Solving Unknown Metal Moles in Chemistry Exam

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Discussion Overview

The discussion revolves around a chemistry exam question involving the reaction of an unknown metal with fluorine to form a compound. Participants explore how to determine the moles of fluorine in the compound, the mass of the metal, and the identity of the metal itself. The scope includes chemical equations and stoichiometry.

Discussion Character

  • Homework-related
  • Mathematical reasoning
  • Technical explanation

Main Points Raised

  • One participant presents a question regarding the reaction of 0.600 mol of metal M with excess fluorine to form 46.8 g of MF2.
  • Another participant proposes a balanced chemical equation: M + F2 -> MF2.
  • One participant suggests that there would be 1.2 mol of F in the compound, based on the stoichiometry of the balanced equation.
  • A later reply confirms the previous claim about the moles of F.

Areas of Agreement / Disagreement

Participants generally agree on the balanced equation and the calculation of moles of fluorine, but the identity of the metal and the mass of the metal remain unaddressed and unresolved.

Contextual Notes

There are assumptions regarding the balanced equation and the calculations involved, which depend on the correct interpretation of the problem and the stoichiometry of the reaction.

bjr_jyd15
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here's a question from my recent chem exam that i don't know how to approach:

a sample of 0.600 mol of a metal M reacts completely with excess fluorine to form 46.8 g MF2

a) how many moles of F are in the sample of the compound that forms?

b) how many grams of M are in this sample of MF2?

c) what element is represented by the symbol M?

i started to try to write a balanced equation for this but I'm not sure if the coeffecients would be right...

any help? thanks!
 
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the balanced equation is just going to be M + F2 -> MF2
 
so there would be 1.2 mol of F in the compound right
 
Yep.
 

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