Let the formula of dark red compound be of the form PtFx (where x is the number of fluorine attached with each Pt)
Molar mass of Pt = 195 g/mol
Molar mass of F = 19 g/mol
Number of moles of Pt = Mass/Molar mass = 0.266/195
This must be equal to number of moles of product formed
Moles of Product formed = (mass)/(molar mass) = 0.422/(195+19x)
Solving the equation for x we get
0.266/195 = 0.422/(195+19x)
195 + 19x = 309.36
19x = 114.36
x = 114/19 = (approximately equal to 6)
Hence the empirical formula of the compound will be PtF6
Note - Post any doubts/queries in comments section.
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