Question

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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Answer 1

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

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:

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

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

According to stoichiometry :

1 mole of $CoF2$ require = 1 mole of $F_2$

Thus 3.000 moles of $CoF_2$ will require=$\frac{1}{1}\times 3.000=3.000moles$  of $F_2$

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