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4. Cobalt(II) chloride reacts with fluorine in a single replacement reaction to produce

cobalt(II) fluoride and chlorine gas.

Balanced Equation:

+

How many moles of fluorine are required to produce 290.8 g of cobalt(II) fluoride?

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User Misterzik
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1 Answer

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13 votes

Answer:
CoCl_2+F_2\rightarrow CoF_2+Cl_2

3.000 moles of flourine are required to produce 290.8 g of cobalt(II) fluoride

Step-by-step explanation:

A single replacement reaction is one in which a more reactive element displaces a less reactive element from its salt solution.

When cobalt chloride is added to flourine, chlorine being more reactive than flourine, displaces chlorine atom its salt solution and lead to formation of cobalt flouride and chlorine gas.


CoCl_2+F_2\rightarrow CoF_2+Cl_2

To calculate the number of moles, we use the equation:


\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}


\text{Number of moles of cobalt flouride}=(290.8g)/(96.93g/mol)=3.000mol

According to stoichiometry :

1 mole of
CoF2 require = 1 mole of
F_2

Thus 3.000 moles of
CoF_2 will require=
(1)/(1)* 3.000=3.000moles of
F_2

Thus 3.000 moles of flourine are required to produce 290.8 g of cobalt(II) fluoride

User Mattias Nordberg
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