Chemistry Solving Unknown Metal Moles in Chemistry Exam

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To solve the chemistry exam question, the balanced equation for the reaction is M + F2 -> MF2. Given that 0.600 mol of metal M reacts with excess fluorine, the formation of 46.8 g of MF2 indicates that there are 1.2 moles of fluorine (F) in the compound. The mass of M in MF2 can be calculated using the molar mass of MF2, which leads to determining the identity of metal M. The calculations confirm that the coefficients in the balanced equation are correct, and the problem can be resolved with these steps. Understanding stoichiometry is crucial for solving such chemistry problems effectively.
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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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