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bagirrra123 [75]
3 years ago
12

What is the mole ratio needed to determine the mass of phosphorus trifluoride produced from the reaction of 120 g of phosphorus

with excess fluorine?

Chemistry
1 answer:
Vitek1552 [10]3 years ago
8 0

Answer:

\frac{4molPF_3}{1molP_4}

Explanation:

Hello

In this case, given the reaction:

P_4(s)+6F_2(g)\rightarrow 4PF_3(g)

It means that since the coefficients preceding phosphorous and phosphorous trifluoride are 1 and 4, the correct mole ratio should be:

\frac{4molPF_3}{1molP_4}

Because given the mass of phosphorous it is convenient to convert it to moles and then cancel it out with the moles on bottom of the mole ratio.

Bes regards!

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              # of Moles  =  Number of Atoms / 6.022 × 10²³
Or,
             Number of Atoms  =  Moles × 6.022 × 10²³     ------- (1)    

Calculating Moles,
As,
                              Moles  =  Mass / M.mass
So,
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Putting value of mole in eq.1,

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Result:
            4.25 g 
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