluoride (NF₃) produced by the reaction of 9.65 moles of Fluorine gas (F₂). This can be obtained as follow:

From the balanced equation above,

3 moles of F₂ reacted to produce 2 moles of NF₃.

Therefore, 9.65 moles of F₂ will react to to produce = (9.65 × 2)/3 = 6.43 moles of NF₃.

Thus, 6.43 moles of NF₃ were obtained from the reaction.

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You combine 13 g of magnesium with 5 g of nitrogen to form a compound.
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Answer:

\large \boxed{28 \, \% }

Explanation:

magnesium  + nitrogen ⟶ Product

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Mass of product = 13 g + 5 g = 18 g

The product contains 5 g of nitrogen .

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7 0
3 years ago
What is the volume of 13.21 g of ethane gas (C2H6) at STP?
yuradex [85]

The volume at STP : 9.856 L

<h3>Further explanation</h3>

Given

Mass of ethane : 13.21 g

Required

The volume at STP

Solution

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Volume at STP :

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6 0
3 years ago
If you had an object with a mass of 76g and a volume of 22 ml, what is its density? If you cut this object in half, what would b
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Answer:

The halogens are extremely reactive, whilst the noble gases are mainly inert.

Only some noble gases tend to form compounds, such as xenon and krypton. However, some like helium, almost have no compounds at all. Noble gases also have octet rule shells, which causes the little reactivity associated with them. To form bonds with noble gases, a lot of energy is required to form those bonds. Halogens, on the other hand, are extremely reactive. Compounds like chlorine and fluorine must be stored carefully, as they will oxidise anything that they can find, just to get one extra electron to get an octet configuration.


Hope this helps :)

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3 years ago
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